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COMPLETE FULL COURSE STRAIGHTERLINE CHEM 101 - GENERAL CHEMISTRY 1, 2, 3 , 4, 5 & 6 - APRIL 2022
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 1 - APRIL 2022
• CHEM101_MH_V4 • Topic 3: Stoichiometry Started on Friday, April 15, 2022, 7:00 PM State Finished Completed on Friday, April 15, 2022, 7:25 PM Ti... [Show More] me taken 25 mins 47 secs Grade 115.00 out of 115.00 (100%) Feedback You’re off to a good start. A course grade of 70% is required to request a transcript. You’ve met that for the first exam already, but if you want to reattempt for a higher grade you can retake this assessment. Study hard for each exam, and consider using tutoring anytime you get stuck. Remember that 10 hours of tutoring are provided to you through your StraighterLine membership. Question 1 Correct 4.60 points out of 4.60 Flag question Question text Which of the following cannot be separated into simpler substances by chemical means? Select one: a. Element b. Emulsion c. Compound d. Homogeneous mixture e. Heterogeneous mixture Question 2 Correct 4.60 points out of 4.60 Flag question Question text What is a unifying principle that explains a body of experimental observations? Select one: a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a chemical change? Select one: a. Boiling water b. Melting wax c. Broiling a steak on a grill d. Condensing water vapor into rainfall e. Carving a piece of wood Question 4 Correct 4.60 points out of 4.60 Flag question Question text If a liquid contains 60% sugar and 40% water throughout its composition then what is it called? Select one: a. Solute b. Compound c. Homogeneous mixture d. Heterogeneous mixture e. Solvent Question 5 Correct 4.60 points out of 4.60 Flag question Question text Which one of these represents a physical change? Select one: a. Water, when heated, forms steam. b. Bleach turns hair yellow. c. Sugar, when heated, becomes brown. d. Milk turns sour. e. Apples, when exposed to air, turn brown. Question 6 Correct 4.60 points out of 4.60 Flag question Question text The dark meat of a 20-pound turkey requires an internal temperature of 180°F to be fully cooked. What minimum temperature reading should be displayed on a food thermometer that only measures in degrees Celsius? Select one: a. 82°C b. 354°C c. 261°C d. –192°C e. –310°C Question 7 Correct 4.60 points out of 4.60 Flag question Question text Which is correct if 52.068881 is rewritten in scientific notation and rounded to three significant figures? Select one: a. 5.21 × 10–1 b. 5.20 × 10–1 c. 5.21 × 101 d. 5.20 × 101 e. 5.21 × 102 Question 8 Correct 4.60 points out of 4.60 Flag question Question text How many significant figures are in 0.006570? Select one: a. 3 b. 4 c. 5 d. 6 e. 7 Question 9 Correct 4.60 points out of 4.60 Flag question Question text What element is represented by X in the atomic symbol notation ? Select one: a. Iridium b. Platinum c. Palladium d. Selenium e. Magnesium Question 10 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a metalloid? Select one: a. Carbon, C, Z = 6 b. Sulfur, S, Z = 16 c. Germanium, Ge, Z = 32 d. Iridium, Ir, Z = 77 e. Bromine, Br, Z = 35 Question 11 Correct 4.60 points out of 4.60 Flag question Question text The elements in Group 7A are known by what name? Select one: a. Transition metals b. Halogens c. Alkali metals d. Alkaline earth metals e. Noble gases Question 12 Correct 4.60 points out of 4.60 Flag question Question text Which of these materials are usually poor conductors of heat and electricity? Select one: a. Metals b. Metalloids c. Nonmetals d. Alkaline earth metals e. Alkali metals Question 13 Correct 4.60 points out of 4.60 Flag question Question text The scientist who determined the magnitude of the electric charge on the electron was Select one: a. John Dalton b. Robert Millikan c. J. J. Thomson d. Henry Moseley e. J. Burdge Question 14 Correct 4.60 points out of 4.60 Flag question Question text Which of these compounds is most likely to be ionic? Select one: a. KF b. CCl4 c. CS2 d. CO2 e. ICl Question 15 Correct 4.60 points out of 4.60 Flag question Question text The compound, P4S10, is used in the manufacture of safety matches. What is its name? Select one: a. phosphorus sulfide b. phosphoric sulfide c. phosphorus decasulfide d. tetraphosphorus decasulfide e. phosphorus sulfite Question 16 Correct 4.60 points out of 4.60 Flag question Question text Which one of these species is an ion? Select one: a. B3+ b. NaCl c. He d. 14C e. None of these species is an ion. Question 17 Correct 4.60 points out of 4.60 Flag question Question text What is the formula for the permanganate ion? Select one: a. MnO2– b. MnO4– c. MgO42– d. Mn2O7– e. MgO22– Question 18 Correct 4.60 points out of 4.60 Flag question Question text Calculate the mass of 3.00 moles of CF2Cl2. Select one: a. 3.00 g b. 174 g c. 363 g d. 1.81 × 1024 g e. 40.3 Question 19 Correct 4.60 points out of 4.60 Flag question Question text How many grams are contained in a 0.183 mol sample of ammonium phosphate? Select one: a. 1.23 × 10–3 g b. 617 g c. 20.7 g d. 27.3 g e. 815.1 g Question 20 Correct 4.60 points out of 4.60 Flag question Question text Which of the following substances contains the greatest mass of carbon? Select one: a. 100 g CH4 b. 100 g C2H4 c. 100 g CCl4 d. 100 g CH2Cl2 e. 100 g CO2 Question 21 Correct 4.60 points out of 4.60 Flag question Question text What is the molar mass of nicotine, C10H14N2? Select one: a. 134 g/mol b. 148 g/mol c. 158 g/mol d. 210 g/mol e. 162 g/mol Question 22 Correct 4.60 points out of 4.60 Flag question Question text Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the coefficients? (Don't forget to include coefficients of one.) ___ CH4 + ___ Cl2 → ___ CCl4 + ___ HCl Select one: a. 4 b. 6 c. 8 d. 10 e. 12 Question 23 Correct 4.60 points out of 4.60 Flag question Question text What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the chemical equation below? 2Al + Cr2O3 → Al2O3 + 2Cr Select one: a. 7.7 g b. 15.4 g c. 27.4 g d. 30.8 g e. 49.9 g Question 24 Correct 4.60 points out of 4.60 Flag question Question text What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers? ___ Al4C3 + ___ H2O → ___ Al(OH)3 + ___ CH4 Select one: a. 3 b. 4 c. 6 d. 12 e. 24 Question 25 Correct 4.60 points out of 4.60 Flag question Question text If 13.9 g of oxygen react with 33.7 g of calcium to produce calcium oxide, what is the limiting reactant and what mass of calcium oxide is produced? Select one: a. Calcium is the limiting reactant and 47.2 g of calcium oxide are produced b. Oxygen is the limiting reactant and 24.4 g of calcium oxide are produced c. Calcium is the limiting reactant and 60.6 g of calcium oxide are produced d. Oxygen is the limiting reactant and 48.7 g of calcium oxide are produced e. Calcium is the limiting reactant and 23.6 g of calcium oxide are produced [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 1 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 3: Stoichiometry Started on Thursday, March 17, 2022, 9:21 AM State Finished Completed on Thursday, March 17, 20... [Show More] 22, 10:39 AM Time taken 1 hour 18 mins Grade 105.80 out of 115.00 (92%) Feedback You’re off to a good start. A course grade of 70% is required to request a transcript. You’ve met that for the first exam already, but if you want to reattempt for a higher grade you can retake this assessment. Study hard for each exam, and consider using tutoring anytime you get stuck. Remember that 10 hours of tutoring are provided to you through your StraighterLine membership. Question 1 Correct 4.60 points out of 4.60 Flag question Question text What is the term used for findings that are summarized based on a pattern or trend? Select one: a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction Question 2 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a tentative explanation for a set of observations? Select one: a. Law b. Hypothesis c. Theory d. Phenomena e. Prediction Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is an extensive property? Select one: a. Density b. Temperature c. Mass d. Specific Heat e. Pressure Question 4 Incorrect 0.00 points out of 4.60 Flag question Question text Which of the following is an extensive property of oxygen? Select one: a. Boiling point b. Temperature c. Average kinetic energy of molecules d. Density e. Mass Question 5 Correct 4.60 points out of 4.60 Flag question Question text Which of these is an example of a physical property? Select one: a. Corrosiveness of sulfuric acid b. Toxicity of cyanide c. Flammability of gasoline d. Neutralization of stomach acid with an antacid e. Lead becomes a liquid when heated to 601°C. Question 6 Correct 4.60 points out of 4.60 Flag question Question text The density of magnesium is 1.7 g/cm3, and the density of iron is 7.9 g/cm3. Consider a block of iron with a mass of 819 g. What is the mass of a block of magnesium that has the same volume as the block of iron? Select one: a. 1.8 x 102 g b. 61 g c. 2.8 x 103 g d. 3.8 x 103 g e. None of the above. Question 7 Correct 4.60 points out of 4.60 Flag question Question text What is the volume of a container that contains 14.3 g of a substance having a density of 0.988 g/cm3? Select one: a. 14.1 cm3 b. 0.0691 cm3 c. 14.5 cm3 d. 141 cm3 e. 691 cm3 Question 8 Correct 4.60 points out of 4.60 Flag question Question text The result of (3.8621 × 1.5630) – 5.98 is properly written as Select one: a. 0.06 b. 0.056 c. 0.0565 d. 0.05646 e. 0.056462 Question 9 Correct 4.60 points out of 4.60 Flag question Question text Atoms of the same element with different mass numbers are called Select one: a. ions. b. neutrons. c. chemical groups. d. chemical families. e. isotopes. Question 10 Correct 4.60 points out of 4.60 Flag question Question text Which of these elements is chemically similar to oxygen? Select one: a. Sulfur b. Calcium c. Iron d. Nickel e. Potassium Question 11 Correct 4.60 points out of 4.60 Flag question Question text Which of these elements is chemically similar to magnesium? Select one: a. Sulfur b. Calcium c. Iron d. Nickel e. Potassium Question 12 Correct 4.60 points out of 4.60 Flag question Question text C(graphite) and C(diamond) are examples of: Select one: a. isotopes of carbon. b. allotropes of carbon. c. the law of definite proportions. d. different carbon ions. Question 13 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a type of radioactive radiation that consists of electrons and is deflected away from the negatively charged plate? Select one: a. α rays b. β rays c. γ rays d. δ rays e. ε rays Question 14 Correct 