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Straighterline CHEM101 General Chemistry I Graded Exams 1, 2, 3, 4 & Midterm (New Version June 2024
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Straighterline CHEM101 General Chemistry I Graded Exam 4 (New Version June 2024)
Question 1 Correct 5.00 points out of 5.00 According to which scientific law does the entropy of the universe increase in spontaneous processes and re... [Show More] main unchanged in equilibrium processes? Select one: A. 1st universal law B. 1st law of entropy C. 2nd law of thermodynamics D. 3rd law of thermodynamics E. 1st law of thermodynamics Straighterline CHEM101 General Chemistry I Graded Exam 4 (New Version June 2024) We are a team of experts offering class attendance for all Straighterline, Online ATI, HESI, NCLEX, Portage Learning, Sophia etc courses (including final proctored exams!!). We also write essays, discussion posts, research papers and school assignments. Should you need any of these services, Contact us via email: [email protected] or WhatsApp: +1 (540) 753-5914. Guaranteed Passing! CHEM101_MH_V6 | Topic 18: Organic Chemistry Started on State Finished Completed on Time taken 47 mins 20 secs GradeQuestion 3 Correct 5.00 points out of 5.00 The heat of vaporization of 1-pentanol is 55.5 kJ/mol, and its entropy of vaporization is . What is the approximate boiling point of 1-pentanol? Select one: A. 0°C B. 100°C C. 375°C D. 25°C Question 2 Correct 5.00 points out of 5.00 What is ΔS° for the following reaction? 4Cr(s) + 3O2(g) → 2Cr2O3(s) Substance S° (J/K • mol) Cr(s) 23.77 O2(g) 205.138 Cr2O3(s) 80.65 Select one: A. –549.19 J/K • mol B. +66.22 J/K • mol C. +148.26 J/K • mol D. +871.80 J/K • mol E. –148.26 J/K • molThe temperature at which the following process reaches equilibrium at 1.0 atm is the normal melting point for phosphoric acid. H3PO4(s) H3PO4(l) Use the following thermodynamic data at 298 K to estimate this temperature. A. 315 K B. 3170 K C. 347 K D. 305 K E. 286 K Question 5 Correct 5.00 points out of 5.00 Which of the following results in a decrease in the entropy of the system? Select one: A. NH3(l), –34.5°C → NH3(g), –34.5°C B. 2H2O2(g) → 2H2O(g) + O2(g) C. N2(g), 25°C → N2(aq), 25°C D. H2O(s), 0°C → H2O(l), 0°C E. O2(g), 300 K → O2(g), 400 K Substance: H3PO4(s) H3PO4(l) ΔH°f (kJ/mol): –1284.4 –1271.7 ΔG°f (kJ/mol): –1124.3 –1123.6 S°(J/K • mol): Select one: 110.5 150.8 Question 4 Correct 5.00 points out of 5.00Question 7 Correct 5.00 points out of 5.00 Identify the missing species in the following nuclear transmutation. U-238 + ? → 1 neutron + Fm-249 Select one: A. Al B. Al C. Li D. O E. O Question 6 Correct 5.00 points out of 5.00 Consider the figure below which shows ΔG° for a chemical process plotted against absolute temperature. From this plot, it is reasonable to conclude that: Select one: A. B. C. D. E. None of these choices is correct.Question 9 Incorrect 0.00 points out of 5.00 What other particle is emitted when a neutron is converted to a proton in a nucleus? Select one: A. Beta particle B. Alpha particle C. Positron D. Gamma particle E. None of the answers is correct. Question 8 Incorrect 0.00 points out of 5.00 A mass of 6.02 × 1026 amu is equivalent to Select one: A. 1 g. B. 1 kg. C. 1 mol. D. 1 mg. E. 1 J.Question 11 Correct 5.00 points out of 5.00 Which of the following is used to image the liver? Select one: A. 131I B. 123I C. 99Tc D. 24Na E. 18O Question 10 Incorrect 0.00 points out of 5.00 In the following diagrams, A represents a radioactive isotope that decays into a new isotope, X. Each circle represents 1 mmol of atoms. t = 0: t = 25.0 s: Over the first 25.0 s, what is the disintegration rate of A? Select one: A. 7.23 × 1019 disintegrations per second B. 1.38 × 10–20 disintegrations per second C. 3.00 disintegrations per second D. 0.120 disintegrations per second E. 1.81 × 1021 disintegrations per secondQuestion 13 Correct 5.00 points out of 5.00 How many 4d electrons does a ground-state Cd2+ ion have? Select one: A. 7 B. 2 C. 9 D. 10 E. 8 Question 14 Correct 5.00 points out of 5.00 Which of the following ligands has two different types of donor atoms? Select one: A. NH4+ B. H2O C. NH3 D. NO2– E. ethylenediamine Question 12 Correct 5.00 points out of 5.00 What is the energy equivalent of 1 amu? (c = 2.99792458 × 108 m/s) Select one: A. 6.6 × 109 J B. 5.4 × 1043 J C. 1.5 × 10–10 J D. 5.0 × 10–19 JQuestion 16 Correct 5.00 points out of 5.00 In the complex ion [Fe(CN)6]4–, what is the oxidation number of Fe? Select one: A. +1 B. –4 C. +3 D. +6 E. +2 Question 17 Correct 5.00 points out of 5.00 What is the coordination number of cobalt in the complex ion [Co(en)Cl4]–? (en = ethylenediamine) Select one: A. 6 B. 2 C. 8 D. 1 E. 4 Question 15 Correct 5.00 points out of 5.00 Which of these square planar complex ions can have cis-trans isomers? Select one: A. [Pt(NH3)Cl3]– B. [Pt(NH3)4]2+ C. [Ni(NH3)4]2+ D. [Ni(NH3)3Cl]+ E. [Pt(NH3)2Cl2]Question 19 Correct 5.00 points out of 5.00 What is the systematic name for Cr(CO)3(NH3)3? Select one: A. triamminechromium carbonate B. chromiumtriaminotricarbonyl