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What intermolecular bonds or forces are present in P4(s) ?


A) Hydrogen bonds
B) Covalent bonds
C) Ionic bonds
D) Dipole forces
E) Dispersion forces

F) A) and E)
G) C) and E)

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The first step in the synthesis of nitric acid involves the reaction of ammonia with oxygen to produce nitrogen monoxide. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g) What volume of NO is produced if 14.0 L NH3 is reacted with 15.0 L O2? Assume the reaction is 100% efficient.


A) 12.0 L
B) 14.0 L
C) 15.0 L
D) 23.2 L
E) 29.0 L

F) A) and B)
G) A) and E)

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Which of the following oxoacids has the largest Ka value?


A) HClO4
B) HClO3
C) HClO2
D) HClO
E) All of the above oxoacids have similar Ka values.

F) A) and B)
G) D) and E)

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Hydrazine is made commercially by reacting aqueous ammonia with hypochlorite ion.Write a balanced equation for this reaction.


A) 2NH3(aq) + ClO4−(aq) → N2H4(aq) + ClO3−(aq) + H2O(l)
B) 2NH3(aq) + ClO3−(aq) → N2H4(aq) + ClO2−(aq) + H2O(l)
C) 2NH3(aq) + ClO2−(aq) → N2H4(aq) + Cl−(aq) + H2O2(aq)
D) 2NH3(aq) + ClO−(aq) → N2H4(aq) + Cl−(aq) + H2O(l)
E) 2NH3(aq) + ClO−(aq) → N2H4(aq) + H2(aq) + ClO−(aq)

F) A) and B)
G) B) and D)

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Which of the following molecules has the ability to dilate blood vessels,thereby lowering blood pressure?


A) NO
B) N2O
C) CO
D) HCl
E) SO3

F) D) and E)
G) B) and D)

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Fluorine and chlorine gases are primarily produced by


A) distillation.
B) oxidation by electrolysis.
C) oxidation by hydronium ion.
D) reduction by carbon monoxide.
E) roasting with copper(II) sulfide.

F) B) and D)
G) A) and B)

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As one might predict,one allotrope of arsenic has the formula


A) As4
B) As8
C) As2
D) As3
E) As10

F) A) and D)
G) C) and E)

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Which of the following statements is INCORRECT?


A) Sodium dihydrogen phosphate,NaH2PO4,is used in acidic cleaners.
B) Sodium phosphate,Na3PO4,is used in strongly basic cleaners.
C) Calcium dihydrogen phosphate,Ca(H2PO4) 2 is used in fertilizers.
D) The principal use of Na2HPO4 is as an emulsifier in the manufacture of cheese.
E) Phosphoric acid is a strong acid,a powerful oxidizing agent,and a drying agent.

F) B) and E)
G) All of the above

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Write a half-reaction for the reduction of aqueous hydrogen peroxide in an acidic solution.


A) H2O2(aq) + 2e− → H2(g) + O22−(aq)
B) 2H2O2(aq) + 2e− → O2(g) + 2H2O(l)
C) H2O2(aq) + 2e− → 2OH−(aq)
D) H2O2(aq) + 2H+(aq) + 2e− → 2H2O(l)
E) Hydrogen peroxide cannot be reduced under acidic conditions.

F) C) and D)
G) B) and D)

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Write a balanced net ionic equation for the reaction of chlorine gas with aqueous potassium iodide.


A) Cl2(g) + 2KI(aq) → 2KCl(s) + I2(aq)
B) Cl2(g) + 2I−(aq) → 2ICl(aq)
C) Cl2(g) + 2I−(aq) → 2Cl−(aq) + I2(aq)
D) Cl2(g) + 2I−(aq) → Cl2I(aq) + I−(aq)
E) Cl2(g) + K+(aq) + I−(aq) → KCl(s) + ICl(g)

F) A) and B)
G) C) and D)

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Which of the following oxoanions of chlorine cannot act as an oxidizing agent?


A) HClO
B) HClO2
C) HClO3
D) HClO4
E) All of the above can act as oxidizing agents.

F) B) and D)
G) B) and E)

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Nitric acid solutions slowly turn brown when exposed to sunlight.Which of the following reactions is responsible?


A) NO3−(aq) → NO(g) + O2(g)
B) 2NO3−(aq) → 2NO2(g) + O2(g)
C) 2H+(aq) + NO3−(aq) → NO2(g) + H2O(l)
D) 4H+(aq) + 4NO3−(aq) → 4NO2(g) + 2H2O(l) + O2(g)
E) 4H+(aq) + NO3−(aq) → NO(g) + 2H2(g) + O2(g)

F) A) and D)
G) None of the above

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Hydrogen sulfide is used to remove sulfur dioxide in power plant smokestacks.The reaction produces elemental sulfur and water.Write a balanced chemical equation for this reaction.