4.60 points out of 4.60 Flag question Question text What is the name of ClO – ion? Select one: a. hypochlorite b. chlorate c. chlorite d. perchlorate e. perchlorite Question 15 Correct 4.60 points out of 4.60 Flag question Question text What is the formula of iodous acid? Select one: a. HI b. HIO3 c. HIO d. HIO4 e. HIO2 Question 16 Correct 4.60 points out of 4.60 Flag question Question text What is the formula for lead(II) oxide? Select one: a. PbO b. PbO2 c. Pb2O d. PbO4 e. Pb2O3 Question 17 Correct 4.60 points out of 4.60 Flag question Question text Which of these compounds is most likely to be ionic? Select one: a. NCl3 b. BaCl2 c. CO d. SO2 e. SF4 Question 18 Correct 4.60 points out of 4.60 Flag question Question text What is the percent carbon in CH3CH2OH? Select one: a. 13% b. 26% c. 35% d. 46% e. 52% Question 19 Correct 4.60 points out of 4.60 Flag question Question text What is the mass of 0.0250 mol of P2O5? Select one: a. 35.5 g b. 5676 g c. 0.0250 g d. 1.51 × 1022 g e. 3.55 g Question 20 Correct 4.60 points out of 4.60 Flag question Question text What is the mass of 1.63 × 1021 atoms of silicon? (NA = 6.022 × 1023 mol–1) Select one: a. 2.71 × 10–23 g b. 4.58 × 1022 g c. 28.08 g d. 1.04 × 104 g e. 7.60 × 10–2 g Question 21 Incorrect 0.00 points out of 4.60 Flag question Question text What is the percent sulfur in iron(III) sulfate? Select one: a. 28% b. 32% c. 24% d. 48% e. 42% Question 22 Correct 4.60 points out of 4.60 Flag question Question text Which is a representation of a balanced chemical equation for the reaction of nitrogen gas and chlorine gas to form nitrogen trichloride? Select one: a. b. c. d. e. Question 23 Correct 4.60 points out of 4.60 Flag question Question text Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the coefficients? (Don't forget to include coefficients of one.) ___ Cr + ___ H2SO4 → ___ Cr2(SO4)3 + ___ H2 Select one: a. 4 b. 9 c. 11 d. 13 e. 15 Question 24 Correct 4.60 points out of 4.60 Flag question Question text Once the following equation is balanced with the smallest set of whole number coefficients, what is the sum of the coefficients? (Don't forget to include coefficients of one.) ___ Al + ___ H2SO4 → ___ Al2(SO4)3 + ___ H2 Select one: a. 3 b. 5 c. 6 d. 9 e. 12 Question 25 Correct 4.60 points out of 4.60 Flag question Question text The first step in the Ostwald process for producing nitric acid is as follows: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g). If the reaction of 15.0 g of ammonia with 15.0 g of oxygen gas yields 8.70 g of nitric oxide, what is the percent yield of this reaction? Select one: a. 29.0% b. 32.9% c. 49.5% d. 61.8% e. 77.3% [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 2 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 6: Quantum Theory Started on Friday, April 15, 2022, 7:28 PM State Finished Completed on Friday, April 15, 2022,... [Show More] 7:50 PM Time taken 21 mins 36 secs Grade 115.00 out of 115.00 (100%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text A 0.8838-g sample of an ionic compound containing bromide ions and an unknown metal cation is dissolved in water and treated with an excess of AgNO3. If 1.573 g of a AgBr precipitate forms, what is the percent by mass of Br in the original compound? Select one: a. 62.13% b. 75.72% c. 56.19% d. 42.55% e. 37.87% Question 2 Correct 4.60 points out of 4.60 Flag question Question text Based on the solubility rules, which one of these compounds is soluble in water? Select one: a. CaSO4 b. BaSO4 c. PbSO4 d. K2SO4 e. Ag2SO4 Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a weak acid? Select one: a. H2SO4 b. HNO3 c. HF d. HBr e. HCl Question 4 Correct 4.60 points out of 4.60 Flag question Question text Which is a strong acid? Select one: a. Ba(OH)2 b. H3PO4 c. HC2H3O2 d. NaCl e. HClO4 Question 5 Correct 4.60 points out of 4.60 Flag question Question text What is the oxidizing agent in the following reaction? 5Fe2+(aq) + MnO4–(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) Select one: a. Fe2+ b. MnO4– c. H+ d. Mn2+ e. Fe3+ Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which is a correct description of the following reaction? H2SO4 + Cd(OH)2 → 2H2O + CdSO4 Select one: a. This reaction is an acid-base reaction. b. In this reaction, hydrogen is oxidized. c. In this reaction, sulfur is oxidized. d. In this reaction, cadmium is oxidized. e. In this reaction, oxygen is oxidized. Question 7 Correct 4.60 points out of 4.60 Flag question Question text Balance the following oxidation-reduction equation: Li(s) + O2(g) → Li2O(s) Select one: a. 2Li(s) + O2(g) → Li2O(s) b. Li(s) + O2(g) → Li2O(s) c. 4Li(s) + O2(g) → 2Li2O(s) d. 2Li(s) + O2(g) → 2Li2O(s) e. 2Li(s) + O2(g) → 4Li2O(s) Question 8 Correct 4.60 points out of 4.60 Flag question Question text What is the reducing agent in the following reaction? 5Fe2+(aq) + MnO4–(aq) + 8H+(aq) → 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) Select one: a. Fe2+ b. MnO4– c. H+ d. Mn2+ e. Fe3+ Question 9 Correct 4.60 points out of 4.60 Flag question Question text For the reaction depicted below, if Z represents Zn, which metal could A represent? Select one: a. Fe b. Co c. Pb d. Ca e. Cu Question 10 Correct 4.60 points out of 4.60 Flag question Question text Aluminum oxide can be reduced to aluminum metal using carbon, the other reaction product being carbon monoxide. What is the enthalpy change if 12.50 g of aluminum is produced by this method? Substance ΔH°f(kJ/mol) CO(g) –110.5 Al2O3(s) –1669.8 Select one: a. 310.0 kJ b. 386.8 kJ c. 412.4 kJ d. 773.6 kJ e. 824.8 kJ Question 11 Correct 4.60 points out of 4.60 Flag question Question text How much heat is required to raise the temperature of 22.8 g of copper from 20.0°C to 875.0°C? The specific heat of copper is 0.385 J/g·°C. Select one: a. 14.4 J b. 176 J c. 7.51 kJ d. 7.68 kJ e. 9.90 kJ Question 12 Correct 4.60 points out of 4.60 Flag question Question text Ethylene glycol, used as a coolant in automotive engines, has a specific heat capacity of 2.42 J/g°C. Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C. Select one: a. –1900 kJ b. –420 kJ c. –99 kJ d. –0.42 kJ e. –4.2 × 10–6 kJ Question 13 Correct 4.60 points out of 4.60 Flag question Question text Which equation has a ΔHrxn that is not equal to ΔHof of the product? Select one: a. O2(g) + H2(g) → H2O2(g) b. ½O2(g) + H2(g) → H2O(g) c. H2(g) + ½O2(g) + → H2O(l) d. NO(g) + ½O2(g) → NO2(l) e. ½H2(g) + ½Cl2(g) → HCl(g) Question 14 Correct 4.60 points out of 4.60 Flag question Question text An exothermic reaction causes the surroundings to Select one: a. warm up. b. become acidic. c. expand. d. decrease its temperature. e. release CO2. Question 15 Correct 4.60 points out of 4.60 Flag question Question text Which represents an enthalpy change at 25 °C and 1 atm that is equal to ΔHof for H2O(l)? Select one: a. O2(g) + 2H2(g) → 2H2O(l) b. ½O2(g) + H (g) → H2O(g) c. H2(g) + ½O2(g) → H2O(l) d. 2H2O(l) → O2(g) + 2H2(g) e. H2O(l) → ½O2(g) + H2(g) Question 16 Correct 4.60 points out of 4.60 Flag question Question text An ideal gas (the system) is contained in a flexible balloon at a pressure of 1 atm and is initially at a temperature of 20.°C. The surrounding air is at the same pressure, but its temperature is 25°C. When the system has equilibrated with its surroundings, both system and surroundings are at 25°C and 1 atm. In changing from the initial to the final state, which one of the following relationships regarding the system is correct? Select one: a. ΔU < 0 b. ΔU = 0 c. ΔH = 0 d. w > 0 e. q > 0 Question 17 Correct 4.60 points out of 4.60 Flag question Question text How much heat is released if 7.15 g CaO(s) is added to 152 g of H2O(l)? CaO(s) + H2O(l) → Ca(OH)2(s) ΔH°rxn = –64.8 kJ/mol Select one: a. 7.68 kJ b. 8.26 kJ c. 508 kJ d. 547 kJ e. 555 kJ Question 18 Correct 4.60 points out of 4.60 Flag question Question text The solar radiation spectrum peaks at a wavelength of approximately 500 nm. Calculate the energy of one photon of that radiation (c = 3.00 × 108 m/s; h = 6.63 × 10–34 J • s). Select one: a. 4 × 10–10 J b. 6 × 1014 J c. 1 × 10–27 J d. 2 × 10–25 J e. 4 × 10–19 J Question 19 Correct 4.60 points out of 4.60 Flag question Question text Which element has the following ground-state electron configuration? [Kr]5s24d105p2 Select one: a. Sn b. Sb c. Pb d. Ge e. Te Question 20 Correct 4.60 points out of 4.60 Flag question Question text The unusual electron configuration of Mo indicates the Select one: a. unusual stability of half-filled d-orbitals. b. unpredictability of the electron filling patterns of the non-representative elements. c. unusually large size of Mo atoms. d. greater than expected electronegativity of Mo. Question 21 Correct 4.60 points out of 4.60 Flag question Question text Select the arrangement of electromagnetic radiation which starts with the shortest wavelength and increases to longest wavelength. Select one: a. radio, infrared, ultraviolet, gamma rays b. radio, ultraviolet, infrared, gamma rays c. gamma rays, radio, ultraviolet, infrared d. gamma rays, infrared, radio, ultraviolet e. gamma rays, ultraviolet, infrared, radio Question 22 Correct 4.60 points out of 4.60 Flag question Question text Which ground-state atom has an electron configuration described by the following orbital diagram? [Ar] ↿⇂ ↿⇂ ↿⇂ ↿⇂ ↿⇂ ↿⇂ ↿⇂ ↿ ↿ 4s 3d 4p Select one: a. phosphorus b. germanium c. selenium d. tellurium e. potassium Question 23 Correct 4.60 points out of 4.60 Flag question Question text Which element has the following ground-state electron configuration? 