C. triamminetricarbonylchromate(0) D. tris(amino)tris(carbonyl)chromium E. triamminetricarbonylchromium(0) Question 20 Correct 5.00 points out of 5.00 Silicon carbide is an important industrial chemical. Which of the following statements about silicon carbide is true? Select one: A. It is the hardest known substance. B. It is used for cutting, grinding, and polishing metals and glasses. C. It is used in the preparation of glass which can be used at high temperature. D. It is a naturally occurring mineral source of silicon. E. It will react with water to form acetylene. Question 18 Correct 5.00 points out of 5.00 In the complex ion [Co(en)2Br2]+, what is the oxidation number of Co? Select one: A. +3 B. –1 C. +2 D. –2 E. +1Question 22 Incorrect 0.00 points out of 5.00 What is the formal charge on the iodine atom in the iodate ion, IO3–? Select one: A. –1 B. +2 C. +1 D. –2 E. 0 Question 23 Correct 5.00 points out of 5.00 What is the formal charge on sulfur in the best Lewis structure for the SCN–? Select one: A. –2 B. 0 C. –1 D. +1 E. +2 Question 21 Correct 5.00 points out of 5.00 Which of these compounds is most likely to be covalent? Select one: A. NF3 B. CaO C. Sr(NO3)2 D. LiF E. CsOHQuestion 25 Correct 5.00 points out of 5.00 What is the general electron configuration for atoms of all elements in Group 5A? Select one: A. ns2np3 B. ns2np4 C. ns2np5 D. ns2np1 E. ns2np6 Quiz navigation 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 Show one page at a time Finish review Question 24 Correct 5.00 points out of 5.00 In their elemental forms, the halogens are Select one: A. strong bases. B. strong reducing agents. C. strong oxidizing agents. D. amphoteric. E. strong acids.© 2023 StraighterLine. All rights reserved [Show Less]
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Straighterline CHEM101 General Chemistry I Graded Exam 3 (New Version June 2024)
Question 1 Correct 5.00 points out of 5.00 If 2.38 mol of a gas has a volume of 120.0 mL, what is the volume of 1.97 mol of the gas at the same temper... [Show More] ature and pressure? Select one: A. 99.3 mL B. 119 mL C. 145 mL D. 25.6 mL E. 563 mL Question 2 Correct 5.00 points out of 5.00 What are the conditions of STP? Select one: A. 0°C and 760 atm B. 273.15°C and 760 torr C. 0 K and 1 atm D. 0°C and 1 torr E. 273.15 K and 760 torr Straighterline CHEM101 General Chemistry I Graded Exam 3 (New Version June 2024) We are a team of experts offering class attendance for all Straighterline, Online ATI, HESI, NCLEX, Portage Learning, Sophia etc courses (including final proctored exams!!). We also write essays, discussion posts, research papers and school assignments. Should you need any of these services, Contact us via email: [email protected] or WhatsApp: +1 (540) 753-5914. Guaranteed Passing! CHEM101_MH_V6 | Topic 14: Acid-Base Equilibria and Solubility Equilibria Started on State Finished Completed on Time taken 35 mins 28 secs GradeQuestion 4 Correct 5.00 points out of 5.00 Determine the molar mass of Freon-11 gas if a sample weighing 0.597 g occupies 100 cm3 at 95°C and 1000 mmHg (R = 0.08206 L • atm/K • mol, 1 atm = 760 mmHg). Select one: A. 70.9 g/mol B. 35.3 g/mol C. 0.19 g/mol D. 137 g/mol E. 384 g/mol What is the pressure in atmospheres exerted by a column of mercury that is 100. m high? (density of mercury = 13.5951 g/cm3, gravitational constant = 9.80665 m/s2, 1 atm = 101,325 Pa = 760 torr = 760 mmHg) Select one: A. 1.37 atm B. 0.013 atm C. 0.73 atm D. 132 atm E. 1.4 × 1010 atm Question 3 Correct 5.00 points out of 5.00Question 6 Correct 5.00 points out of 5.00 Which of the following gas molecules have the highest average kinetic energy at 25°C? Select one: A. H2 B. N2 C. O2 D. Cl2 E. All the gases have the same average kinetic energy. Question 7 Correct 5.00 points out of 5.00 Krypton has a higher melting point than argon because of its Select one: A. stronger dispersion forces. B. greater ionization energy. C. ionic bonds. D. permanent dipole moment. E. hydrogen bonding. 1.00 atm of oxygen gas, placed in a container having a pinhole opening in its side, leaks from the container 2.14 times faster than does 1.000 atm of an unknown gas placed in this same apparatus. Which of the following species could be the unknown gas? Select one: A. Cl2 B. Kr C. UF6 D. Xe E. SF6 Question 5 Correct 5.00 points out of 5.00Question 9 Correct 5.00 points out of 5.00 Which substance has the lowest vapor pressure at room temperature? Select one: A. H2 B. HCl C. HBr D. HI E. HF Question 10 Correct 5.00 points out of 5.00 Select the pair of substances in which the one with the higher vapor pressure at a given temperature is listed first. Select one: A. Xe, Kr B. H2O, H2S C. C7H16, C5H12 D. CCl4, CBr4 E. CH3CH2OH, CH3–O–CH3 If a molecule at the surface of a liquid has enough kinetic energy to escape the liquid phase and enter the gas phase, then which of the following terms is used to describe this phenomenon? Select one: A. Condensation B. Vaporization C. Gasification D. Sublimation E. Boiling point Question 8 Correct 5.00 points out of 5.00Question 12 Correct 5.00 points out of 5.00 Which one