Deck 21: Electrochemistry Chemical Change and Electrical Work

Question 1

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO₄(aq) + OH_-(aq) → Al₂O₃(s) + S_2-(aq) + H₂O(l)

A) 1.
B) 3.
C) 4.
D) 8.
E) None of these choices are correct.

Answer 1

3.

Question 2

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s)
Which of the following processes occurs at the cathode?

A) Cu(s) → Cu²⁺(aq) + 2e^-
B) Cu²⁺(aq) + 2e^- → Cu(s)
C) Ag(s) → Ag⁺(aq) + e^-
D) Ag⁺(aq) + e^- → Ag(s)
E) Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

Answer 2

Ag⁺(aq) + e^- → Ag(s)

Question 3

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be Zn(s) + ReO₄(aq) → Re(s) + Zn₂₊(aq) (acidic solution)

A) 2.
B) 7.
C) 8.
D) 16.
E) None of these choices are correct.

Answer 3

7.

Question 4

Which of the following statements about voltaic and electrolytic cells is correct?

A) The anode will definitely gain weight in a voltaic cell.
B) Oxidation occurs at the cathode of both cells.
C) The free energy change, ΔG, is negative for the voltaic cell.
D) The electrons in the external wire flow from cathode to anode in an electrolytic cell.
E) None of these choices are correct.

Question 5

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al₃₊(aq) || Ni₂₊(aq) | Ni(s)
Which of the following reactions occurs at the anode?

A) Al(s) → Al³⁺(aq) + 3e^-
B) Al³⁺(aq) + 3e → Al(s)
C) Ni(s) → Ni²⁺(aq) + 2e^-
D) Ni²⁺(aq) + 2e^- → Ni(s)
E) None of these choices are correct.

Question 6

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²₊(aq) || I^-(aq) | I₂(s) | C(graphite)
Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

A) 2I^-(aq) + Zn²⁺(aq) → I₂(s) + Zn(s)
B) I₂(s) + Zn(s) → 2I^-(aq) + Zn²⁺(aq)
C) 2I^-(aq) + Zn(s) → I₂(s) + Zn²⁺(aq)
D) I₂(s) + Zn²⁺(aq) → 2I^-(aq) + Zn(s)
E) None of these choices are correct.

Question 7

Which one of the following statements about electrochemical cells is correct?

A) In a salt bridge, current is carried by cations moving toward the anode, and anions toward the cathode.
B) In the external wire, electrons travel from cathode to anode.
C) The anode of a voltaic cell is labeled minus (-).
D) Oxidation occurs at the cathode, in an electrolytic cell.
E) None of these choices are correct.

Question 8

Consider the following balanced redox reaction Mn²+(aq) + S₂O8^2-(aq) + 2H₂O(l) → MnO₂(s) + 4H(aq) + 2SO₄^2-(aq)
Which of the following statements is true?

A) Mn²⁺(aq) is the oxidizing agent and is reduced.
B) Mn²⁺(aq) is the oxidizing agent and is oxidized.
C) Mn²⁺(aq) is the reducing agent and is oxidized.
D) Mn²⁺(aq) is the reducing agent and is reduced.
E) Manganese does not change its oxidation number in this reaction.

Question 9

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH)3-will be Bi(OH)₃(s) + Sn(OH)₃(aq) → Sn(OH)₆^2-(aq) + Bi(s) (basic solution)

A) 1.
B) 2.
C) 3.
D) 6.
E) None of these choices are correct.

Question 10

Consider the reaction CuO(s) + H₂(g) → Cu(s) + H₂O(l)
In this reaction, which substances are the oxidant and reductant, respectively?

A) CuO and H₂
B) H₂ and CuO
C) CuO and Cu
D) H₂O and H₂
E) None of these choices are correct.

Question 11

Which component of the following cell notation is the anode? P | || R | S

A) P
B)
C) R
D) S
E) One of the | symbols is the anode.

Question 12

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be--. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

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

Question 13

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I-(aq) + NO₃-(aq) → NO(g) + I₂(s) (acidic solution)

A) 2.
B) 3.
C) 6.
D) 8.
E) None of these choices are correct.

Question 14

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states)?