1s2 2s2 2p6 3s2 Select one: a. Na b. Mg c. Al d. Si e. Ne Question 24 Correct 4.60 points out of 4.60 Flag question Question text The FM station KDUL broadcasts music at 99.1 MHz. Find the wavelength of these waves. (c = 3.00 × 108 m/s) Select one: a. 1.88 × 10–2 m b. 0.330 m c. 3.03 m d. 5.33 × 102 m e. > 103 m Question 25 Correct 4.60 points out of 4.60 Flag question Question text Which scientist proposed that energy of radiation is composed of extremely small indivisible packages called quanta? (“Quanta” is the plural of “quantum.”) Select one: a. Max Planck b. Louis de Broglie c. Clinton Davisson d. Sir Isaac Newton e. Lothan Meyer [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 2 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 6: Quantum Theory Started on Monday, March 28, 2022, 10:23 AM State Finished Completed on Monday, March 28, 2022... [Show More] , 11:01 AM Time taken 38 mins 28 secs Grade 101.20 out of 115.00 (88%) Question 1 Incorrect 0.00 points out of 4.60 Flag question Question text Which accurately characterizes all nonelectrolyte solutions? Select one: a. Nonelectrolyte solutions contain molecules. b. Nonelectrolyte solutions conduct electricity. c. Nonelectrolyte solutions react with other solutions. d. Nonelectrolyte solutions do not conduct electricity. e. Nonelectrolyte solutions conduct heat. Question 2 Correct 4.60 points out of 4.60 Flag question Question text Vinegar is a solution of acetic acid, HC2H3O2 , dissolved in water. A 5.54-g sample of vinegar was neutralized by 30.10 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar? Select one: a. 0.0543% b. 1.08% c. 3.26% d. 5.43% e. 9.23% Question 3 Incorrect 0.00 points out of 4.60 Remove flag Question text Which is the net ionic equation for the reaction between aqueous solutions of lithium hydroxide and hydrobromic acid? LiOH(aq) + HBr(aq) → H2O(l) + LiBr(aq) Select one: a. LiOH(aq) → Li+(aq) + OH–(aq) b. HBr(aq) → H+(aq) + Br–(aq) c. H+(aq) + OH–(aq) → H2O(l) d. Li+(aq) + Br–(aq) → LiBr(aq) e. Li+(aq) + OH–(aq)+ H+(aq) + Br–(aq) → H2O(l) + LiBr(aq) Question 4 Correct 4.60 points out of 4.60 Flag question Question text The substance (CH3CH2)2NH is considered to be Select one: a. a weak acid. b. a weak base. c. a strong acid. d. a strong base. e. neither acidic nor basic. Question 5 Correct 4.60 points out of 4.60 Flag question Question text Which represents the result of mixing equal volumes of 1 M HCl and 1 M NH3 solutions? (Each sphere represents 1 mol of ions.) Select one: a. b. c. d. e. Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which of these chemical equations describes a metal displacement reaction? Select one: a. 2NaN3(s) → 2Na(s) + 3N2(g) b. Fe2O3(s) + 2Al(s) → 2Fe(s) + Al2O3(s) c. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) d. 2P(s) + 3Cl2(g) → 2PCl3(g) e. 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g) Question 7 Correct 4.60 points out of 4.60 Flag question Question text What is the oxidation number of oxygen in potassium superoxide, KO2? Select one: a. +1 b. 0 c. –½ d. +½ e. –2 Question 8 Correct 4.60 points out of 4.60 Flag question Question text Which of these equations does not represent an oxidation-reduction reaction? Select one: a. 3Al + 6HCl → 3H2 + AlCl3 b. 2H2O → 2H2 + O2 c. 2NaCl + Pb(NO3)2 → PbCl2 + 2NaNO3 d. 2NaI + Br2 → 2NaBr + I2 e. Cu(NO3)2 + Zn → Zn(NO3)2 + Cu Question 9 Correct 4.60 points out of 4.60 Flag question Question text For the reaction depicted below, if Z represents Zn, which metal could A represent? Select one: a. Fe b. Co c. Pb d. Ca e. Cu Question 10 Correct 4.60 points out of 4.60 Flag question Question text A 275-g sample of nickel at 100.0°C is placed in 100.0 g of water at 22.0°C. What is the final temperature of the water? Assume no heat transfer with the surroundings. The specific heat of nickel is 0.444 J/g·°C and the specific heat of water is 4.184 J/g·°C. Select one: a. 39.6°C b. 40.8°C c. 61.0°C d. 79.2°C e. 82.4°C Question 11 Correct 4.60 points out of 4.60 Flag question Question text Which of the following has a standard enthalpy of formation value (ΔH°f) of zero at 298 K? Select one: a. H2O(g) b. O(g) c. H2O(l) d. O2(g) e. O3(g) Question 12 Correct 4.60 points out of 4.60 Flag question Question text When 0.7521 g of benzoic acid was burned in a calorimeter containing 1000. g of water, a temperature rise of 3.60°C was observed. What is the heat capacity of the bomb calorimeter, excluding the water? The heat of combustion of benzoic acid is –26.42 kJ/g. Select one: a. 15.9 kJ/°C b. 4.2 kJ/°C c. 5.5 kJ/°C d. 1.3 kJ/°C e. 752 kJ/°C Question 13 Correct 4.60 points out of 4.60 Flag question Question text Complete the sentence: When heat is transferred to the system, the process is said to be ____________, and the sign of q is __________. Select one: a. exothermic, positive b. exothermic, negative c. endothermic, positive d. endothermic, negative e. forbidden, indeterminate Question 14 Correct 4.60 points out of 4.60 Flag question Question text Two solutions (the system), each with a volume of 25.0 mL at 25.0°C, are mixed in a beaker. A reaction occurs between them, and the temperature rises to 35.0°C. After the products have equilibrated with the surroundings, the temperature is again 25.0°C and the total volume is 50.0 mL. No gases are involved in the reaction. Which relationship concerning the change from initial to final states (both at 25.0°C) is correct? Select one: a. ΔU = 0 b. ΔH = 0 c. ΔU > 0 d. q = 0 e. w = 0 Question 15 Correct 4.60 points out of 4.60 Flag question Question text A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings. If the initial internal energy, U, is 61.2 kJ, what is the final value of U? Select one: a. 32.7 kJ b. 46.5 kJ c. 61.2 kJ d. 75.9 kJ e. 89.7 kJ Question 16 Correct 4.60 points out of 4.60 Flag question Question text Pentaborane B5H9(s) burns vigorously in O2 to give B2O3(s) and H2O(l). What is ΔH° for the combustion of 1 mol of B5H9(s)? Substance ΔH°f (kJ/mol) B2O3(s) –1273.5 B5H9(s) +73.2 H2O(l) –285.8 Select one: a. -1.5 × 103 kJ b. -1.6× 103 kJ c. -4.4 × 103 kJ d. -4.7× 103 kJ e. -9.0× 103 kJ Question 17 Correct 4.60 points out of 4.60 Flag question Question text If 325 g of water at 4.2°C absorbs 12.28 kJ, what is the final temperature of the water? The specific heat of water is 4.184 J/g·°C. Select one: a. 4.21°C b. 4.8°C c. 9.0°C d. 13.2°C e. 2938°C Question 18 Correct 4.60 points out of 4.60 Flag question Question text Atomic orbitals that have the same amount of energy are ______________. Select one: a. regenerative b. negatively charged c. degenerate d. positively charged e. zwitterionic Question 19 Correct 4.60 points out of 4.60 Flag question Question text ___________________ is the wavelength associated with a moving particle. Select one: a. The de Broglie wavelength b. The Heisenburg wavelength c. The Hund wavelength d. The Aufbau wavelength e. None of the answers is correct. Question 20 Correct 4.60 points out of 4.60 Flag question Question text The size of an atomic orbital is associated with Select one: a. the principal quantum number (n). b. the angular momentum quantum number (l). c. the magnetic quantum number (ml). d. the spin quantum number (ms). e. the angular momentum and magnetic quantum numbers, together. Question 21 Correct 4.60 points out of 4.60 Flag question Question text Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = –2.18 × 10–18 J(1/n2 ). (h = 6.63 × 10–34 J • s) Select one: a. 3.08 × 1015 s-1 b. 1.03 × 108 s-1 c. 2.06 × 1014 s-1 d. 1.35 × 10–51 s-1 e. 8.22 × 1014 s-1 Question 22 Correct 4.60 points out of 4.60 Flag question Question text A possible set of quantum numbers for the last electron added to complete an atom of germanium in its ground state is n l ml ms A 4 0 0 +1/2 B 3 0 +1 –1/2 C 4 1 –1 +1/2 D 3 1 +1 –1/2 E 4 2 +2 –1/2 Select one: a. A b. B c. C d. D e. E Question 23 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a correct set of quantum numbers for an electron in a 5f orbital? Select one: a. n = 5, l = 3, ml = +1 b. n = 5, l = 2, ml = +3 c. n = 4, l = 3, ml = 0 d. n = 4, l = 2, ml = +1 e. n = 5, l = 4, ml = 3. Question 24 Incorrect 0.00 points out of 4.60 Remove flag Question text How many electrons are in the 4p orbitals of selenium? Select one: a. 0 b. 2 c. 4 d. 5 e. 6 Question 25 Correct 4.60 points out of 4.60 Flag question Question text What is the frequency of light having a wavelength of 360 nm? (c = 3.00 x 108 m/s) Select one: a. 8.3 × 1014 s–1 b. 1.2 × 10–6 s–1 c. 8.3 × 105 s–1 d. 108 s–1 e. 1.2 × 10–15 s–1 [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 3 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 9: Properties of Gases Started on Friday, April 15, 2022, 7:51 PM State Finished Completed on Friday, April 15, ... [Show More] 2022, 8:09 PM Time taken 17 mins 47 secs Grade 115.00 out of 115.00 (100%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text The nineteenth century chemists arranged elements in the periodic table according to increasing Select one: a. atomic number. b. number of electrons. c. atomic mass. d. number of neutrons. e. nuclear binding energy. Question 2 Correct 4.60 points out of 4.60 Flag question Question text Which one of these ions is not isoelectronic with Kr? Select one: a. As3+ b. Se2– c. Rb+ d. Sr2+ e. Br– Question 3 Correct 4.60 points out of 4.60 Flag question Question text Elements with ________________ first ionization energies and ___________ electron affinities generally form cations. Select one: a. low, very negative b. high, positive or slightly negative c. low, positive or slightly negative d. high, very negative e. None of these is generally correct. Question 4 Correct 4.60 points out of 4.60 Flag question Question text Which ground-state ion does not have an electron configuration described by the following orbital diagram? [Ar] ↿ ↿ ↿ ↿ 4s 3d Select one: a. V+ b. Cr2+ c. Mn3+ d. Co5+ e. Fe4+ Question 5 Correct 4.60 points out of 4.60 Flag question Question text An element with the electron configuration [noble gas]ns2(n – 1)d8 has ___________ valence electrons. Select one: a. 2 b. 6 c. 8 d. 10 e. None of these choices is correct. Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which pair of ions exhibits the greatest attractive force between them? Select one: a. Na+ and Cl– b. Ca2+ and Cl– c. Na+ and S2– d. Al3+ and Mg2+ e. Mg2+ and O2– Question 7 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is an amphoteric oxide? Select one: a. Na2O b. MgO c. Al2O3 d. SO2 e. Cl2O7 Question 8 Correct 4.60 points out of 4.60 Flag question Question text In the best Lewis structure for the fulminate ion, CNO–, what is the formal charge on the central nitrogen atom? Select one: a. +2 b. +1 c. 0 d. –1 e. –2 Question 9 Correct 4.60 points out of 4.60 Flag question Question text Which of the following contains ionic bonding? Select one: a. CO b. SrF2 c. Al d. OCl2 e. HCl Question 10 Correct 4.60 points out of 4.60 Flag question Question text What is the formal charge on phosphorus in a Lewis structure for the phosphate ion that satisfies the octet rule? Select one: a. –2 b. –1 c. 0 d. +1 e. +2 Question 11 Correct 4.60 points out of 4.60 Flag question Question text How many dots does the Lewis dot symbol for sodium have around it? Select one: a. 1 b. 2 c. 0 d. 3 e. 7 Question 12 Correct 4.60 points out of 4.60 Flag question Question text What formal charge resides on the carbon of CO32–? Select one: a. 0 b. +1 c. +2 d. +3 e. +4 Question 13 Correct 4.60 points out of 4.60 Flag question Question text Which of these compounds is most likely to be ionic? Select one: a. NCl3 b. BaCl2 c. CO d. SO2 e. SF4 Question 14 Correct 4.60 points out of 4.60 Flag question Question text Which is true concerning the dipole moment of a CO2 molecule? Select one: a. The dipole moment is zero because the C–O bond is nonpolar. b. The dipole moment is zero because the molecule is linear. c. The dipole moment is zero because the molecule is bent. d. The dipole moment is nonzero because the molecule is linear. e. The dipole moment is nonzero because the molecule is bent. Question 15 Correct 4.60 points out of 4.60 Flag question Question text What is the total number of electron domains around the central atom for a molecule having a trigonal pyramidal molecular geometry, such as NH3? Select one: a. 5 b. 2 c. 3 d. 4 e. 6 Question 16 Correct 4.60 points out of 4.60 Flag question Question text What is the molecular geometry of SiF62– as predicted by the VSEPR model? Select one: a. trigonal bipyramidal b. octahedral c. tetrahedral d. seesaw e. square pyramidal Question 17 Correct 4.60 points out of 4.60 Flag question Question text Using the VSEPR model, what is the predicted molecular geometry of the PCl3 molecule? Select one: a. linear b. bent c. trigonal planar d. trigonal pyramidal e. tetrahedral Question 18 Correct 4.60 points out of 4.60 Flag question Question text The nitrosonium ion, NO+, forms a number of interesting complexes with nickel, cobalt, and iron. According to molecular orbital theory, which statement about NO+ is correct? Select one: a. NO+ has a bond order of 2 and is paramagnetic. b. NO+ has a bond order of 2 and is diamagnetic. c. NO+ has a bond order of 3 and is paramagnetic. d. NO+ has a bond order of 3 and is diamagnetic. e. NO+ has a bond order of 2.5 and is neither paramagnetic nor diamagnetic. Question 19 Correct 4.60 points out of 4.60 Flag question Question text What is the molecular geometry of HOF as predicted by the VSEPR model? Select one: a. trigonal pyramidal b. bent c. tetrahedral d. linear e. trigonal planar Question 20 Correct 4.60 points out of 4.60 Flag question Question text What is the Kelvin temperature at 24°C? Select one: a. 249 K b. 11.4 K c. –297 K d. –249 K e. 297 K Question 21 Correct 4.60 points out of 4.60 Flag question Question text What is the temperature in Celsius at 77 K, which is the normal boiling point of liquid nitrogen? Select one: a. –350°C b. –196°C c. 350°C d. 196°C e. 3.55°C Question 22 Correct 4.60 points out of 4.60 Flag question Question text What is the temperature in Celsius at 4 K, which is the normal boiling point of liquid helium? Select one: a. –269°C b. 269°C c. 277°C d. 68.3°C e. –277°C Question 23 Correct 4.60 points out of 4.60 Flag question Question text A gas sample occupies 8.76 L at a temperature of 37°C. What is the volume if the temperature is lowered to 0°C at constant pressure? Select one: a. 9.95 L b. 0 L c. 4.22 L d. 74.1 L e. 7.71 L Question 24 Correct 4.60 points out of 4.60 Flag question Question text The Kelvin temperature scale is useful when comparing Select one: a. various gas samples at different densities. b. volume of a gas sample with temperature at constant pressure. c. pressure of gas samples at different volumes and constant temperature. d. various liquids at constant pressure. Question 25 Correct 4.60 points out of 4.60 Flag question Question text A sample of gas occupies 24.5 L at a pressure of 1.57 atm. What is the pressure if the volume is increased to 48.3 L at constant temperature? Select one: a. 0.796 atm b. 1.26 atm c. 3.10 atm d. 5.38 × 10–4 atm e. 1.86 × 103 atm [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 3 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 9: Properties of Gases Started on Thursday, March 17, 2022, 6:27 PM State Finished Completed on Thursday, March ... [Show More] 17, 2022, 7:27 PM Time taken 59 mins 46 secs Grade 101.20 out of 115.00 (88%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text What elements and groups have properties that are most similar to those of chlorine? Select one: a. F, Br, I, and nonmetals in Group 7A b. Cl, K, C, and metals in Group 1B c. N, P, As, and lanthanides d. He, Ne, Xe, and nonmetals in Group 7A e. O, S, and P Question 2 Correct 4.60 points out of 4.60 Flag question Question text Which species have the most similar atomic radii? Select one: a. S2– and Cl– b. Ar and As c. Rb+ and K+ d. I– and Br – e. Br and Cs Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which of these elements has the smallest first ionization energy? Select one: a. Cl b. Na c. Be d. K e. As Question 4 Correct 4.60 points out of 4.60 Flag question Question text Which of these choices is the electron configuration for the chloride ion? Select one: a. [Ne]3s23p4 b. [Ne]3s23p7 c. [Ar] d. [Ar]4s1 e. [Ne]3s23p5 Question 5 Correct 4.60 points out of 4.60 Flag question Question text The general electron configuration for noble gas atoms is Select one: a. ns2np6. b. ns2np5. c. ns2np4. d. ns2np3. e. ns2. Question 6 Incorrect 0.00 points out of 4.60 Flag question Question text Which of the following most accurately describes the trend in metallic character? Select one: a. Increases from left to right across a period because the number of valence electrons increases b. Decreases from left to right across a period because the electronegativity increases c. Increases from top to bottom in a group because the ionization energy decreases d. Decreases from top to bottom because the nuclear charge increases Question 7 Correct 4.60 points out of 4.60 Flag question Question text Which of the following elements will form an acidic compound with hydrogen? Select one: a. Sodium b. Carbon c. Fluorine d. Nitrogen e. Boron Question 8 Correct 4.60 points out of 4.60 Flag question Question text The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What does the dot or dots represent? Select one: a. Electron configuration b. Valence electrons c. Atomic number d. Atomic mass e. Core electrons Question 9 Incorrect 0.00 points out of 4.60 Flag question Question text How many dots does the Lewis dot symbol for oxygen have around it? Select one: a. 4 b. 2 c. 6 d. 3 e. 7 Question 10 Correct 4.60 points out of 4.60 Flag question Question text The number of resonance structures for the sulfur dioxide molecule that satisfy the octet rule is Select one: a. 1. b. 2. c. 3. d. 4. e. none of these Question 11 Correct 4.60 points out of 4.60 Flag question Question text The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What does the dot or dots represent? Select one: a. Electron configuration b. Valence electrons c. Atomic number d. Atomic mass e. Core electrons Question 12 Correct 4.60 points out of 4.60 Flag question Question text Select the compound with the highest (i.e., most negative) lattice energy. Select one: a. CaS(s) b. BaO(s) c. NaI(s) d. LiBr(s) e. MgO(s) Question 13 Correct 4.60 points out of 4.60 Flag question Question text The Lewis structure for CS2 is: Select one: a. b. c. d. Question 14 Correct 4.60 points out of 4.60 Flag question Question text The PCl5 molecule has Select one: a. nonpolar bonds, and is a nonpolar molecule. b. nonpolar bonds, but is a polar molecule. c. polar bonds, and is a polar molecule. d. polar bonds, but is a nonpolar molecule. Question 15 Correct 4.60 points out of 4.60 Flag question Question text Which statement is not true of molecular orbitals? Select one: a. The number of molecular orbitals formed is always equal to the number of atomic orbitals combined. b. A molecular orbital can accommodate up to two electrons. c. When electrons are added to orbitals of the same energy, the most stable arrangement is predicted by Hund's rule. d. Low-energy molecular orbitals fill before high-energy molecular orbitals fill. e. Antibonding molecular orbitals are higher in energy than all of the bonding molecular orbitals. Question 16 Correct 4.60 points out of 4.60 Flag question Question text What is the predicted O–C–O bond angle in CO2? Select one: a. 60° b. 90° c. 109.5° d. 120° e. 180° Question 17 Correct 4.60 points out of 4.60 Flag question Question text Using the VSEPR model, predict the molecular geometry around the central atom in PO43–. Select one: a. trigonal planar b. trigonal pyramidal c. tetrahedral d. trigonal bipyramidal e. octahedral Question 18 Incorrect 0.00 points out of 4.60 Flag question Question text The hybridization of the central nitrogen atom in the molecule N2O is Select one: a. sp. b. sp2. c. sp3. d. sp3d. e. sp3d2. Question 19 Correct 4.60 points out of 4.60 Flag question Question text Using the VSEPR model, predict the molecular geometry around the central atom in SO32–. Select one: a. trigonal planar b. trigonal pyramidal c. tetrahedral d. trigonal bipyramidal e. octahedral Question 20 Correct 4.60 points out of 4.60 Flag question Question text What is the temperature in Celsius at 4 K, which is the normal boiling point of liquid helium? Select one: a. –269°C b. 269°C c. 277°C d. 68.3°C e. –277°C Question 21 Correct 4.60 points out of 4.60 Flag question Question text What is the Kelvin temperature at 24°C? Select one: a. 249 K b. 11.4 K c. –297 K d. –249 K e. 297 K Question 22 Correct 4.60 points out of 4.60 Flag question Question text What is the temperature in Celsius at 77 K, which is the normal boiling point of liquid nitrogen? Select one: a. –350°C b. –196°C c. 350°C d. 196°C e. 3.55°C Question 23 Correct 4.60 points out of 4.60 Flag question Question text A sample of nitrogen gas is confined to a 14.0-L container at 375 torr and 37.0°C. How many moles of nitrogen are in the container? (R = 0.08206 L • atm/K • mol, 1 atm = 760 torr) Select one: a. 0.272 mol b. 2.27 mol c. 3.69 mol d. 206 mol e. 227 mol Question 24 Correct 4.60 points out of 4.60 Flag question Question text What is the density of carbon dioxide gas at –25.2°C and 98.0 kPa? (R = 0.08206 L • atm/K • mol, 1 atm = 101,325 Pa) Select one: a. 0.232 g/L b. 0.279 g/L c. 0.994 g/L d. 1.74 g/L e. 2.09 g/L Question 25 Correct 4.60 points out of 4.60 Flag question Question text In the van der Waals equation, the constant a is a constant that is part of a correction factor for _________. Select one: a. the volume of the gas b. the temperature of the gas c. the pressure of the gas d. the ideal gas constant [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 4 - APRIL 2022