of the following substances crystallizes as a molecular solid? Select one: A. Sn B. SiO2 C. CH3OH D. KI E. Al2(SO4)3 Question 13 Correct 5.00 points out of 5.00 The density of a 20.3 M CH3OH (methanol) solution is 0.858 g/mL. What is the molality of this solution? H2O is the solvent. Select one: A. 70.0 m B. 20.8 m C. 97.8 m D. 23.7 m E. 17.4 m The location that indicates conditions under which two phases can exist in equilibrium is called the Select one: A. phase diagram. B. transition state. C. phase boundary. D. triple point. E. critical point. Question 11 Correct 5.00 points out of 5.00Question 15 Correct 5.00 points out of 5.00 Which of the following sets of conditions could exist when two liquids which are completely miscible in one another are mixed? Select one: A. ΔHsoln ≈ 0, entropy of system decreases B. ΔHsoln > 0, entropy of system decreases C. ΔHsoln ≈ 0, entropy of system increases D. ΔHsoln ≈ 0, entropy change of system ≈ 0 E. None of these choices is correct. From the following list of aqueous solutions and water, select the one with the highest boiling point. Select one: A. pure water B. 1.0 M KNO3 C. 2.0 M C12H22O11 (sucrose) D. 0.75 M CuCl2 E. 0.75 M NaCl Question 14 Correct 5.00 points out of 5.00Question 17 Correct 5.00 points out of 5.00 Which substance is present in the largest proportion in a solution? Select one: A. solvent B. solid C. solute D. salute E. gas Question 18 Correct 5.00 points out of 5.00 Which accurately characterizes all nonelectrolyte solutions? Select one: A. Nonelectrolyte solutions conduct heat. B. Nonelectrolyte solutions do not conduct electricity. C. Nonelectrolyte solutions conduct electricity. D. Nonelectrolyte solutions react with other solutions. E. Nonelectrolyte solutions contain molecules. What volume of ethanol (density = 0.7893 g/cm3) should be added to 450. mL of water in order to have a solution that freezes at –15.0°C? Assume the density of water is 1.0 g/mL. (For water, Kf = 1.86°C/m.) Select one: A. 470 mL B. 212 mL C. 132 mL D. 371 mL E. 167 mL Question 16 Correct 5.00 points out of 5.00Question 20 Correct 5.00 points out of 5.00 Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10–10) solution. Select one: A. 5.85 B. 8.71 C. 5.15 D. 13.0 E. 9.91 What is defined as the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated solution? Select one: A. Osmosis B. Vapor pressure C. Permeability D. Semipermeability E. Osmotic pressure Question 19 Correct 5.00 points out of 5.00Which one of the following is the best representation of the titration curve which will be obtained in the titration of a weak diprotic acid H2A (0.10 M) with a strong base of the same concentration? Select one: A. B. Question 21 Correct 5.00 points out of 5.00C. D. E.Suppose 3.0 × 10–3 mol of NaOH are added to 6.0 × 10–3 mol of the weak acid HA. Which is the best representation of the final solution at equilibrium? (Each circle represents 1.0 × 10–3 mol of atoms, and the volume of each box is 1.0 L. Solvent water molecules are omitted for clarity.) Select one: A. B. Question 22 Correct 5.00 points out of 5.00C. D. E.Question 24 Correct 5.00 points out of 5.00 What is the [H3O+] in a buffer that consists of 0.30 M HCOOH and 0.20 M HCOONa? [Ka(HCOOH) = 1.7 × 10–4] Select one: A. 1.1 × 10–4 M B. 2.6 × 10–4 M C. 1.7 × 10–4 M D. 4.3 × 10–4 M E. 6.7 × 10–5 M Question 25 Correct 5.00 points out of 5.00 If 50.0 mL of 1.2 × 10–3 M Pb(NO3)2 are added to 50.0 mL of 2.0 × 10–4 M Na2S, what takes place? Select one: A. A precipitate of PbS forms. B. A precipitate of Pb(NO3)2 forms. C. No precipitate forms. D. A precipitate of NaNO3 forms. E. A precipitate of Na2S forms. Which indicator would be the best to use if 0.050 M benzoic acid (Ka = 6.6 × 10–5) is titrated with 0.050 M NaOH? Select one: A. phenol red, pH range: 6.9–8.5 B. bromcresol green, pH range: 3.8–5.4 C. bromphenol blue, pH range: 3.0–4.5 D. alizarin, pH range: 5.7–7.2 Question 23 Correct 5.00 points out of 5.00© 2023 StraighterLine. All rights reserved Quiz navigation 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 Show one page at a time Finish review [Show Less]
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Straighterline CHEM101 General Chemistry I Graded Exam 1 (New Version June 2024)
Question 1 Correct 5.00 points out of 5.00 Talc is a mineral with low conductivity for heat and electricity which is not attacked by acid. It is used ... [Show More] in talcum powder and face powder. Suppose a sample of talc weighs 13.65 g with a density of 1.75 g/cm3 in mineral oil. If this same sample of talc in air weighs 35.97 g, assuming no volume change, what is the density of the talc sample in air? Select one: A. 2.44 g/cm3 B. 2.82 g/cm3 C. 1.61 g/cm3 D. 4.61 g/cm3 E. 2.63 g/cm3 Question 2 Correct 5.00 points out of 5.00 Which of the following represents the greatest mass? Select one: A. 3.0 × 1012 pg B. 2.0 × 103 mg C. 10.0 dg D. 1.0 × 106 µg E. 0.0010 kg Straighterline CHEM101 General Chemistry I Graded Exam 1 (New Version June 2024) We are a team of experts offering class attendance for all Straighterline, Online ATI, HESI, NCLEX, Portage