Question 1

Which one of the following reagents is capable of oxidizing Cu(s) to Cu2+ (1 M)

Accepted Answer

A)  I- (1 M) 
B)  Ni(s) 
C)  Ag+ (1 M) 
D)  Al3+ (1 M) 
E)  H+ (1 M) 
A)  I- (1 M) 
B)  Ni(s) 
C)  Ag+ (1 M) 
D)  Al3+ (1 M) 
E)  H+ (1 M)

Question 2

The measured voltage of a cell in which the following reaction occurs is 0.96 V: 
H2(g, 1.0 atm) + 2Ag+(aq, 1.0 M) $\rarr$ 2H+(aq, pH
) + 2Ag(s)
Calculate the pH of the H+(aq) solution.

Accepted Answer

A)  1.4 
B)  2.7 
C)  5.4 
D)  7.1 
E)  14.9 
A)  1.4 
B)  2.7 
C)  5.4 
D)  7.1 
E)  14.9

Question 3

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II) iodide solution is

Accepted Answer

A) I2 + 2e- $\rarr$ 2I-. 
B) Cu $\rarr$ Cu2+ + 2e-. 
C) Cu2+ + 2e- $\rarr$ Cu. 
D) 2I- $\rarr$ I2 + 2e-. 
E) 2e- + 2H2O $\rarr$ H2 + 2OH-. 
A) I2 + 2e- $\rarr$ 2I-. 
B) Cu $\rarr$ Cu2+ + 2e-. 
C) Cu2+ + 2e- $\rarr$ Cu. 
D) 2I- $\rarr$ I2 + 2e-. 
E) 2e- + 2H2O $\rarr$ H2 + 2OH-.

Question 4

The measured voltage of the cell Pt(s) | H2 (1.0 atm) | H+(aq) || Ag+(1.0 M) | Ag(s) is 1.02 V at 25$\circ$C. Calculate the pH of the solution.

Accepted Answer

A)  1.86 
B)  1.69 
C)  3.72 
D)  3.89 
E)  7.43 
A)  1.86 
B)  1.69 
C)  3.72 
D)  3.89 
E)  7.43

Question 5

Calculate E$\circ$cell for the following electrochemical cell: Mn(s) | Mn2+(aq) || Ce4+(aq),Ce3+(aq) | Pt(s)

Accepted Answer

A)  2.39 V 
B)  2.59 V 
C)  2.79 V 
D)  2.99 V 
E)  None of the above 
A)  2.39 V 
B)  2.59 V 
C)  2.79 V 
D)  2.99 V 
E)  None of the above

Question 6

How many coulombs of charge are required to cause reduction of 0.20 mole of Cr3+ to Cr

Accepted Answer

A)  0.60 C 
B)  3.0 C 
C)  2.9 * 104 C 
D)  5.8 * 104 C 
E)  9.65 * 104 C 
A)  0.60 C 
B)  3.0 C 
C)  2.9 * 104 C 
D)  5.8 * 104 C 
E)  9.65 * 104 C

Question 7

You wish to electroplate a metal utensil with a surface area of 736 cm2 with gold to give an average thickness of 0.025 mm over the entire surface. Starting with a solution of excess Au3+ and applying a constant current of 14 A, how long will it take to electroplate the utensil The density of gold is 19.3 g/cm3.

Accepted Answer

A)  42 minutes 
B)  62 minutes 
C)  82 minutes 
D)  1022 minutes 
E)  None of the above 
A)  42 minutes 
B)  62 minutes 
C)  82 minutes 
D)  1022 minutes 
E)  None of the above

Question 8

Under acidic conditions, the correctly balanced redox reaction for Cu(s) + NO3-(aq) $\rarr$ Cu2+(aq) + NO2(g) is:
Cu(s) + 2NO3-(aq) + 2H+(aq) $\rarr$ Cu2+(aq) + 2NO2(g) + H2O(l)

Accepted Answer

A) True 
 B)False

Question 9

How many coulombs of charge are required to cause reduction of 0.25 mole of Cu2+ to Cu

Accepted Answer

A)  0.25 C 
B)  0.50 C 
C)  1.2 * 104 C 
D)  2.4 * 104 C 
E)  4.8 * 104 C 
A)  0.25 C 
B)  0.50 C 
C)  1.2 * 104 C 
D)  2.4 * 104 C 
E)  4.8 * 104 C