• CHEM101_MH_V4 • Topic 11: Modern Materials Started on Friday, April 15, 2022, 8:10 PM State Finished Completed on Friday, April 15, 2022, 8:31 PM... [Show More] Time taken 20 mins 58 secs Grade 115.00 out of 115.00 (100%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text Which substance has the highest vapor pressure at room temperature? Select one: a. HF b. HCl c. HBr d. HI e. All of these substances have the same vapor pressure at room temperature. Question 2 Correct 4.60 points out of 4.60 Flag question Question text Choose the response that lists the member of each of the following pairs that has the higher boiling point. I. H2O or KI, II. HF or HI, III. Cl2 or Br2 Select one: a. H2O, HF, and Cl2 b. KI, HF, and Br2 c. KI, HI, and Br2 d. H2O, HI, and Cl2 e. KI, HF, and Cl2 Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is defined as the attractive forces between polar molecules? I. dispersion forces II. dipole-dipole interactions III. ion-dipole interactions Select one: a. I and III b. II only c. III only d. I, II, and III e. I only Question 4 Correct 4.60 points out of 4.60 Flag question Question text What is the name given for the attraction between unlike molecules involved in capillary action? Select one: a. Adhesion b. Ionization c. Cohesion d. Surface tension e. Viscosity Question 5 Correct 4.60 points out of 4.60 Flag question Question text Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first. Select one: a. C7H16, C5H12 b. CCl4, CBr4 c. H2O, H2S d. CH3CH2OH, CH3–O–CH3 e. Xe, Kr Question 6 Correct 4.60 points out of 4.60 Flag question Question text Platinum has a face-centered cubic crystal structure and a density of 21.5 g/cm3. What is the radius of a platinum atom? Select one: a. 69 pm b. 98 pm c. 139 pm d. 196 pm e. 277 pm Question 7 Correct 4.60 points out of 4.60 Flag question Question text Which corresponds to the temperature-dependent partial pressure above the surface of a liquid? Select one: a. Surface tension b. Vapor pressure c. Boiling point d. Viscosity e. Capillary action Question 8 Correct 4.60 points out of 4.60 Flag question Question text Use the following data to determine the molar heat of vaporization of chlorine gas. (R = 8.314 J/K • mol) T (°C) –84.5 –71.2 –47.3 P (mmHg) 40.0 100.0 400.0 Select one: a. 34.7 kJ/mol b. 21.9 kJ/mol c. 3.45 kJ/mol d. 712 J/mol e. 9.99 kJ/mol Question 9 Correct 4.60 points out of 4.60 Flag question Question text Based on the phase diagram of a pure substance given below, what phase exists at point F? Select one: a. vapor + liquid b. vapor c. liquid d. solid e. supercritical fluid Question 10 Correct 4.60 points out of 4.60 Flag question Question text What mass of water would need to evaporate from your skin in order to dissipate 1.70 ×105 J of heat from the surface of your body? H2O(l) → H2O(g) ΔHvap = 40.7 kJ/mol Select one: a. 2.26 g b. 4.18 g c. 75.2 g d. 4.18 ×103 g e. 4.07 × 104 g Question 11 Correct 4.60 points out of 4.60 Flag question Question text Iron crystallizes in the body-centered cubic lattice. What is the coordination number for Fe? Select one: a. 4 b. 6 c. 8 d. 10 e. 12 Question 12 Correct 4.60 points out of 4.60 Flag question Question text What is defined as the number of atoms surrounding an atom in a crystal lattice and indicates how tightly the atoms are packed together? Select one: a. the unit cell b. the radius of the cubic cell c. the coordination number d. the area of the cubic cell e. the atoms themselves Question 13 Correct 4.60 points out of 4.60 Flag question Question text An amino acid is a compound that contains at least Select one: a. one amino group and one amide group. b. two amino groups and one carboxylic acid group. c. one hydroxyl group and one methyl group. d. one carboxylic acid group and one amino group. e. one methyl group and one amide group. Question 14 Correct 4.60 points out of 4.60 Flag question Question text A peptide bond (also called an amide bond) joins two amino acids together. What atoms are linked by this bond? Select one: a. C — O b. C — H c. C — N d. N — S e. S — C Question 15 Correct 4.60 points out of 4.60 Flag question Question text Which one of these choices is the general structural formula of an amino acid? Select one: a. b. R–CH2–NH2 c. d. Question 16 Correct 4.60 points out of 4.60 Flag question Question text Which one of these elements is not found in proteins? Select one: a. S b. P c. C d. O e. N Question 17 Correct 4.60 points out of 4.60 Flag question Question text The segment represents the polymer named Select one: a. polyethylene. b. polyvinyl chloride. c. polystyrene. d. polybutylene. e. polypropylene. Question 18 Correct 4.60 points out of 4.60 Flag question Question text The polymer formed from the monomer CH2=CH–CN is Select one: a. . b. (CH2=CHCN)n. c. (CH2=CH=CN)n. d. . Question 19 Correct 4.60 points out of 4.60 Flag question Question text Most high-temperature superconducting materials are Select one: a. metals. b. metal chlorides. c. polymers. d. fullerenes. e. ceramics. Question 20 Correct 4.60 points out of 4.60 Flag question Question text Which is NOT an example of a block copolymer formed between monomers A and B? Select one: a. -A-A-B-B-B-A-A-B-B-B- b. -A-B-A-B-A-B-A-B-A-B- c. -A-A-A-B-B-B-A-A-A-B-B-B- d. -A-A-A-B-B-A-A-A-B-B- e. -B-B-A-A-B-B-A-A-B-B- Question 21 Correct 4.60 points out of 4.60 Flag question Question text Which of the following polymers is a condensation polymer? Select one: a. Polystyrene b. Teflon® c. Polyvinylchloride d. Polypropylene e. Dacron® Question 22 Correct 4.60 points out of 4.60 Flag question Question text Polyacrylonitrile, characterized by the following repeating unit, is made from which of these monomers? Select one: a. CH3CH2CN b. HOCH2CH2CH3 c. CH3CH=CHCN d. CH2=CHCN e. CH2=CNCH3 Question 23 Correct 4.60 points out of 4.60 Flag question Question text Which monomer, when polymerized, results in the polymer polystyrene? Select one: a. CF2=CF2 b. CCl2=CF2 c. C6H5–CH=CH2 d. CH3CH=CH2 e. CH3CH=CH2CH3 Question 24 Correct 4.60 points out of 4.60 Flag question Question text What is the name given to the polymers that can be melted and reshaped or heated and bent? Select one: a. Flex polymers b. Thermal polymers c. T-polymers d. Thermoplastic polymers e. Thermosetting polymers Question 25 Correct 4.60 points out of 4.60 Flag question Question text Which one of these materials is a copolymer? Select one: a. Styrene-butadiene b. Polyvinyl chloride c. Polypropylene d. Poly-cis-isoprene e. Polyethylene [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 4 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 11: Modern Materials Started on Saturday, March 26, 2022, 12:57 AM State Finished Completed on Saturday, March 2... [Show More] 6, 2022, 1:29 AM Time taken 31 mins 47 secs Grade 96.60 out of 115.00 (84%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text How much energy (heat) is required to convert 52.0 g of ice at –10.0°C to steam at 100°C? Specific heat of ice 2.09 J/g • °C Specific heat of water 4.18 J/g • °C Specific heat of steam 1.84 J/g • °C Molar heat of fusion 6.02 kJ/mol Molar heat of vaporization 40.7 kJ/mol Select one: a. 12.0 kJ b. 23.0 kJ c. 46.4 kJ d. 158 kJ e. 2.30 ×104 kJ Question 2 Correct 4.60 points out of 4.60 Flag question Question text The vapor pressure of ethanol is 400. mmHg at 63.5°C. Its molar heat of vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol, in mmHg, at 34.9°C? (R = 8.314 J/K • mol) Select one: a. 109 mmHg b. 220 mmHg c. 366 mmHg d. 376 mmHg e. 1470 mmHg Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which of the following statements is true? Select one: a. The higher the viscosity, the faster a liquid flows. b. The viscosity increases with increasing temperature. c. The stronger the intermolecular forces, the higher the viscosity. d. Hydrogen bonding in water gives rise to its unusually low viscosity. e. The viscosity of gases is larger than the viscosity of liquids. Question 4 Correct 4.60 points out of 4.60 Flag question Question text What is another name given to dispersion forces? Select one: a. ion-dipole interactions b. dipole-dipole interactions c. hydrogen bonding d. covalent forces e. London forces Question 5 Correct 4.60 points out of 4.60 Flag question Question text Which of the following atoms does not participate in hydrogen bonding? Select one: a. S b. O c. F d. N e. H Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which substance should exhibit hydrogen bonding in the liquid phase? Select one: a. PH3 b. He c. H2S d. CH4 e. CH3OH Question 7 Correct 4.60 points out of 4.60 Flag question Question text Liquid ammonia can be used as a refrigerant and heat transfer fluid. How much energy is required to heat 25.0 g of NH3(l) from –65.0°C to –12.0°C? Normal boiling point –33.4°C Specific heat of NH3(l) 4.7 J/g • °C Specific heat of NH3(g) 2.2 J/g • °C Molar heat of vaporization 23.5 kJ/mol Select one: a. 4.92 kJ b. 16.0 kJ c. 34.5kJ d. 39.4 kJ e. 182.8kJ Question 8 Correct 4.60 points out of 4.60 Flag question Question text Octane has a vapor pressure of 40. torr at 45.1°C and 400. torr at 104.0°C. What is its heat of vaporization? (R = 8.314 J/K • mol) Select one: a. 39.1 kJ/mol b. 46.0 kJ/mol c. 590 kJ/mol d. 710 kJ/mol e. None of these choices is correct. Question 9 Correct 4.60 points out of 4.60 Flag question Question text Octane is a component of fuel used in internal combustion engines. The dominant intermolecular forces in octane are Select one: a. dipole-dipole forces. b. London dispersion forces. c. hydrogen bonding. d. covalent bonds. e. carbon-hydrogen bonds. Question 10 Incorrect 0.00 points out of 4.60 Flag question Question text The location that indicates conditions under which two phases can exist in equilibrium is called the Select one: a. triple point. b. critical point. c. phase boundary. d. phase diagram. e. transition state. Question 11 Correct 4.60 points out of 4.60 Flag question Question text What is defined as the number of atoms surrounding an atom in a crystal lattice and indicates how tightly the atoms are packed together? Select one: a. the unit cell b. the radius of the cubic cell c. the coordination number d. the area of the cubic cell e. the atoms themselves Question 12 Correct 4.60 points out of 4.60 Flag question Question text Lead crystallizes in the face-centered cubic lattice. What is the coordination number for Pb? Select one: a. 4 b. 6 c. 8 d. 10 e. 12 Question 13 Correct 4.60 points out of 4.60 Flag question Question text Which one of these choices is the general structural formula of an amino acid? Select one: a. b. R–CH2–NH2 c. d. Question 14 Correct 4.60 points out of 4.60 Flag question Question text A peptide bond (also called an amide bond) joins two amino acids together. What atoms are linked by this bond? Select one: a. C — O b. C — H c. C — N d. N — S e. S — C Question 15 Correct 4.60 points out of 4.60 Flag question Question text Which one of these elements is not found in proteins? Select one: a. S b. P c. C d. O e. N Question 16 Incorrect 