Learning, Sophia etc courses (including final proctored exams!!). We also write essays, discussion posts, research papers and school assignments. Should you need any of these services, Contact us via email: [email protected] or WhatsApp: +1 (540) 753-5914. Guaranteed Passing! CHEM101_MH_V6 | Topic 5: Ionic and Covalent Compounds Started on State Finished Completed on Time taken 55 mins 20 secs GradeQuestion 4 Correct 5.00 points out of 5.00 The boiling point for liquid helium is 4.0 K. What is the temperature in degrees Fahrenheit? Select one: A. –452.5°F B. 530.9°F C. –237.2°F D. 131.8°F E. –498.9°F Question 5 Correct 5.00 points out of 5.00 The average distance between Earth and the Moon is 240,000 miles. Express this distance in meters. (1 mi = 1609 m) Select one: A. 5.3 × 105 m B. 1.5 × 105 m C. 6.1 × 105 m D. 3.9 × 108 m E. 9.4 × 104 m How many hertz is 600.11 MHz? Select one: A. 6.0011 × 106 Hz B. 6.0011 × 10–2 Hz C. 6.0011 × 108 Hz D. 6.0011 × 10–4 Hz E. 60.011 Hz Question 3 Correct 5.00 points out of 5.00Question 7 Incorrect 0.00 points out of 5.00 Which one of the following statements about atoms and subatomic particles is correct? Select one: A. The neutron's mass is equal to that of a proton plus an electron. B. A neutral atom contains equal numbers of protons and electrons. C. The proton and the neutron have identical masses. D. An atomic nucleus contains equal numbers of protons and neutrons. E. Rutherford discovered the atomic nucleus by bombarding gold foil with electrons. Question 8 Correct 5.00 points out of 5.00 In the periodic table, atoms are arranged in order of Select one: A. periodicity. B. chemical reactivities. C. physical properties. D. increasing atomic mass. E. increasing atomic number. Iron(III) chloride hexahydrate is used as a coagulant for sewage and industrial wastes. What is its formula? Select one: A. Fe(Cl·6H2O)3 B. Fe3Cl(H2O)6 C. FeCl3·6H2O D. FeCl3(H2O)6 E. Fe3Cl·6H2O Question 6 Incorrect 0.00 points out of 5.00Question 10 Correct 5.00 points out of 5.00 A row of the periodic table is called a(n) Select one: A. subshell. B. isotopic mixture. C. period. D. family. E. group. Question 11 Correct 5.00 points out of 5.00 The electron configuration of a ground-state copper atom is Select one: A. [Ar]3d9. B. [Ar]4s24p63d3. C. [Ar]4s23d9. D. [Ar]4s24d4. E. [Ar]4s13d10. Who discovered the neutron, the subatomic particle having a neutral charge? Select one: A. Chadwick B. Millikan C. Thomson D. Dalton E. Rutherford Question 9 Correct 5.00 points out of 5.00Question 13 Incorrect 0.00 points out of 5.00 The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of Select one: A. Kr. B. Ni. C. Pd. D. Fe. E. None of these choices is correct. Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10–27 kg and h = 6.63 × 10–34 J • s) Select one: A. 5.05 mm B. 1.8 × 1050 m C. 198 nm D. 216 nm E. 1.98 × 10–9 m Question 12 Correct 5.00 points out of 5.00Question 15 Correct 5.00 points out of 5.00 The orbital diagram for a ground-state nitrogen atom is Select one: A. A B. B C. C D. D E. E Which ground-state atom has an electron configuration described by the following orbital diagram? Select one: A. germanium B. tellurium C. selenium D. phosphorus E. potassium Question 14 Correct 5.00 points out of 5.00Question 17 Correct 5.00 points out of 5.00 An oxide ion, O2–, has Select one: A. 8 protons and 7 electrons. B. 10 protons and 8 electrons. C. 8 protons and 10 electrons. D. 10 protons and 7 electrons. E. 8 protons and 9 electrons. Question 18 Correct 5.00 points out of 5.00 Which of the following is an amphoteric oxide? Select one: A. SO2 B. Na2O C. MgO D. Cl2O7 E. Al2O3 Which one of these ions does not have [Xe] as its electronic configuration? Select one: A. I– B. Sn4+ C. Te2– D. Cs+ E. Ba2+ Question 16 Correct 5.00 points out of 5.00Question 20 Correct 5.00 points out of 5.00 In 1864, the English chemist John Newlands noticed that when the elements were arranged in order of increasing atomic mass, every eighth element had similar properties. Newlands referred to this relationship as the Select one: A. law of orbitals. B. law of octaves. C. law of proportionality. D. law of periodicity. E. law of loopholes. Each of the noble gases has a completely filled p subshell except for which one? Select one: A. Radon B. Argon C. Helium D. Xenon E. Neon Question 19 Correct 5.00 points out of 5.00Select the Lewis structure for XeO2F2 which correctly minimizes formal charges. Select one: A. B. C. D. Question 21 Correct 5.00 points out of 5.00Question 22 Correct 5.00 points out of 5.00 What formal charge resides on the carbon of CO32–? Select one: A. 0 B. +4 C. +1 D. +2 E. +3 Question 23 Correct 5.00 points out of 5.00 How many single bonds are bonded to sulfur in SF6? Select one: A. 2 B. 7 C. 4 D. 6 E. 8 E.Which of these elements is most likely to exhibit an expanded octet in its compounds? Select one: A. O B. Na C. C D. S E. N Question 24 Correct 5.00 points out of 5.00Quiz navigation 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 Show one page at a time Finish review Which of these choices is the best Lewis structure for ozone, O3? Select one: A. B. C. D. E. Question 25 Correct 5.00 points out of 5.00© 2023 StraighterLine. All rights reserved [Show Less]