Question 10

Write the formula of the strongest reducing agent given the following standard reduction potentials in acid solution: $\begin{array}{ll}
\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{-} \rightarrow 2 \mathrm{H}_{2} \mathrm{O} & \mathrm{E}^{\circ}=+1.23 \mathrm{~V} \
\mathrm{Sn}^{4+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Sn}^{2+} & \mathrm{E}^{\circ}=+0.13 \mathrm{~V} \
\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(\mathrm{~s}) & \mathrm{E}^{\circ}=-0.76 \mathrm{~V}
\end{array}$

Accepted Answer

A)  4H+ 
B)  2H2O 
C)  Sn4+ 
D)  Zn 
E)  None of the above 
A)  4H+ 
B)  2H2O 
C)  Sn4+ 
D)  Zn 
E)  None of the above

Question 11

Complete and balance the following redox equation using the set of smallest whole-number coefficients. What is the sum of the coefficients
HI + HNO3 $\rarr$I2 + NO (acidic solution)

Accepted Answer

A)  5 
B)  7 
C)  14 
D)  17 
E)  None of these. 
A)  5 
B)  7 
C)  14 
D)  17 
E)  None of these.

Question 12

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge.
- a Fe electrode in 1.0 M FeCl2 solution 
- a Ni electrode in 1.0 M Ni(NO3)2 solution
When the cell is running spontaneously, which choice includes only true statements and no false ones

Accepted Answer

A)  The nickel electrode loses mass and the nickel electrode is the cathode. 
B)  The nickel electrode gains mass and the nickel electrode is the cathode. 
C)  The iron electrode gains mass and the iron electrode is the anode. 
D)  The iron electrode loses mass and the iron electrode is the cathode. 
A)  The nickel electrode loses mass and the nickel electrode is the cathode. 
B)  The nickel electrode gains mass and the nickel electrode is the cathode. 
C)  The iron electrode gains mass and the iron electrode is the anode. 
D)  The iron electrode loses mass and the iron electrode is the cathode.

Question 13

Which one of the following reagents is capable of reducing Fe3+ (1 M) to Fe2+ (1 M)

Accepted Answer

A)  H2(1 atm) 
B)  NO3- (1 M) 
C)  O2(1 atm) 
D)  Br- (1 M) 
E)  H+ (1 M) 
A)  H2(1 atm) 
B)  NO3- (1 M) 
C)  O2(1 atm) 
D)  Br- (1 M) 
E)  H+ (1 M)

Question 14

Which of the following would be considered a Lead Storage Battery

Accepted Answer

A) C3H8(g) + 5O2(g) $\rarr$3CO2(g) + 4H2O(l) 
B) Pb(s) + PbO2(s) + 4H+(aq) + 2SO42-(aq) $\rarr$ 2PbSO4(s) + 2H2O(l) 
C) Zn(s) + 2NH4+(aq) + 2MnO2(s) $\rarr$ Zn2+(aq) + 2NH3(aq) + H2O(l) + Mn2O3(s) 
D) Zn(Hg) + HgO(s) $\rarr$ ZnO(s) + Hg(l) 
E) 2Fe(s) + O2(g) + 4H+(aq) $\rarr$2Fe2+(aq) + 2H2O(l) 
A) C3H8(g) + 5O2(g) $\rarr$3CO2(g) + 4H2O(l) 
B) Pb(s) + PbO2(s) + 4H+(aq) + 2SO42-(aq) $\rarr$ 2PbSO4(s) + 2H2O(l) 
C) Zn(s) + 2NH4+(aq) + 2MnO2(s) $\rarr$ Zn2+(aq) + 2NH3(aq) + H2O(l) + Mn2O3(s) 
D) Zn(Hg) + HgO(s) $\rarr$ ZnO(s) + Hg(l) 
E) 2Fe(s) + O2(g) + 4H+(aq) $\rarr$2Fe2+(aq) + 2H2O(l)

Question 15

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced with the set of smallest whole-number coefficients
H2O + MnO4- + I- $\rarr$MnO2 + IO3- (basic solution)

Accepted Answer

A)  1 
B)  2 
C)  4 
D)  10 
E)  None of these. 
A)  1 
B)  2 
C)  4 
D)  10 
E)  None of these.