0.00 points out of 4.60 Flag question Question text The functional group found in proteins is called a (an) Select one: a. amide. b. carboxylic acid. c. amine. d. amino acid. e. dipeptide. Question 17 Correct 4.60 points out of 4.60 Flag question Question text A polymer made in a polymerization reaction that produces small molecules (such as water) as well as the polymer is classified as a/an _______ polymer. Select one: a. addition b. natural c. condensation d. elimination e. copolymer Question 18 Correct 4.60 points out of 4.60 Flag question Question text What is meant by HIPS? Select one: a. High polysaccharides b. High in polysaccharides c. Highly ionic polymer solution d. High-impact polystyrene e. Highly ionic protein solution Question 19 Correct 4.60 points out of 4.60 Flag question Question text What is the name of the industrial process in which sulfur (S8) is used to create linkages between individual polymer chains in rubber? Select one: a. Rubberization b. Vulcanization c. Smelting d. Sulfonafication e. Sulfonation Question 20 Correct 4.60 points out of 4.60 Flag question Question text Materials with no resistance to the flow of electrons are called Select one: a. conductors. b. insulators. c. superconductors. d. semiconductors. e. nonconductors. Question 21 Incorrect 0.00 points out of 4.60 Flag question Question text Which of the following polymers is used in plastic food bags and wraps? Select one: a. LDPE b. PVC c. Polystyrene d. HDPE e. Polypropylene Question 22 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a synthetic polymer? Select one: a. cellulose b. polyisoprene c. DNA d. poly(hexamethyleneadipamide) e. enzymes Question 23 Incorrect 0.00 points out of 4.60 Flag question Question text What is the process called that produces particles of nearly uniform size that are much more likely to produce a solid ceramic without gaps or cracks? Select one: a. Sintering b. Roasting c. Firing d. Stonewaring e. Sol-gel Question 24 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a medical application using polymers? Select one: a. Implants b. Prosthetics c. Wound dressings d. All of these choices are correct e. None of these choices is correct. Question 25 Correct 4.60 points out of 4.60 Flag question Question text What name is given to the polymers whose shape is determined as part of the chemical process that formed the polymer? Select one: a. Flex polymers b. Thermal polymers c. T-polymers d. Thermoplastic polymers e. Thermosetting polymers [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 5 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 13: Acids and Bases Started on Friday, April 15, 2022, 8:48 PM State Finished Completed on Friday, April 15, 202... [Show More] 2, 9:08 PM Time taken 19 mins 14 secs Grade 115.00 out of 115.00 (100%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text A solution of chloroform, CHCl3, and acetone, (CH3)2CO, exhibits a negative deviation from Raoult's law. This result implies that Select one: a. chloroform-chloroform interactions are stronger than chloroform-acetone interactions. b. chloroform-chloroform interactions are weaker than chloroform-acetone interactions. c. acetone-acetone interactions are stronger than chloroform-acetone interactions. d. acetone-acetone interactions are weaker than chloroform-acetone interactions. e. Choice 2 and 4 Question 2 Correct 4.60 points out of 4.60 Flag question Question text At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's law constant of Cl2 in water? (R = 0.0821 atm • L • mol–1• K–1 ) Select one: a. 3.8 mol • L–1• atm–1 b. 0.043 mol • L–1• atm–1 c. 36 mol • L–1• atm–1 d. 3.1 mol • L–1• atm–1 e. 0.13 mol • L–1• atm–1 Question 3 Correct 4.60 points out of 4.60 Flag question Question text What is the vapor pressure above a solution prepared by dissolving 0.500 mol of a nonvolatile solute in 275 g of hexane (86.18 g/mol) at 49.6°C? P°hexane = 400.0 torr at 49.6°C. Select one: a. 54 torr b. 154 torr c. 246 torr d. 346 torr e. 400. torr Question 4 Correct 4.60 points out of 4.60 Flag question Question text A solution is 40.00% by volume benzene (C6H6) in carbon tetrachloride at 20°C. The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm3; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm3. If this solution is ideal, its total vapor pressure at 20°C is Select one: a. 84.64 mmHg b. 84.30 mmHg c. 82.96 mmHg d. 81.63 mmHg e. 165.93 mmHg Question 5 Correct 4.60 points out of 4.60 Flag question Question text Safrole was once used as a flavoring in root beer, until it was banned in 1960. What is the vapor pressure of a solution prepared by dissolving 0.75 mol of nonvolatile safrole in 950 g of ethanol (46.07 g/mol)? P°ethanol = 50.0 torr at 25°C. Select one: a. 1.8 torr b. 11 torr c. 15 torr d. 40 torr e. 48 torr Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which combination of a 36.0% (w/w) stock solution of acetic acid (d = 1.045 g/mL) and water will result in 1.00 kg of a 15.0% (w/w) acetic acid solution? Select one: a. 417 mL of 36% acetic acid in 583 mL of distilled water b. 417 g of 36% acetic acid in 583 g of distilled water c. 360 mL of 36% acetic acid in 640 mL of distilled water d. 360 g of 36% acetic acid in 640 g of distilled water e. 150 g of 36% acetic acid in 850 g of distilled water Question 7 Correct 4.60 points out of 4.60 Flag question Question text What is the name of a solution that obeys Raoult's law? Select one: a. Ideal solution b. Nonideal solution c. Suspension d. Solute e. Solvent Question 8 Correct 4.60 points out of 4.60 Flag question Question text The osmotic pressure of a 0.82 M HCl solution is 35.9 atm at 18°C. Calculate the van't Hoff factor for HCl at this concentration. Select one: a. 1.8 b. 17.2 c. 1.5 d. 2.00 Question 9 Correct 4.60 points out of 4.60 Flag question Question text Which is most soluble in CCl4? Select one: a. NaCl b. H2O c. NaOH d. C8H18 e. CH3OH Question 10 Correct 4.60 points out of 4.60 Flag question Question text Cadmium bromide is used in photography and lithography. What is the molality of a solution prepared by dissolving 45.38 g of CdBr2 in 375.0 g of water? Select one: a. 0.03035 m b. 0.01600 m c. 0.1210 m d. 0.4446 m e. 16.00 m Question 11 Correct 4.60 points out of 4.60 Flag question Question text What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution? Select one: a. 0.0371 g b. 0.888 g c. 21.3 g d. 250. g e. 340. g Question 12 Correct 4.60 points out of 4.60 Flag question Question text The structure of Vitamin B1, thiamine, is shown here. Vitamin B1 is most soluble in _________. Select one: a. fats b. water c. air d. carbon tetrachloride e. octane Question 13 Correct 4.60 points out of 4.60 Flag question Question text The distinguishing characteristic of all electrolyte solutions is that they Select one: a. contain molecules. b. conduct electricity. c. react with other solutions. d. always contain acids. e. conduct heat. Question 14 Correct 4.60 points out of 4.60 Flag question Question text A 0.100 m K2SO4 solution has a freezing point of –0.43°C. What is the van't Hoff factor for this solution? (Kf = 1.86°C/m) Select one: a. 0.77 b. 1.0 c. 2.3 d. 3.0 e. 3.7 Question 15 Correct 4.60 points out of 4.60 Flag question Question text Since arsenic is a nonmetal, As2O3 is expected to be a/an _____ oxide. Select one: a. acidic b. ionic c. amphoteric d. neutral e. basic Question 16 Correct 4.60 points out of 4.60 Flag question Question text Ammonium chloride is used as an electrolyte in dry cells. Which statement about a 0.10 M solution of NH4Cl is correct? Select one: a. The solution is weakly basic. b. The solution is strongly basic. c. The solution is neutral. d. The solution is acidic. e. The values for Ka and Kb for the species in solution must be known before a prediction can be made. Question 17 Correct 4.60 points out of 4.60 Flag question Question text Which is a Lewis acid? Select one: a. CH3NH2 b. BCl3 c. F– d. BF4– e. CH4 Question 18 Correct 4.60 points out of 4.60 Flag question Question text What is the pH of a 0.014 M Ca(OH)2 solution? Select one: a. 1.85 b. 1.55 c. 12.15 d. 12.45 e. 15.85 Question 19 Correct 4.60 points out of 4.60 Flag question Question text What is the name given to a substance that can act as a Brønsted acid or as a Brønsted base according to what it is reacting with? Select one: a. hydrophilic b. hydrophobic c. amphoteric d. isoprotic e. isoelectronic Question 20 Correct 4.60 points out of 4.60 Flag question Question text What is the conjugate base of water? Select one: a. H3O+ b. OH– c. H3O d. OH e. H2O2 Question 21 Correct 4.60 points out of 4.60 Flag question Question text Calculate the pH of a 0.021 M NaCN solution. [Ka(HCN) = 4.9 × 10–10] Select one: a. 1.68 b. 3.19 c. 4.69 d. 9.31 e. 10.81 Question 22 Correct 4.60 points out of 4.60 Flag question Question text Which is a Lewis acid but not a Brønsted acid? Select one: a. HCN b. CO32– c. OH– d. Cl– e. Al3+ Question 23 Correct 4.60 points out of 4.60 Flag question Question text What is the pH of a 0.056 M HNO3 solution? Select one: a. 0.056 b. 1.25 c. 12.75 d. 2.88 e. 11.11 Question 24 Correct 4.60 points out of 4.60 Flag question Question text Below is a representation of an aqueous solution of a weak acid HA at equilibrium. (Each circle represents 1.0 mmol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are not shown for clarity.) What is the percent ionization of HA? Select one: a. 100% b. 50% c. 25% d. 12.5% e. Cannot be calculated without knowledge of Ka Question 25 Correct 4.60 points out of 4.60 Flag question Question text Hard water deposits (calcium carbonate) have built up around your bathroom sink. Which of these substances would be most effective in dissolving the deposits? Select one: a. ammonia b. bleach (sodium hypochlorite) c. lye (sodium hydroxide) d. vinegar (acetic acid) [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 5 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 13: Acids and Bases Started on Monday, March 28, 2022, 9:26 AM State Finished Completed on Monday, March 28, 202... [Show More] 2, 10:05 AM Time taken 38 mins 38 secs Grade 105.80 out of 115.00 (92%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text Consider the following four solutions: • NaCl in water • Acetic acid in water • Acetic acid in benzene • Naphthalene in benzene Which of these solutions has the strongest solute-solvent interactions and the interaction is of which type? Select one: a. Acetic acid in water; hydrogen bonding b. Acetic acid in benzene; dipole-induced dipole interaction c. NaCl in water; ion-dipole interaction d. Naphthalene in