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Straighterline CHEM101 General Chemistry I Graded Exam 2 (New Version June 2024)
Question 1 Correct 5.00 points out of 5.00 Aluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and the manufacture of antiperspi... [Show More] rants. Calculate its formula mass. Select one: A. 342.17 amu B. 315.15 amu C. 278.02 amu D. 74.98 amu E. 450.06 amu Question 2 Correct 5.00 points out of 5.00 Calculate the molar mass of sulfuric acid. Select one: A. 98.086 g/mol B. 49 g/mol C. 81.078 g/mol D. 41 g/mol E. None of the answers is correct. Straighterline CHEM101 General Chemistry I Graded Exam 2 (New Version June 2024) We are a team of experts offering class attendance for all Straighterline, Online ATI, HESI, NCLEX, Portage Learning, Sophia etc courses (including final proctored exams!!). We also write essays, discussion posts, research papers and school assignments. Should you need any of these services, Contact us via email: [email protected] or WhatsApp: +1 (540) 753-5914. Guaranteed Passing! CHEM101_MH_V6 | Topic 9: Energy Changes in Chemical Reactions Started on State Finished Completed on Time taken 59 mins 34 secs GradeQuestion 4 Correct 5.00 points out of 5.00 Balance the following equation for the combustion of benzene: C6H6(l) + O2(g) → H2O(g) + CO2(g) Select one: A. C6H6(l) + 9O2(g) → 6H2O(g) + 6CO2(g) B. 2C6H6(l) + 9O2(g) → 6H2O(g) + 12CO2(g) C. C6H6(l) + 9O2(g) → 3H2O(g) + 6CO2(g) D. C6H6(l) + 15O2(g) → 3H2O(g) + 6CO2(g) E. 2C6H6(l) + 15O2(g) → 6H2O(g) + 12CO2(g) Question 3 Correct 5.00 points out of 5.00 Aluminum metal reacts with chlorine gas to form solid aluminum chloride. What mass of chlorine gas is required to react completely with 163 g of aluminum? Select one: A. 214 g B. 643 g C. 428 g D. 321 g E. 286 gQuestion 6 Correct 5.00 points out of 5.00 What is the mass of 7.80 × 1018 carbon atoms? (NA = 6.022 × 1023 mol–1) Select one: A. 7.80 × 1018 g B. 6.43 × 103 g C. 1.56 × 10–4 g D. 12.01 g E. 1.30 × 10–5 g Question 5 Correct 5.00 points out of 5.00 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.) SF4 + H2O → H2SO3 + HF Select one: A. 4 B. 9 C. 6 D. 7 E. None of these answers is correct.Question 8 Incorrect 0.00 points out of 5.00 A system which does work on the surroundings with no heat change (i.e., q = 0) has Select one: A. w > 0, ΔU > 0. B. w < 0, ΔU < 0. C. w < 0, ΔU = 0. D. w > 0, ΔU < 0. E. w < 0, ΔU > 0. Question 7 Correct 5.00 points out of 5.00 Balance the following equation: C8H18O3(l) + O2(g) → H2O(g) + CO2(g) Select one: A. C8H18O3(l) + 11O2(g) → 9H2O(g) + 8CO2(g) B. 2C8H18O3(l) + 22O2(g) → 9H2O(g) + 16CO2(g) C. 2C8H18O3(l) + 17O2(g) → 18H2O(g) + 16CO2(g) D. C8H18O3(l) + 13O2(g) → 18H2O(g) + 8CO2(g) E. C8H18O3(l) + 8O2(g) → 9H2O(g) + 8CO2(g)Question 10 Correct 5.00 points out of 5.00 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 CO(g) Al2O3(s) –110.5 –1669.8 Select one: A. 310.0 kJ B. 412.4 kJ C. 386.8 kJ D. 773.6 kJ E. 824.8 kJ Question 9 Correct 5.00 points out of 5.00 An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide according to the following balanced chemical equation. What is ΔH°rxn for this reaction? 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) Substance NH3(g) NO(g) H2O(g) (kJ/mol) –46.3 90.3 –241.8 Select one: A. –240.2 kJ/mol B. –1274.8 kJ/mol C. –197.8 kJ/mol D. –904.4 kJ/mol E. 197.8 kJ/molQuestion 12 Correct 5.00 points out of 5.00 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. w = 0 B. C. D. E. q = 0 Suppose a new metallic element X is discovered, and its reactions with oxygen gas and chlorine gas at 298 K are studied. Trial Reaction ΔH°rxn (kJ/mol) 1 4X(s) + 3O2(g) → 2X2O3(s) 600 2 2X(s) + 3Cl2(g) → 2XCl3(s) 800 3 4XCl3(s) + 3O2(g) → 2X2O3(s) + 6Cl2(g) 200 However, it is later discovered that one of the samples was contaminated, and the ΔH°rxn value from this trial is not reliable. Which trial had the contaminated sample, and what should the correct value of ΔH° rxn be for this trial? Select one: A. Trial 1 had the contaminated sample; its ΔH°rxn value should be –900 kJ/mol. B. Trial 2 had the contaminated sample; its ΔH°rxn value should be +100 kJ/mol. C. Trial 3 had the contaminated sample; its ΔH°rxn value should be +1000 kJ/mol. D. Trial 3 had the contaminated sample; its ΔH°rxn value should be –1000 kJ/mol. E. Not enough information is provided; all three trials must be redone. Question 11 Correct 5.00 points out of 5.00Question 14 Incorrect 0.00 points out of 5.00 What is the molecular geometry of NO2– as predicted by the VSEPR model? Select one: A. tetrahedral B. bent C. trigonal pyramidal D. linear E. trigonal planar Question 15 Correct 5.00 points out of 5.00 Consider the species N2–, N2, and N2+. Which of these species will be paramagnetic? Select one: A. N2+ and N2– B. N2 and N2– C. N2–, N2, and N2+ D. N2+ and N2 E. None is paramagnetic. Question 13 Correct 5.00 points out of 5.00 To which one of the following reactions, occurring at 25°C, does the symbol