A) HCl and Cl-
B) H+ and OH-
C) H₂O and H⁺
D) Fe³⁺ and Fe₂O₃
E) MnO₂ and Mn²⁺

Question 15

Which of the following statements about voltaic and electrolytic cells is correct?

A) The electrons in the external wire flow from cathode to anode in both types of cell.
B) Oxidation occurs at the cathode only in a voltaic cell.
C) The free energy change, ΔG, is negative for an electrolytic cell.
D) The cathode is labeled as positive (+) in a voltaic cell but negative (-) in an electrolytic cell.
E) Reduction occurs at the anode in an electrolytic cell.

Question 16

Consider the following redox equation Mn(OH)₂(s) + MnO₄(aq) → MnO₄^2-(aq) (basic solution)
When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

A) 4, reactant side
B) 4, product side
C) 6, reactant side
D) 6, product side
E) None of these choices are correct.

Question 17

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s)
Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

A) Ni²⁺(aq) + Al(s) → Al³⁺(aq) + Ni(s)
B) 3Ni²⁺(aq) + 2Al(s) → 2Al³⁺(aq) + 3Ni(s)
C) Ni(s) + Al³⁺(aq) → Ni²⁺(aq) + Al(s)
D) 3Ni(s) + 2Al³⁺(aq) → 3Ni²⁺(aq) + 2Al(s)
E) None of these choices are correct.

Question 18

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) → N₂(g) + 3H₂O(l) + 3Cu(s)
Which of the following statements is true?

A) CuO(s) is the oxidizing agent and copper is reduced.
B) CuO(s) is the oxidizing agent and copper is oxidized.
C) CuO(s) is the reducing agent and copper is oxidized.
D) CuO(s) is the reducing agent and copper is reduced.
E) CuO(s) is the oxidizing agent and N₂(g) is the reducing agent.

Question 19

Which one of the following is not a redox reaction?

A) Al(OH)₄(aq) + 4H(aq) → Al³+(aq) + 4H₂O(l)
B) C₆H₁₂O₆(s) + 6O₂(g) → 6CO₂(g) + 6H₂O(l)
C) Na₆FeCl₈(s) + 2Na(l) → 8NaCl(s) + Fe(s)
D) 2H₂O₂(aq) → 2H₂O(l) + O₂(g)
E) CO₂(g) + H₂(g) → CO(g) + H₂O(g)

Question 20

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

A) zinc
B) graphite
C) copper
D) iron
E) sodium

Question 21

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E°_cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S₂O₈^2-(aq) + 2H⁺ + 2I^-(aq) → 2HSO₄^-(aq) + I₂(aq)

A) -1.051 V
B) -2.123 V
C) 1.051 V
D) 2.123 V
E) None of these choices are correct.

Question 22

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^-
Cr(s) E° = -0.913 V
Fe²⁺(aq) + 2e^-
Fe(s) E° = -0.447 V
Sr²⁺(aq) + 2e^-
Sr(s) E° = -2.89 V
Co²⁺(aq) + 2e^-
Co(s) E° = -0.28 V

A) Cr²⁺(aq)
B) Fe(s)
C) Fe²⁺(aq)
D) Sr²⁺(aq)
E) Co²⁺(aq)

Question 23

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

A) 0.96 V
B) 0.52 V
C) -0.52 V
D) -0.96 V
E) Need to know the cell reaction in order to calculate the answer.

Question 24

The voltaic cell made up of cobalt, copper, and their M²⁺ ions, has E°_cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

A) -0.28 V
B) -0.96 V
C) 0.28 V
D) 0.96 V
E) None of these choices are correct.

Question 25

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

A) E _cell l = E° _cell
B) E° _cell = 0
C) = 1
D) < K
E) = K

Question 26

When metal A is placed in a solution of metal ions B²⁺, a reaction occurs between A and B²⁺, and metal ions A²⁺ appear in the solution. When metal B is placed in acid solution, gas bubbles form on its surface. When metal A is placed in a solution of metal ions C²⁺, no reaction occurs. Which of the following reactions would not occur spontaneously?

