Question 1
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The SI base unit of mass is
Select one:
A. g.
B. metric ton.
C. mg.
D. lb.
E. kg.
Question
... [Show More] 2
Correct
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)
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CHEM101_MH_V6 | Topic 9: Energy Changes in Chemical Reactions
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GradeQuestion 4
Correct
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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
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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
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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
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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
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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
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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
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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
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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
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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
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of 4.00Question 35
Correct
4.00 points out
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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
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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
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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
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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
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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
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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
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In which molecule is the central atom sp2 hybridized?
Select one:
A. N2O
B. NF3
C. SO2
D. PF5
E. BeCl2Question 46
Correct
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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
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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
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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
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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
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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
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Which is an amphoteric oxide?
Select one:
A. Al2O3
B. MgO
C. SO2
D. Na2O
E. Cl2O7Quiz navigation
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