benzene; London Dispersion Forces e. NaCl in water; hydrogen bonding Question 2 Correct 4.60 points out of 4.60 Flag question Question text What states that the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution? Select one: a. Entropy b. Henry's law c. Dissolution d. Vapor pressure e. Enthalpy of salvation Question 3 Correct 4.60 points out of 4.60 Flag question Question text A solution is 40.00% by volume benzene (C6H6) in carbon tetrachloride at 20°C. The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm3; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm3. If this solution is ideal, its total vapor pressure at 20°C is Select one: a. 84.64 mmHg b. 84.30 mmHg c. 82.96 mmHg d. 81.63 mmHg e. 165.93 mmHg Question 4 Correct 4.60 points out of 4.60 Flag question Question text Which statement is false? Select one: a. The vapor pressure of a solvent over a solution decreases as its mole fraction increases. b. The solubility of a gas increases as the temperature decreases. c. The vapor pressure of a solvent over a solution is less than that of pure solvent. d. The greater the pressure of a gas over a solution, the greater its solubility. e. Ionic solutes dissociate in solution, causing an enhancement of all colligative properties. Question 5 Correct 4.60 points out of 4.60 Flag question Question text Safrole was once used as a flavoring in root beer, until it was banned in 1960. What is the vapor pressure of a solution prepared by dissolving 0.75 mol of nonvolatile safrole in 950 g of ethanol (46.07 g/mol)? P°ethanol = 50.0 torr at 25°C. Select one: a. 1.8 torr b. 11 torr c. 15 torr d. 40 torr e. 48 torr Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which of these compounds is a weak electrolyte? Select one: a. HCl b. NH3 c. C6H12O6 (glucose) d. N2 e. KCl Question 7 Correct 4.60 points out of 4.60 Flag question Question text What relationship states that the partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent times the mole fraction of the solvent in the solution? Select one: a. Henry's law b. Law of partial pressures c. Curie's law d. Raoult's law e. Vapor pressure Question 8 Correct 4.60 points out of 4.60 Flag question Question text When 12.1 g of the sugar sucrose (a nonelectrolyte) are dissolved in exactly 800 g of water, the solution has a freezing point of –0.082°C. What is the molar mass of sucrose? (Kf of water is 1.86°C/m.) Select one: a. 426 g/mol b. 99.2 g/mol c. 178 g/mol d. 266 g/mol e. 343 g/mol Question 9 Correct 4.60 points out of 4.60 Flag question Question text What is the freezing point of a solution made from 22.0 g of octane (C8H18) dissolved in 148.0 g of benzene? (For benzene, freezing point = 5.50°C; Kf = 5.12°C/m) Select one: a. –1.16°C b. 0.98°C c. 6.66°C d. 12.2°C e. 5.49°C Question 10 Correct 4.60 points out of 4.60 Flag question Question text What volume of water (d = 1.00 g/mL) should be added to 600. mL of ethanol in order to have a solution that boils at 95.0°C? (For ethanol, Kb = 1.22 °C/m; density = 0.789 g/cm3; boiling point = 78.4°C) Select one: a. 186 mL b. 245 mL c. 518 mL d. 116 mL e. 322 mL Question 11 Correct 4.60 points out of 4.60 Flag question Question text What is the name for a solute that does not exert a vapor pressure when it is dissolved in a liquid? Select one: a. Colloid b. Amorphous solid c. Nonvolatile d. Crystalline solid e. Electrolyte Question 12 Correct 4.60 points out of 4.60 Flag question Question text The solubility of nitrogen gas in water at 25°C and a nitrogen pressure of 522 mmHg is 4.7 × 10–4 mol/L. What is the value of the Henry's law constant in mol L–1• atm–1? Select one: a. 6.8 × 10–4 mol L–1• atm–1 b. 4.7 × 10–4 mol L–1• atm–1 c. 3.2 × 10–4 mol L–1• atm–1 d. 9.0 × 10–7 mol L–1• atm–1 e. 1.5 × 103 mol L–1• atm–1 Question 13 Correct 4.60 points out of 4.60 Flag question Question text What is the name given to a solution that contains more solute than it has the capacity to dissolve? Select one: a. Unsaturated b. Saturated c. Soluted d. Supersaturated e. Oversaturated Question 14 Correct 4.60 points out of 4.60 Flag question Question text What mass of ethanol (C2H5OH), a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at –10.0°C? Assume the density of water is 1.0 g/mL. (Kf of water is 1.86°C/m.) Select one: a. 85.7 kg b. 24.8 kg c. 5.38 kg d. 2.48 kg e. 1.17 kg Question 15 Correct 4.60 points out of 4.60 Flag question Question text What is [OH–] for a solution at 25°C that has [H3O+] = 8.23 × 10–2 M? Select one: a. 8.23 × 10–2 M b. 1.22 × 10–6 M c. 8.23 × 10–12 M d. 1.22 × 10–13 M e. 8.23 × 10–16 M Question 16 Incorrect 0.00 points out of 4.60 Flag question Question text A solution is prepared by adding 0.10 mol of iron(III) nitrate, Fe(NO3)3, to 1.00 L of water. Which statement about the solution is correct? Select one: a. The solution is basic. b. The solution is neutral. c. The solution is acidic. d. The value of Ka for the species in solution must be known before a prediction can be made. e. The value of Kb for the species in solution must be known before a prediction can be made. Question 17 Correct 4.60 points out of 4.60 Flag question Question text Which one of these salts will form an acidic solution upon dissolving in water? Select one: a. LiBr b. NaF c. NH4Br d. KOH e. NaCN Question 18 Correct 4.60 points out of 4.60 Flag question Question text Which statement is true regarding the reversible reaction below? H2CO3+ F– HCO3+ HF. Ka1(H2CO3) = 4.2 × 10–7; Ka(HF) = 7.1 × 10–4 Select one: a. At equilibrium, [HF] > [H2CO3] because HF is a stronger acid than H2CO3. b. At equilibrium, [HF] > [H2CO3] because H2CO3 is a stronger acid than HF. c. At equilibrium, [HF] = [H2CO3]. d. At equilibrium, [H2CO3] > [HF] because HF is a stronger acid than H2CO3. e. At equilibrium, [H2CO3] > [HF] because H2CO3 is a stronger acid than HF. Question 19 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is the correct Kb expression for the reaction below? B(aq) + H2O(l) HB+(aq) + OH–(aq) Select one: a. Kb = [B][H2O] b. c. d. e. Kb = [HB+][OH–] Question 20 Incorrect 0.00 points out of 4.60 Flag question Question text What is the H+ ion concentration in a 2.1 × 10–4 M Ca(OH)2 solution? Select one: a. 7.3 × 10–4 M b. 4.2 × 10–4 M c. 2.1 × 10–4 M d. 2.4 × 10–11 M e. 4.8 × 10–11 M Question 21 Correct 4.60 points out of 4.60 Flag question Question text Which is a basic oxide? Select one: a. NO2 b. H2O c. Na2O d. SnO e. SO2 Question 22 Correct 4.60 points out of 4.60 Flag question Question text What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 × 10–5] Select one: a. 3.74 b. 4.98 c. 6.53 d. 9.02 e. 11.28 Question 23 Correct 4.60 points out of 4.60 Flag question Question text In the reaction, HSO4–(aq) + OH–(aq) SO42–(aq) + H2O(l), the conjugate acid-base pairs are pair 1 pair 2 Select one: a. HSO4– and SO42–; H2O and OH–. b. HSO4– and H3O+; SO42 – and OH–. c. HSO4– and OH–; SO42 – and H2O. d. HSO4– and H2O; OH – and SO42–. e. HSO4– and OH–; SO42 – and H3O+. Question 24 Correct 4.60 points out of 4.60 Flag question Question text Which is an acidic oxide? Select one: a. P4O10 b. MgO c. Fe2O3 d. K2O e. Cr2O3 Question 25 Correct 4.60 points out of 4.60 Flag question Question text What is [OH–] for a solution at 25°C that has [H3O+] = 2.35 × 10–3 M? Select one: a. 4.26 × 10–5 M b. 2.35 ×10–11 M c. 4.26 × 10–12 M d. 2.35 × 10–17 M e. 2.35 ×10–3 M [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 6 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 16: Nonmetallic Elements and Organic Chemistry Started on Friday, April 15, 2022, 9:09 PM State Finished Complet... [Show More] ed on Friday, April 15, 2022, 9:31 PM Time taken 22 mins 2 secs Grade 110.40 out of 115.00 (96%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text What is ΔS° for the following reaction? 4Cr(s) + 3O2(g) → 2Cr2O3(s) Substance Cr(s) O2(g) Cr2O3(s) S°(J/K • mol) 23.77 205.138 80.65 Select one: a. –549.19 J/K • mol b. –148.26 J/K • mol c. +148.26 J/K • mol d. +66.22 J/K • mol e. +871.80 J/K • mol Question 2 Correct 4.60 points out of 4.60 Flag question Question text A spontaneous reaction Select one: a. is always exothermic. b. may be exothermic or endothermic. c. is always endothermic. d. does not involve any heat exchange with surroundings. Question 3 Correct 4.60 points out of 4.60 Flag question Question text Which is the thermodynamic condition for a spontaneous process at constant T and P? Select one: a. ΔS > 0 b. ΔS < 0 c. ΔG < 0 d. ΔG > 0 e. ΔG° = 0 Question 4 Correct 4.60 points out of 4.60 Flag question Question text Consider the following redox equation. Mn(OH)2(s) + MnO4–(aq) → MnO42–(aq) (basic solution) When the equation is balanced with the smallest whole number coefficients, what is the coefficient for OH–(aq) and on which side of the equation is OH–(aq) present? Select one: a. 4, reactant side b. 4, product side c. 6, reactant side d. 6, product side e. 8, reactant side Question 5 Correct 4.60 points out of 4.60 Flag question Question text Which statement is correct? Select one: a. The cathode is the electrode where the oxidation takes place. b. The cathode is the electrode where the reduction takes place. c. Both oxidation and reduction make take place at the cathode, depending on the cell. d. The cathode is always positive. e. The anode is always negative. Question 6 Correct 4.60 points out of 4.60 Flag question Question text Which one of the following statements relating to the glass electrode is correct? Select one: a. The glass electrode detects hydrogen gas. b. The glass of a glass electrode serves to conduct electrons. c. When pH is measured, only a single electrode, the glass electrode, need be used. d. The potential of the glass electrode varies linearly with the pH of the solution. e. None of these statements is correct. Question 7 Correct 4.60 points out of 4.60 Flag question Question text Two cells are connected in series, so that the same current flows through two electrodes, where the following half-reactions occur: Cu2+(aq) + 2e– → Cu(s) and Ag+(aq) + e– → Ag(s) For every 1.00 g of copper produced in the first process, how many grams of silver will be produced in the second one? Select one: a. 0.294 g Ag b. 0.588 g Ag c. 0.850 g Ag d. 1.70 g Ag e. 3.40 g Ag Question 8 Correct 4.60 points out of 4.60 Flag question Question text Iodine-131, t1/2 = 8.0 days, is used in the diagnosis and treatment of thyroid gland diseases. If a laboratory sample of iodine-131 initially emits 9.95 × 1018 β particles per day, how long will it take for the activity to drop to 6.22 × 1017 β particles per day? Select one: a. 2.0 days b. 16 days c. 32 days d. 128 days e. None