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• CHEM101_MH_V4
• Topic 6: Quantum Theory
Started on Monday, March 28, 2022, 10:23 AM
State Finished
Completed on Monday, March 28,
... [Show More] 2022, 11:01 AM
Time taken 38 mins 28 secs
Grade 101.20 out of 115.00 (88%)
Question 1
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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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
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___________________ 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
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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
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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
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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
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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
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How many electrons are in the 4p orbitals of selenium?
Select one:
a. 0
b. 2
c. 4
d. 5
e. 6
Question 25
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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]