ΔH°f [H2SO4(l)] refer? Select one: A. H2(g) + S(s) + 2 O2(g) < ---- > H2SO4(l) B. H2(g) + S(g) + 2 O2(g) <---- > H2SO4(l) C. 2 H(g) + S(g) + 4 O(g) <---- > H2SO4(l) D. H2SO4(l) < ---- > H2(g) + S(s) + 2 O2(g) E. H2SO4(l) < ---- > 2 H(g) + S(s) + 4 O(g)Question 17 Correct 5.00 points out of 5.00 What does the abbreviation VSEPR stand for? Select one: A. Very Selective Electron Pair theory B. Valence Shell for Every Proton C. Very Specific Electron and Proton Repair D. Valence-Shell Electron-Pair Repulsion E. Variable Selective of Electron and Protons Question 18 Correct 5.00 points out of 5.00 According to the VSEPR model, which molecule is predicted to be linear? Select one: A. BF3 B. H2CO C. H2S D. HCN E. SO3 Question 16 Correct 5.00 points out of 5.00 A molecule with the formula AB3 and a trigonal planar molecular geometry uses to form its σ bonds. Select one: A. sp3d2 hybrid orbitals B. sp3d hybrid orbitals C. sp hybrid orbitals D. sp2 hybrid orbitals E. sp3 hybrid orbitalsQuestion 20 Correct 5.00 points out of 5.00 Which one of these salts will form an acidic solution upon dissolving in water? Select one: A. NaCN B. NH4Br C. KOH D. LiBr E. NaF Question 19 Correct 5.00 points out of 5.00 According to molecular orbital theory, what is the bond order in the O2+ ion? Select one: A. 2.5 B. 5.5 C. 4 D. 1.5 E. 5Question 22 Incorrect 0.00 points out of 5.00 Which is the weakest acid? Select one: A. HBrO B. HBrO4 C. HBrO3 D. HBrO2 E. HBr Question 21 Correct 5.00 points out of 5.00 Below is a representation of an aqueous solution of a weak acid HA at equilibrium. (Each circle represents 1.0 × 10–3 mol of atoms, and the volume of the box is 1.0 L. Solvent water molecules are not shown for clarity.) What is the pH of the solution? Select one: A. 11.6 B. 11.0 C. 2.1 D. 3.0 E. 2.4Question 24 Correct 5.00 points out of 5.00 A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this acid? Select one: A. 2.7 × 10–4 B. 7.2 × 101 C. 9.9 × 10–2 D. 1.4 × 10–3 E. 1.6 × 10–1 Question 25 Incorrect 0.00 points out of 5.00 Find the pH of a 0.183 M aqueous solution of hypobromous acid (HOBr), for which . Select one: A. 4.712 B. 0.738 C. 4.576 D. 8.686 E. 9.288 Question 23 Correct 5.00 points out of 5.00 Which one of the following is a strong acid? Select one: A. H3PO4 B. CH3COOH C. HClO3 D. NH3 E. H2SO3© 2023 StraighterLine. All rights reserved Quiz navigation 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 Show one page at a time Finish review [Show Less]
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Straighterline CHEM101 General Chemistry I Midterm Exam (New Version June 2024)
Question 1 Correct 4.00 points out of 4.00 The SI base unit of mass is Select one: A. g. B. metric ton. C. mg. D. lb. E. kg. Question 2 Correct... [Show More] 4.00 points out of 4.00 The boiling point for liquid nitrogen is 77 K. What is the temperature in degrees Fahrenheit? Select one: A. –289°F B. –321°F C. –127°F D. 662°F E. 177°F Straighterline CHEM101 General Chemistry I Midterm Exam (New Version June 2024) We are a team of experts offering class attendance for all Straighterline, Online ATI, HESI, NCLEX, Portage Learning, Sophia etc courses (including final proctored exams!!). We also write essays, discussion posts, research papers and school assignments. Should you need any of these services, Contact us via email: [email protected] or WhatsApp: +1 (540) 753-5914. Guaranteed Passing! CHEM101_MH_V6 | Topic 9: Energy Changes in Chemical Reactions Started on State Finished Completed on Time taken 1 hour 18 mins GradeQuestion 4 Correct 4.00 points out of 4.00 Acetic acid boils at 244.2°F. What is its boiling point in degrees Celsius? Select one: A. 382.0°C B. 103.7°C C. 117.9°C D. 167.7°C E. 153.4°C Question 5 Correct 4.00 points out of 4.00 One of the common intravenous fluids, called physiological saline, is a homogeneous mixture of NaCl in water. In this mixture, 0.89% of the mass is contributed by the NaCl. What mass of NaCl is found in 450. mL of physiological saline? (Density of physiological saline = 1.005 g/cm3) Select one: A. 2.0 g B. 5.1 g C. 4.0 g D. 508 g E. 400 g Question 3 Correct 4.00 points out of 4.00 Which of the following cannot be separated into simpler substances by chemical means? Select one: A. Homogeneous mixture B. Compound C. Element D. Emulsion E. Heterogeneous mixtureQuestion 7 Correct 4.00 points out of 4.00 Which of these materials are typically poor conductors of heat and electricity? Select one: A. Alkaline earth metals B. Metalloids C. Alkali metals D. Nonmetals E. Metals Question 8 Correct 4.00 points out of 4.00 The elements in Group 2 are known by what name? Select one: A. Noble gases B. Halogens C. Alkaline earth metals D. Alkali metals E. Transition metals Question 6 Correct 4.00 points out of 4.00 Which of the following is the empirical formula for hexane, C6H14? Select one: A. C0.43H B. C12H28 C. C6H14 D. C3H7 E. CH2.3Question 10 Correct 4.00 points out of 4.00 What is the formula of iodous acid? Select one: A. HIO3 B. HIO4 C. HIO2 D. HI E. HIO Question 11 Correct 4.00 points out of 4.00 Determine the number of ammonia