A) C(s) + 2^H+(aq) → H₂(g) + C+(aq)
B) C(s) + A²⁺(aq) → A(s) + C²⁺(aq)
C) B(s) + C²⁺(aq) → C(s) + B²⁺(aq)
D) A(s) + 2^H+(aq) → H₂(g) + A²⁺(aq)
E) B(s) + 2H⁺(aq) → H₂(g) + B²⁺(aq)

Question 27

Examine the following half-reactions and select the strongest reducing agent among the species listed. HgO(s) + H2O(l) + 2e^-
Hg(l) + 2OH^-(aq) E°= 0.0977 V
Zn(OH)₂(s) + 2e^-
Zn(s) + 2OH^-(aq) E° = -1.25 V
Ag₂O(s) + H₂O(l) + 2e^-
Ag(s) + 2OH^-(aq) E° = 0.342 V
B(OH)₃(aq) + 7H⁺(aq) + 8e^-
BH4^-(aq) + 3H₂O(l) E° = -0.481 V

A) Hg(l)
B) Zn(s)
C) Ag(s)
D) BH₄^-(aq)
E) Zn(OH)₂(s)

Question 28

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co³⁺(aq) + e^-
Co²⁺(aq) E° = 1.82 V
MnO₄^-(aq) + 2H₂O(l) + 3e^- MnO₂(s) + 4OH^-(aq) E° = 0.59 V
Overall reaction:
MnO₄^-(aq) + 2H₂O(l) + 3Co²⁺(aq) → MnO₂(s) + 3Co³⁺(aq) + 4OH^-(aq)

A) E° _cell = -1.23 V, spontaneous
B) E° _cell = -1.23 V, nonspontaneous
C) E° _cell = 1.23 V, spontaneous
D) E° _cell = 1.23 V, nonspontaneous
E) E° _cell = -0.05 V, nonspontaneous

Question 29

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄(aq) + 8H(aq) + 8e Cl-(aq) + 4H₂O(l) E° = 1.389 V
VO₂(aq) + 2H(aq) + e^- j VO(aq) + H₂O(l) E° = 0.991 V

A) -0.398 V
B) -2.380 V
C) 0.398 V
D) 2.380 V
E) None of these choices are correct.

Question 30

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e- Cu(s) E° = 0.34 V
Sn⁴⁺(aq) + 2e- Sn²⁺(aq) E° = 0.13 V

A) 0.47 V
B) 0.21 V
C) -0.21 V
D) -0.47 V
E) 0.42 V

Question 31

Calculate E° _cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l) E° = 1.77 V
Fe³⁺ (aq) + e^- Fe²⁺(aq) E° = 0.77 V
Overall reaction:
2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq)

A) E° _cell = -1.00 V, nonspontaneous
B) E° _cell = -1.00 V, spontaneous
C) E° _cell = 1.00 V, nonspontaneous
D) E° _cell = 1.00 V, spontaneous
E) E° _cell = -0.23 V, nonspontaneous

Question 32

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s), indicates that

A) Co is the reducing agent.
B) Co²⁺ ions are oxidized.
C) Al is the reducing agent.
D) Al³⁺ is the reducing agent.
E) aluminum metal is the cathode.

Question 33

Examine the following half-reactions and select the strongest oxidizing agent among the substances. [PtCl₄]^2-(aq) + 2e^-
Pt(s) + 4Cl^-(aq) E° = 0.755 V
RuO₄(s) + 8H⁺(aq) + 8e^-
Ru(s) + 4H₂O(l) E° = 1.038 V
FeO₄^2-(aq) + 8H⁺(aq) + 3e^-
Fe³⁺(aq) + 4H₂O(l) E° = 2.07 V
H₄XeO₆(aq) + 2H⁺(aq) + 2e^-
XeO₃(aq) + 3H₂O(l) E° = 2.42 V

A) [PtCl₄]^2-(aq)
B) RuO₄(s)
C) HFeO₄^- (aq)
D) H₄XeO₆(aq)
E) Cl^-(aq)

Question 34

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I₂(s) + 2e^-
2I^-(aq) E° = 0.53 V
Cr³⁺(aq) + 3e^-
Cr(s) E° = -0.74 V
Overall reaction:
2Cr(s) + 3I₂(s) → 2Cr³⁺(aq) + (aq) + 6I^-(aq)

A) E°_cell = -1.27 V, spontaneous
B) E° _cell = -1.27 V, nonspontaneous
C) E° _cell = 1.27 V, spontaneous
D) E° _cell = 1.27 V, nonspontaneous
E) E° _cell = 1.54 V, spontaneous

Question 35

Calculate E° _cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O₂(g) + 4H⁺(aq) + 4e^-
2H₂O(l) E° = 1.229 V
Al³⁺(aq) + 3e^-
Al(s) E° = -1.662 V
Overall reaction:
4Al(s) + 3O₂(g) + 12H⁺(aq) → 4Al³⁺(aq) + 6H₂O(l)

A) E° _cell = -2.891 V, nonspontaneous
B) E° _cell = -2.891 V, spontaneous
C) E° _cell = 2.891 V, nonspontaneous
D) E° _cell = 2.891 V, spontaneous
E) None of these choices are correct.