of the answers is correct. Question 9 Correct 4.60 points out of 4.60 Flag question Question text The dose unit of ionizing radiation is called the rad. The rad is defined in terms of Select one: a. the half-life of a radioisotope. b. the energy deposited per gram of an object. c. the biological damage produced. d. the accumulation of fission products. e. the number of ions per centimeter. Question 10 Correct 4.60 points out of 4.60 Flag question Question text Alpha particles are identical to Select one: a. protons. b. helium atoms. c. hydrogen atoms. d. helium nuclei. e. electrons. Question 11 Correct 4.60 points out of 4.60 Flag question Question text In the following reaction, identify X. Select one: a. b. c. d. e. Question 12 Correct 4.60 points out of 4.60 Flag question Question text Which of the following ions could exist in only the high-spin state in an octahedral complex? Select one: a. Cr2+ b. Mn4+ c. Fe3+ d. Co3+ e. Ni2+ Question 13 Correct 4.60 points out of 4.60 Flag question Question text Iron(III) forms an octahedral complex with the ligand CN–. How many unpaired electrons are in the d orbitals of iron? Select one: a. 1 b. 3 c. 5 d. 7 e. 9 Question 14 Correct 4.60 points out of 4.60 Flag question Question text Which of these atoms is the most electronegative? Select one: a. Si b. Cl c. P d. F e. C Question 15 Incorrect 0.00 points out of 4.60 Flag question Question text How many resonance structures does the sulfur dioxide molecule have? Select one: a. 0 b. 3 c. 1 d. 2 e. 4 Question 16 Correct 4.60 points out of 4.60 Flag question Question text Which of these pairs consists of isoelectronic species? Select one: a. Zn2+ and Cu2+ b. Cl– and S c. Na+ and K+ d. Mn2+ and Ar e. K+ and Cl– Question 17 Correct 4.60 points out of 4.60 Flag question Question text What products are formed from the reaction of Cl2(g) with I–(aq)? Select one: a. ICl b. ICl2 c. ICl3 d. I2 and Cl– e. I and Cl2– Question 18 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is the strongest acid? Select one: a. HClO3 b. HBrO3 c. HIO3 d. HIO2 e. HClO Question 19 Correct 4.60 points out of 4.60 Flag question Question text The nitrate anion is Select one: a. a strong acid. b. a strong base. c. amphoteric. d. a strong reducing agent. e. a strong oxidizing agent. Question 20 Correct 4.60 points out of 4.60 Flag question Question text Which of the following is a metalloid? Select one: a. Al b. Sn c. As d. Se e. Bi Question 21 Correct 4.60 points out of 4.60 Flag question Question text Which is NOT a hydride? Select one: a. b. c. d. e. Question 22 Correct 4.60 points out of 4.60 Flag question Question text Which of these elements is the most abundant in the universe? Select one: a. Hydrogen b. Nitrogen c. Carbon d. Oxygen e. Sodium Question 23 Correct 4.60 points out of 4.60 Flag question Question text What process involves the addition of a hydrogen molecule to compounds containing multiple bonds? Select one: a. Hydration b. Alkanation c. Hydrogenation d. Esterification e. Coagulation Question 24 Correct 4.60 points out of 4.60 Flag question Question text Which one of these compounds will result from the addition of HCl to CH3−CH=CH2? Select one: a. CH3Cl + CH2=CH2 b. CH3−CHCl=CH2 c. CH3−CHCl–CH3 d. CH3−CH2−CH2Cl e. None of these choices is correct. Question 25 Correct 4.60 points out of 4.60 Flag question Question text Which one of these materials is a copolymer? Select one: a. Polystyrene-polybutadiene b. Polyvinyl chloride c. Polypropylene d. Poly-cis-isoprene e. Polyethylene [Show Less]
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STRAIGHTERLINE CHEM 101 GENERAL CHEMISTRY GRADED EXAM 6 - APRIL 2022
Page path • CHEM101_MH_V4 • Topic 16: Nonmetallic Elements and Organic Chemistry Started on Thursday, March 24, 2022, 11:12 AM State Finished Comp... [Show More] leted on Thursday, March 24, 2022, 11:48 AM Time taken 36 mins 25 secs Grade 110.40 out of 115.00 (96%) Question 1 Correct 4.60 points out of 4.60 Flag question Question text What is ΔS° at 298 K for the following reaction? Fe2O3(s) + 3CO(g) → 3CO2(g) + 2Fe(s) Substance ΔG°f(kJ/mol) ΔH°f(kJ/mol) Fe2O3(s) –741.0 –822.2 CO(g) –137.2 –110.5 CO2(g) –394.4 –393.5 Select one: a. 12.7 J/K • mol b. –12.7 J/K • mol c. 527.9 J/K • mol d. 157.2 J/K • mol e. 4.6 J/K • mol Question 2 Correct 4.60 points out of 4.60 Flag question Question text In a spontaneous exothermic process, Select one: a. system heats up while surroundings lose energy. b. surroundings heat up, but there is no change in system’s energy. c. system loses energy while surroundings heat up. d. system heats up but there is not change in the energy of surroundings. e. energy content of neither system nor surroundings changes. Question 3 Correct 4.60 points out of 4.60 Flag question Question text Ozone (O3) in the atmosphere can react with nitric oxide (NO) as follows. O3(g) + NO(g) → NO2(g) + O2(g). ΔH°rxn = –199 kJ/mol, ΔS°rxn = –4.1 J/K • mol What is ΔG°rxn for this reaction at 25°C? Select one: a. 1020 kJ/mol b. –1.22 × 103 kJ/mol c. 2.00 × 103 kJ/mol d. –1.42 × 103 kJ/mol e. –198 kJ/mol Question 4 Correct 4.60 points out of 4.60 Flag question Question text Which is not a redox reaction? Select one: a. Al(OH)4–(aq) + 4H+(aq) → Al3+(aq) + 4H2O(l) b. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) c. Na6FeCl8(s) + 2Na(l) → 8NaCl(s) + Fe(s) d. 2H2O2(aq) → 2H2O(l) + O2(g) e. CO2(g) + H2(g) → CO(g) + H2O(g) Question 5 Correct 4.60 points out of 4.60 Flag question Question text What is the name given to the experimental apparatus for generating electricity through the use of a spontaneous reaction? Select one: a. Electrolytic cell b. Galvanic cell c. Redox cell d. Cathode e. Anode Question 6 Correct 4.60 points out of 4.60 Flag question Question text What product forms at the cathode during the electrolysis of molten lithium iodide? Select one: a. Li+(l) b. Li(l) c. I–(l) d. I2(g) e. I3–(l) Question 7 Correct 4.60 points out of 4.60 Flag question Question text Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? Select one: a. b. c. d. e. Question 8 Correct 4.60 points out of 4.60 Flag question Question text Rubidium-87 decays by beta decay with a half-life of 4.9 × 1010 yr. How many 87Rb atoms are in a moon rock sample that has a rubidium decay rate of 3500 disintegrations per hour? Select one: a. 9.0 × 1016 atoms b. 4.3 × 10–4 atoms c. 2.2 × 1018 atoms d. 2.5 × 1014 atoms e. 1.7 × 1014 atoms Question 9 Correct 4.60 points out of 4.60 Flag question Question text Calculate the energy released in joules when one mole of polonium-214 decays according to the following equation. Particle Mass (amu) Pb-210 209.98284 Po-214 213.99519 He-4 4.00260 (1 kg = 6.022 × 1026 amu; NA = 6.022 × 1023 mol–1; c = 2.99792458 × 108 m/s) Select one: a. 8.78 × 1014 J/mol b. 7.2 × 1014 J/mol c. 8.76 × 1011 J/mol d. –9.75 × 10–3 J/mol e. 1.46 × 10–9 J/mol Question 10 Correct 4.60 points out of 4.60 Flag question Question text Uranium-235 decays by alpha emission. What isotope is also produced by this transformation? Select one: a. Pa-234 b. Th-237 c. Pu-237 d. Th-231 e. Pu-239 Question 11 Incorrect 0.00 points out of 4.60 Remove flag Question text In the following reaction, identify X. Select one: a. 7β b. 3α c. 4n d. e. 15p Question 12 Correct 4.60 points out of 4.60 Flag question Question text In the complex ion [Co(en)2Br2]+, what is the oxidation number of Co? Select one: a. +1 b. +2 c. +3 d. –2 e. –1 Question 13 Correct 4.60 points out of 4.60 Flag question Question text Which of the following ligands is most likely to form a high-spin octahedral complex with cobalt(II)? Select one: a. CN– b. en (ethylenediamine) c. NH3 d. CO e. I– Question 14 Correct 4.60 points out of 4.60 Flag question Question text Which of these atoms is the most electronegative? Select one: a. Si b. Cl c. P d. F e. C Question 15 Correct 4.60 points out of 4.60 Flag question Question text Which of these elements is most likely to exhibit an expanded octet in its compounds? Select one: a. C b. O c. N d. S e. Na Question 16 Correct 4.60 points out of 4.60 Flag question Question text Which of these pairs consists of isoelectronic species? Select one: a. Zn2+ and Cu2+ b. Cl– and S c. Na+ and K+ d. Mn2+ and Ar e. K+ and Cl– Question 17 Correct 4.60 points out of 4.60 Flag question Question text What products are formed from the reaction of Cl2(g) with I–(aq)? Select one: a. ICl b. ICl2 c. ICl3 d. I2 and Cl– e. I and Cl2– Question 18 Correct 4.60 points out of 4.60 Flag question Question text Which oxide is an amphoteric oxide? Select one: a. Na2O b. Al2O3 c. BaO d. SiO2 e. More that one of these oxides are amphoteric. Question 19 Correct 4.60 points out of 4.60 Flag question Question text The strongest elemental oxidizing agents are found in the _________ _________ region of the periodic table while the strongest reducing agents are found in the ________ ________ region of the periodic table. Select one: a. upper left, lower right b. upper right, lower left c. lower left, upper right d. lower right, upper left e. transition element, main group Question 20 Correct 4.60 points out of 4.60 Flag question Question text Which would exhibit characteristics of both a metal and a nonmetal? Select one: a. Si b. Ge c. Sb d. Po e. All of the above exhibit characteristics of both a metal and a nonmetal. Question 21 Correct 4.60 points out of 4.60 Flag question Question text What group of the periodic table is the element with the electron configuration [Ar]4s23d104p2? Select one: a. 4A b. 3A c. 5A d. 2A e. 6A Question 22 Correct 4.60 points out of 4.60 Flag question Question text Which is NOT true concerning sulfur? Select one: a. Sulfur reacts with carbon to form a flammable liquid. b. Sulfur reacts with fluorine to form an inert compound. c. Sulfur reacts with oxygen to form a strongly acid oxide. d. Sulfur reacts with hydrogen to form a pungent, foul-smelling gas. e. In its solid elemental form, sulfur exists as an eight-membered ring. Question 23 Correct 4.60 points out of 4.60 Flag question Question text Which reaction represents the disproportionation of hydrogen peroxide? Select one: a. b. c. d. e. Question 24 Correct 4.60 points out of 4.60 Flag question Question text What name is given to a compound containing a –CHO group? Select one: a. Aldehyde b. Ketone c. Alcohol d. Carboxylic acid e. Ester Question 25 Correct 4.60 points out of 4.60 Flag question Question text Which one of these materials is a copolymer? Select one: a. Polystyrene-polybutadiene b. Polyvinyl chloride c. Polypropylene d. Poly-cis-isoprene e. Polyethylene [Show Less]
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