A) H2S(l) + SO2(g) → 2HSO(s)
B) H2S(l) + SO2(g) → 2S(s) + 2OH−(aq)
C) 2H2S(l) + SO2(g) → 3S(s) + 2H2O(l)
D) H2S(l) + SO2(g) → 2S(s) + H2O2(aq)
E) H2S(l) + SO2(g) + 2H+(aq) → 2S(s) + 2H2O(l)

F) A) and B)
G) B) and E)

Correct Answer

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Write a balanced equation for the reaction of concentrated sulfuric acid with copper metal.Assume two products are sulfur dioxide and Cu2+.


A) Cu(s) + SO42−(aq) → Cu2+(aq) + O2(g) + SO2(g)
B) Cu(s) + 4H+(aq) + SO42−(aq) → CuS(s) + 2O2(g)
C) Cu(s) + 2H+(aq) + SO42−(aq) → Cu2+(aq) + H2O(l) + SO2(g)
D) Cu(s) + 4H+(aq) + SO42−(aq) → Cu2+(aq) + 2H2O(l) + SO2(g)
E) Cu(s) + 8H+(aq) + SO42−(aq) → Cu2+(aq) + 4H2O(l) + S(g)

F) C) and D)
G) A) and D)

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The standard reduction potential of H2O2 = +1.763 V.Which of the following species will be oxidized by hydrogen peroxide? Co2+(aq) →Co3+(aq) +2eΛg(s) →Ag′(aq) +e−Co(s) →Co2+(aq) +2eZn(s) →Zn2+(aq) +2e−Na(s) →Na+(aq) +e−Ered∘+1.953 V+0.799 V−0.282 V−0.762 V−2.714 V\begin{array}{l}\begin{array}{l}\\\mathrm{Co}^{2+}(a q) \rightarrow \mathrm{Co}^{3+}(a q) +2 e \\\Lambda \mathrm{g}(s) \rightarrow \mathrm{Ag}^{\prime}(a q) +e^{-} \\\mathrm{Co}(s) \rightarrow \mathrm{Co}^{2+}(a q) +2 e \\\mathrm{Zn}(s) \rightarrow \mathrm{Zn}^{2+}(a q) +2 e^{-} \\\mathrm{Na}(s) \rightarrow \mathrm{Na}^{+}(a q) +e-\end{array}\begin{array}{l} E_{\mathrm{red}}^{\circ} \\+1.953 \mathrm{~V} \\+0.799 \mathrm{~V} \\-0.282 \mathrm{~V} \\-0.762 \mathrm{~V} \\-2.714 \mathrm{~V}\end{array}\end{array}


A) Co2+
B) Co2+ and Ag(s)
C) Co(s) and Co2+
D) Zn(s) and Na(s)
E) Ag(s) ,Co(s) ,Zn(s) ,and Na(s)

F) A) and C)
G) C) and E)

Correct Answer

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Write a balanced chemical equation for the reaction of N2O5 and water.


A) N2O5(s) + H2O(l) → N2O4(s) + H2O2(l)
B) N2O5(s) + H2O(l) → N2O(g) + H2O(l) + 2O2(g)
C) N2O5(s) + 3H2O(l) → NH3(g) + 4O2(g)
D) N2O5(s) + H2O(l) → 2HNO3(l)
E) N2O5(s) + H2O(l) → 2HNO2(l) + O2(g)

F) A) and B)
G) A) and E)

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Place the following acids in order from smallest to largest Ka value: HClO,HBrO,and HIO.


A) HClO < HBrO < HIO
B) HClO < HIO < HBrO
C) HBrO < HClO < HIO
D) HBrO < HIO < HClO
E) HIO < HBrO < HClO

F) B) and C)
G) None of the above

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Which reddish-brown gas is a major factor in the formation of photochemical smog?


A) NO
B) NO2
C) SO2
D) CO2
E) CO

F) A) and D)
G) A) and C)

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All of the following statements concerning oxoanions and oxoacids are true EXCEPT


A) MnO4− can never act as an oxidizing agent.
B) Cr2O72− can never act as a reducing agent.
C) ClO4− is a stronger oxidizing agent than ClO−.
D) ClO2− can behave as either an oxidizing or a reducing agent.
E) HClO3 is a stronger acid than HClO2.

F) C) and E)
G) B) and D)

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Write a balanced equation for the reaction of Ni2+ with H2S.


A) Ni2+(aq) + 2H2S(aq) → Ni(HS) 2(s) + 2H+(aq)
B) Ni2+(aq) + H2S(aq) → NiH2(s) + S2−(aq)
C) Ni2+(aq) + H2S(aq) → NiS(s) + 2H+(aq)
D) Ni2+(aq) + H2S(aq) → Ni(s) + S(s) + 2H+(aq)
E) No reaction will occur.

F) C) and D)
G) B) and D)

Correct Answer

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