Question 36

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄(aq) + 3e^-
Au(s) + 4Br^-(aq) E° = 0.854 V
Mn²⁺(aq) + 2e^-
Mn(s) E° = -1.185 V
K⁺(aq) + e^-
K(s) E° = -2.931 V
F₂O(aq) + 2H⁺(aq) + 4e^-
2F^-(aq) + H₂O(l) E° = 2.153 V

A) AuBr₄^-(aq)
B) Mn²⁺(aq)
C) K⁺(aq)
D) F₂O(aq)
E) H⁺(aq)

Question 37

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e- Hg₂²⁺(aq) E° = 0.92 V
Cr³⁺(aq) + 3e- Cr(s) E° = -0.74 V

A) -0.18 V
B) 0.18 V
C) 1.28 V
D) 1.66 V
E) 2.12 V

Question 38

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s) + 2e_-
Pb(s) + 2I^-(aq) E° = -0.365 V
Ca²⁺(aq) + 2e^-
Ca(s) E° = -2.868 V
Pt²⁺(aq) + 2e^-
Pt(s) E° = 1.18 V
Br₂(l) + 2e^-
2Br^-(aq) E° = 1.066 V

A) Pb(s)
B) Ca(s)
C) Pt(s)
D) Br^-(aq)
E) Pt²⁺(aq)

Question 39

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s), indicates that

A) copper metal is a product of the cell reaction.
B) hydrogen gas (H₂) is a product of the cell reaction.
C) Cu is the anode.
D) Pt is the cathode.
E) Cu²⁺ is the reducing agent.

Question 40

Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)₃(s) + 3e^-
Cr(s) + 3OH^-(aq) E° = -1.48 V
SnO₂(s) + 2H₂O(l) + 4e^-
Sn(s) + 4OH^-(aq) E° = -0.945 V
MnO₂(s) + 4H⁺(aq) + 2e^-
Mn²⁺(aq) + 2H₂O(l) E° = 1.224 V
Hg₂SO₄(s) + 2e^-
2Hg(l) + SO₄^2-(aq) E° = 0.613 V

A) Cr(s)
B) Sn(s)
C) Mn²⁺(aq)
D) Hg(l)
E) OH^-(aq)

Question 41

Consider the reaction in the lead-acid cell Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(aq) + 2H₂O(l)
For which E° _cell = 2.04 V at 298 K. ΔG° for this reaction is

A) -3.94 × 10⁵ kJ.
B) -3.94 × 10² kJ.
C) -1.97 × 10⁵ kJ.
D) -7.87 × 10² kJ.
E) None of these choices are correct.

Question 42

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) 2NaCl(s) + Fe(s)
For which E° _cell = 2.35 V at 200°C. ΔG° at this temperature is

A) 453 kJ.
B) -453 kJ.
C) 907 kJ.
D) -907 kJ.
E) None of these choices are correct.

Question 43

The following half-reactions occur in the mercury battery used in calculators. If E° _cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25°C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H₂O(l) + 2e^-
Hg(l) + 2OH^-(aq)
ZnO(s) + H₂O(l) + 2e^-
Zn(s) + 2OH^-(aq)

A) 9.4 × 10²²
B) 7.5 × 10⁴⁵
C) 6.4 × 10⁶³
D) 7.8 × 10⁹¹
E) > 9.9 × 10⁹⁹

Question 44

A voltaic cell consists of a Mn/Mn²⁺ electrode (E° = -1.18 V) and a Fe/Fe²⁺ electrode (E° = -0.44 V). Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E _cell = 0.78 V at 25°C.

A) 0.040 M
B) 0.24 M
C) 1.1 M
D) 1.8 M
E) None of these choices are correct.