molecules in 4.85 g of ammonia. (NA = 6.022 × 1023 mol– 1) Select one: A. 5.83 × 10–24 molecules B. 4.73 × 10–25 molecules C. 1.71 × 1023 molecules D. 1.24 × 1023 molecules E. 2.92 × 1023 molecules Question 9 Correct 4.00 points out of 4.00 Which of these pairs of elements would be most likely to form an ionic compound? Select one: A. Al and Rb B. C and O C. P and Br D. Cu and K E. O and ZnQuestion 13 Correct 4.00 points out of 4.00 Calculate the formula mass of rubidium carbonate, Rb2CO3. Select one: A. 230.95 amu B. 145.47 amu C. 255.00 amu D. 113.48 amu E. 340.43 amu Question 14 Correct 4.00 points out of 4.00 Tetraphosphorus hexoxide is formed by the reaction of phosphorus with oxygen gas. If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction? Select one: A. 89.4% B. 57.5% C. 38.0% D. 16.3% E. 48.8% Question 12 Correct 4.00 points out of 4.00 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. 12 B. 9 C. 5 D. 3 E. 6Question 16 Correct 4.00 points out of 4.00 Lead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide? Select one: A. 151 g B. 9.41 g C. 123 g D. 50.3 g E. 37.7 g Question 15 Correct 4.00 points out of 4.00 What mass of nitrogen gas is required to react completely with excess hydrogen gas to produce 13.6 g of ammonia? Select one: A. 11.2 g B. 44.8 g C. 0.06 g D. 22.4 g E. 16.5 gQuestion 17 Correct 4.00 points out of 4.00 Using Hess's law, what is ΔH°rxn for the following reaction? WO3(s) + 3H2(g) → W(s) + 3H2O(g) 2W(s) + 3O2(g) → 2WO3(s) 2H2(g) + O2(g) → 2H2O(g) ΔH° rxn = –1685.8 kJ/mol ΔH° rxn = –483.6 kJ/mol Select one: A. 117.5 kJ/mol B. 235.0 kJ/mol C. 1202.2 kJ/mol D. 359.3 kJ/mol E. 2169.4 kJ/molSuppose a 0.500-g sample of an organic compound is analyzed via bomb calorimetry. The temperature of the calorimeter is measured over time. At t = 5 min, the combustion reaction is initiated. Below is a plot of the data that are obtained. Suppose the experiment is repeated under identical conditions, but with a 1.000-g sample of the organic compound. What might a plot of the resulting data look like? Select one: A. Question 18 Incorrect 0.00 points out of 4.00B. C.D. E.Question 20 Correct 4.00 points out of 4.00 The dissolution of barium hydroxide in water is an exothermic process. Which statement is correct? Select one: A. When barium hydroxide dissolves in water, the system does work on the surroundings. B. The temperature of the solution is lower than of the barium hydroxide and water before mixing. C. The enthalpy of solid barium hydroxide plus pure water is less than that of the solution, at the same temperature. D. The enthalpy of solid barium hydroxide plus pure water is the same as that of the solution, at the same temperature. E. The enthalpy of solid barium hydroxide plus pure water is greater than that of the solution, at the same temperature. Question 19 Correct 4.00 points out of 4.00 Suppose a 50-g block of silver (specific heat = 0.2350 J/g·°C) at 100°C is placed in contact with a 50-g block of iron (specific heat = 0.4494 J/g·°C) at 0°C, and the two blocks are insulated from the rest of the universe. The final temperature of the two blocks Select one: A. will be lower than 50°C. B. will be higher than 50°C. C. will be exactly 50°C. D. is unrelated to the composition of the blocks. E. cannot be predicted.Question 22 Correct 4.00 points out of 4.00 The specific heat (capacity) is Select one: A. the amount of energy needed to increase the temperature of 1 mol of a substance by 1°C. B. the amount of energy needed to increase the temperature of 1 g of a substance by 1°C. C. the temperature increase, in K, associated with heating 1 g of a substance for 1 minute. D. the amount of energy required to melt 1 g of substance. E. the amount of substance that is heated by 1°C. Question 21 Correct 4.00 points out of 4.00 What is ΔH° rxn for the decomposition of calcium carbonate to calcium oxide and carbon dioxide? CaCO3(s) → CaO(s) + CO2(g) Substance CaCO3(s) CaO(s) CO2(g) (kJ/mol) –1206.9 –635.6 –393.5 Select one: A. –2236.0 kJ/mol B. 177.8 kJ/mol C. –1449.0 kJ/mol D. 2236.0 kJ/mol E. –177.8 kJ/molQuestion 24 Correct 4.00 points out of 4.00 De Broglie explained electron movements by relating them to Select one: A. waves only. B. waves and particles. C. particles only. D. None of these choices is correct. Question 25 Correct 4.00 points out of 4.00 What is the maximum number of electrons in an atom that can have the following set of quantum numbers? n = 4, l = 3, ml = –2, ms = +1/2 Select one: A. 6 B. 10 C. 2 D. 1 E. 0 Question 23 Correct 4.00 points out of 4.00 A neutral atom in its ground state contains 28 electrons. This element is considered a element, and has electrons in orbitals with l = 2. Select one: A. actinide, 10 B. transition, 8 C. main group, 10 D. main group, 8 E. transition, 10Which one of the following sets of quantum numbers is not possible? Select one: A. A B. B C. C D. D E. E Question 26 Incorrect Question 27 Correct 4.00 points out of 4.00 Calculate the de Broglie wavelength of a neutron that has a velocity of 200. cm/s. (mass of a neutron = 1.675 × 10–27 kg and h = 6.63 × 10–34 J • s) Select one: A. 216 nm B. 1.98 × 10–9 m C. 198 nm D. 1.8 × 1050 m E. 5.05 mm 0.00 points out n l ml ms of 4.00 A 4 3 –2 +1/2 B 3 2 –3 –1/2 C 3 0 0 +1/2 D 4 1 1 –1/2 E 2 0 0 +1/2Question 29 Correct 4.00 points out of 4.00 Which of these elements has the greatest metallic character? Select one: A. Se B. Si C. As D. Br E. Ni Question 30 Correct 4.00 points out of 4.00 An element with the electron configuration [noble gas]ns2(n – 1)d8 has valence electrons. Select one: A. 6 B. 8 C. 2 D. 10 E. None of these choices is correct. Question 28 Correct 4.00 points out of 4.00 Which element would be expected to have properties similar to calcium? Select one: A. Na B. Ba C. Sc D. Rb E. KQuestion 32 Correct 4.00 points out of 4.00 Select the element with the least metallic character. Select one: A. Sr B. Sn C. Tl D. Ga E. Ge Question 31 Incorrect 0.00 points out of 4.00 Which of the following elements has the smallest atomic size? Select one: A. Na B. Ca C. Kr D. Ar E. KHydrazine, N2H4, is a good reducing agent that has been used as a component in rocket fuels. Select its Lewis structure. Select one: A. B. C. D. E. None of the choices is correct. Question 33 Incorrect 0.00 points out of 4.00Question 35 Correct 4.00 points out of 4.00 Select the compound with the lowest (i.e., least negative) lattice energy. Select one: A. KBr(s) B. CsBr(s) C. CaO(s) D. NaCl(s) E. SrO(s) Question 34 Correct 4.00 points out of 4.00 In the following Lewis structure for ClO3F, chlorine has a formal charge of and an oxidation number of . Select one: A. 7, –1 B. 1, –1 C. 7, 7 D. 1, 7 E. 1, 1Question 37 Incorrect 0.00 points out of 4.00 If an element is bonded to 4 other atoms and has a formal charge of +1, what group must the element be in? Select one: A. 17 B. 13 C. 14 D. 15 E. 16 Question 38 Incorrect 0.00 points out of 4.00 According to the VSEPR model, a molecule with the general formula AB4 with two lone pairs on the central atom will have a(n) molecular geometry. Select one: A. seesaw B. square planar C. square pyramidal D. tetrahedral E. octahedral Question 36 Incorrect 0.00 points out of 4.00 The Lewis structure for a chlorate ion, ClO3–, should show single bond(s), double bond(s), and lone pair(s). Select one: A. 3, 0, 10 B. 1, 2, 8 C. 3, 0, 9 D. 1, 2, 7 E. 2, 1, 9Question 40 Incorrect 0.00 points out of 4.00 According to the VSEPR model, the predicted molecular geometry of SiCl4 is Select one: A. bent. B. linear. C. tetrahedral. D. trigonal planar. E. trigonal pyramidal. Question 41 Correct 4.00 points out of 4.00 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 3 and is diamagnetic. B. NO+ has a bond order of 2 and is diamagnetic. C. NO+ has a bond order of 2 and is paramagnetic. D. NO+ has a bond order of 2.5 and is neither paramagnetic nor diamagnetic. E. NO+ has a bond order of 3 and is paramagnetic. Question 39 Correct 4.00 points out of 4.00 According to the VSEPR model, which molecule is predicted to have a molecular geometry that is trigonal bipyramidal? Select one: A. SF4 B. XeF4 C. SF6 D. NF3 E. PF5Question 43 Correct 4.00 points out of 4.00 What is the predicted molecular geometry of the H2O molecule according to the VSEPR model? Select one: A. bent B. tetrahedral C. seesaw D. square planar E. trigonal pyramidal Question 44 Correct 4.00 points out of 4.00 Find the pH of a 0.135 M aqueous solution of periodic acid (HIO4), for which Ka = 2.3 × 10–2. Select one: A. 1.25 B. 3.28 C. 1.17 D. 1.64 E. 1.34 Question 42 Correct 4.00 points out of 4.00 In which molecule is the central atom sp2 hybridized? Select one: A. N2O B. NF3 C. SO2 D. PF5 E. BeCl2Question 46 Correct 4.00 points out of 4.00 The reaction of a strong acid with water results in Select one: A. a weak conjugate base. B. a weak conjugate acid. C. a strong conjugate base. D. a strong base. E. pure water. Question 47 Correct 4.00 points out of 4.00 Which is the correct statement? Select one: A. All protons are lost from a polyprotic acid at the same time. B. H2O is a diprotic acid. C. NH3 is a polyprotic acid. D. NH3 is a diprotic acid. E. A polyprotic acid has more than two ionizable protons. Question 45 Correct 4.00 points out of 4.00 For H3PO4, Ka1 = 7.3 × 10–3, Ka2 = 6.2 × 10–6, and Ka3 = 4.8 × 10–13. A 0.10 M aqueous solution of Na3PO4 therefore would be . Select one: A. weakly basic B. neutral C. strongly basic D. weakly acidic E. strongly acidicQuestion 49 Correct 4.00 points out of 4.00 A 0.15 M solution of chloroacetic acid has a pH of 1.86. What is the value of Ka for this acid? Select one: A. 7.2 × 101 B. 9.9 × 10–2 C. 1.6 × 10–1 D. 2.7 × 10–4 E. 1.4 × 10–3 Question 50 Correct 4.00 points out of 4.00 The substance NH3 is considered to be Select one: A. a strong base. B. a neutral compound. C. a weak acid. D. a strong acid. E. a weak base. Question 48 Correct 4.00 points out of 4.00 Which is an amphoteric oxide? Select one: A. Al2O3 B. MgO C. SO2 D. Na2O E. Cl2O7Quiz navigation Show one page at a time Finish review 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50 © 2023 StraighterLine. All rights reserved [Show Less]
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