Question 16

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation
PbO2(s) + Cl- $\rarr$ Pb2+ + Cl2(g) (acidic solution)

Accepted Answer

A)  2 
B)  4 
C)  5 
D)  9 
E)  11 
A)  2 
B)  4 
C)  5 
D)  9 
E)  11

Question 17

How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant current of 4.80 amperes through a solution containing CrCl3

Accepted Answer

A)  483 min 
B)  161 min 
C)  322 min 
D)  2.01 * 104 min 
E)  1.11 * 104 min 
A)  483 min 
B)  161 min 
C)  322 min 
D)  2.01 * 104 min 
E)  1.11 * 104 min

Question 18

Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell

Accepted Answer

A) 3Ni2+(aq) + 2Cr(s) $\rarr$ 3Ni(s) + 2Cr3+(aq) 
B) 2Ag+(aq) + Pb(s) $\rarr$ 2Ag(s) + Pb2+(aq) 
C) Br2(l) + 2Cu+(aq) $\rarr$ 2Br-(aq) + Cu2+(aq) 
D) Cr3+(aq) + 3Ag(s) $\rarr$ Cr + 3Ag+(aq) 
E) 2Fe3+(aq) + Sn(s) $\rarr$ 2Fe2+(aq) + Sn2+(aq) 
A) 3Ni2+(aq) + 2Cr(s) $\rarr$ 3Ni(s) + 2Cr3+(aq) 
B) 2Ag+(aq) + Pb(s) $\rarr$ 2Ag(s) + Pb2+(aq) 
C) Br2(l) + 2Cu+(aq) $\rarr$ 2Br-(aq) + Cu2+(aq) 
D) Cr3+(aq) + 3Ag(s) $\rarr$ Cr + 3Ag+(aq) 
E) 2Fe3+(aq) + Sn(s) $\rarr$ 2Fe2+(aq) + Sn2+(aq)

Question 19

The half-reaction that should occur at the anode during electrolysis of an aqueous potassium bromide solution is

Accepted Answer

A) Br2 + 2e- $\rarr$ 2Br-. 
B) Na $\rarr$ Na+ + e-. 
C) Na+ + e- $\rarr$ Na. 
D) 2Br- $\rarr$ Br2 + 2e-. 
E) 2H2O $\rarr$ O2 + 4H+ + 4e-. 
A) Br2 + 2e- $\rarr$ 2Br-. 
B) Na $\rarr$ Na+ + e-. 
C) Na+ + e- $\rarr$ Na. 
D) 2Br- $\rarr$ Br2 + 2e-. 
E) 2H2O $\rarr$ O2 + 4H+ + 4e-.

Question 20

Determine the equilibrium constant for the following reaction at 298 K.2Fe3+(aq) + H2O2(aq) $\leftrightharpoons$ 2H+(aq) + O2(g) + 2Fe2+(aq).

Accepted Answer

A)  1. * 102 
B)  1. * 103 
C)  1. *104 
D)  1. * 105 
E)  None of the above 
A)  1. * 102 
B)  1. * 103 
C)  1. *104 
D)  1. * 105 
E)  None of the above

Exam 18: Electrochemistry

Which one of the following reagents is capable of oxidizing Cu(s) to Cu2+ (1 M)

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H2(g, 1.0 atm) + 2Ag+(aq, 1.0 M) →\rarr→ 2H+(aq, pH ) + 2Ag(s) Calculate the pH of the H+(aq) solution.

The half-reaction occurring at the cathode during electrolysis of an aqueous copper(II) iodide solution is

The measured voltage of the cell Pt(s) | H2 (1.0 atm) | H+(aq) || Ag+(1.0 M) | Ag(s) is 1.02 V at 25 ∘\circ∘ C. Calculate the pH of the solution.

Calculate E ∘\circ∘ cell for the following electrochemical cell: Mn(s) | Mn2+(aq) || Ce4+(aq),Ce3+(aq) | Pt(s)

How many coulombs of charge are required to cause reduction of 0.20 mole of Cr3+ to Cr

Under acidic conditions, the correctly balanced redox reaction for Cu(s) + NO3-(aq) →\rarr→ Cu2+(aq) + NO2(g) is: Cu(s) + 2NO3-(aq) + 2H+(aq) →\rarr→ Cu2+(aq) + 2NO2(g) + H2O(l)

How many coulombs of charge are required to cause reduction of 0.25 mole of Cu2+ to Cu

Write the formula of the strongest reducing agent given the following standard reduction potentials in acid solution: +4+4\rightarrow2 =+1.23 +2\rightarrow =+0.13 +2\rightarrow() =-0.76

Complete and balance the following redox equation using the set of smallest whole-number coefficients. What is the sum of the coefficients HI + HNO3 →\rarr→ I2 + NO (acidic solution)

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl2 solution - a Ni electrode in 1.0 M Ni(NO3)2 solution When the cell is running spontaneously, which choice includes only true statements and no false ones

Which one of the following reagents is capable of reducing Fe3+ (1 M) to Fe2+ (1 M)

Which of the following would be considered a Lead Storage Battery

Complete and balance the following redox equation. What is the coefficient of H2O when the equation is balanced with the set of smallest whole-number coefficients H2O + MnO4- + I- →\rarr→ MnO2 + IO3- (basic solution)

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation PbO2(s) + Cl- →\rarr→ Pb2+ + Cl2(g) (acidic solution)

How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant current of 4.80 amperes through a solution containing CrCl3

Which one of the following reactions must be carried out in an electrolytic cell rather than in a galvanic cell

The half-reaction that should occur at the anode during electrolysis of an aqueous potassium bromide solution is

Determine the equilibrium constant for the following reaction at 298 K.2Fe3+(aq) + H2O2(aq) ⇋\leftrightharpoons⇋ 2H+(aq) + O2(g) + 2Fe2+(aq).

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Which one of the following reagents is capable of oxidizing Cu(s) to Cu²⁺ (1 M)

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H₂(g, 1.0 atm) + 2Ag⁺(aq, 1.0 M) $\rarr$ 2H⁺(aq, pH ) + 2Ag(s) Calculate the pH of the H⁺(aq) solution.

The measured voltage of the cell Pt(s) | H₂ (1.0 atm) | H⁺(aq) || Ag⁺(1.0 M) | Ag(s) is 1.02 V at 25^$\circ$C. Calculate the pH of the solution.

Calculate E^$\circ$_cell for the following electrochemical cell: Mn(s) | Mn²⁺(aq) || Ce⁴⁺(aq),Ce³⁺(aq) | Pt(s)

How many coulombs of charge are required to cause reduction of 0.20 mole of Cr³⁺ to Cr

Under acidic conditions, the correctly balanced redox reaction for Cu(s) + NO₃^-(aq) $\rarr$ Cu²⁺(aq) + NO₂(g) is: Cu(s) + 2NO₃^-(aq) + 2H⁺(aq) $\rarr$ Cu²⁺(aq) + 2NO₂(g) + H₂O(l)

How many coulombs of charge are required to cause reduction of 0.25 mole of Cu²⁺ to Cu

Complete and balance the following redox equation using the set of smallest whole-number coefficients. What is the sum of the coefficients HI + HNO₃ $\rarr$ I₂ + NO (acidic solution)

Consider an electrochemical cell constructed from the following half cells, linked by a KCl salt bridge. - a Fe electrode in 1.0 M FeCl₂ solution - a Ni electrode in 1.0 M Ni(NO₃)₂ solution When the cell is running spontaneously, which choice includes only true statements and no false ones

Which one of the following reagents is capable of reducing Fe³⁺ (1 M) to Fe²⁺ (1 M)

Complete and balance the following redox equation. What is the coefficient of H₂O when the equation is balanced with the set of smallest whole-number coefficients H₂O + MnO₄^- + I^- $\rarr$ MnO₂ + IO₃^- (basic solution)

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation PbO₂(s) + Cl^- $\rarr$ Pb²⁺ + Cl₂(g) (acidic solution)

How many minutes would be required to electroplate 25.0 grams of chromium by passing a constant current of 4.80 amperes through a solution containing CrCl₃

Determine the equilibrium constant for the following reaction at 298 K.2Fe³⁺(aq) + H₂O₂(aq) $\leftrightharpoons$ 2H⁺(aq) + O₂(g) + 2Fe²⁺(aq).