Question 45

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V). Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

A) 0.001 M
B) 0.002 M
C) 0.01 M
D) 0.02 M
E) 0.04 M

Question 46

A voltaic cell consists of a Hg/Hg2²⁺ electrode (E° = 0.85 V) and a Sn/Sn²⁺ electrode (E° = -0.14 V). Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

A) 0.0001 M
B) 0.0007 M
C) 0.005 M
D) 0.03 M
E) 0.05 M

Question 47

A battery is considered "dead" when

A) < 1.
B) = 1.
C) > 1.
D) = K.
E) /K = 0.

Question 48

A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V) and a Fe/Fe²⁺ electrode (E° = -0.44 V). If E_cell = 0 and the temperature is 25°C, what is the ratio [Fe²⁺]/[Cd²⁺]?

A) 2 × 10¹
B) 1 × 10¹
C) 1
D) 1 × 10^-1
E) 5 × 10^-2

Question 49

A voltaic cell consists of a Ag/Ag⁺ electrode (E° = 0.80 V) and a Fe²⁺/Fe³⁺ electrode (E° = 0.77 V) with the following initial molar concentrations: [Fe²⁺] = 0.30 M; [Fe³⁺] = 0.10 M; [Ag⁺] = 0.30 M. What is the equilibrium concentration of Fe³⁺? (Assume the anode and cathode solutions are of equal volume, and a temperature of 25°C.)

A) 0.030 M
B) 0.043 M
C) 0.085 M
D) 0.11 M
E) 0.17 M

Question 50

Calculate ΔG° for the reaction of iron(II) ions with one mole of permanganate ions. MnO₄-(aq) + 8H+(aq) + 5e- Mn₂+(aq) + 4H₂O(l) E° = 1.51 V
Fe³⁺(aq) + e^-
Fe²⁺(aq) E°= 0.77 V

A) -71.4 kJ
B) -286 kJ
C) -357 kJ
D) -428 kJ
E) None of these choices are correct.

Question 51

Consider the reaction of iodine with manganese dioxide 3I₂(s) + 2MnO₂(s) + 8OH^-(aq) 6I^-(aq) + 2MnO₄(aq) + 4H₂O(l)
The equilibrium constant for the overall reaction is 8.30 × 10^-7. Calculate E° _cell for the reaction at 25°C.

A) -0.36 V
B) -0.18 V
C) -0.12 V
D) -0.060 V
E) None of these choices are correct.

Question 52

The value of E° _cell for the reaction 2Cr³⁺(aq) + 6Hg(l) → 2Cr(s) + 3Hg₂²⁺(aq)
Is 1.59 V. Calculate ΔG° for the reaction.

A) -921 kJ
B) -767 kJ
C) -460 kJ
D) -307 kJ
E) None of these choices are correct.

Question 53

Calculate the potential of a voltaic cell (E° _cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

A) 2.17 × 10³ V
B) 2.17 × 10^-3 V
C) 2.17 V
D) 13.6 V
E) 1.36 × 10^-2 V

Question 54

What is the value of the equilibrium constant for the cell reaction below at 25°C? E° _cell = 0.61 V 2Cr(s) + 3Pb²⁺(aq) 3Pb(s) + 2Cr³⁺(aq)

A) 4.1 × 10²⁰
B) 8.2 × 10³⁰
C) 3.3 × 10⁵¹
D) 7.4 × 10⁶¹
E) > 9.9 × 10⁹⁹

Question 55

A concentration cell consists of two Zn/Zn²⁺ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO₃)₂ and in compartment B is 0.60 M Zn(NO₃)₂. What is the voltage of the cell at 25°C?

A) 0.010 V
B) 0.020 V
C) 0.023 V
D) 0.046 V
E) None of these choices are correct.

Question 56

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 10⁵. Calculate ΔG° for the reaction at 25°C.

A) -12.6 kJ
B) -28.9 kJ
C) 12.6 kJ
D) 28.9 kJ
E) None of these choices are correct.

Question 57

Consider the reaction of iodine with manganese dioxide 3I₂(s) + 2MnO₂(s) + 8OH^-(aq) 6I^-(aq) + 2MnO₄(aq) + 4H₂O(l)
The equilibrium constant for the overall reaction is 8.30 × 10^-7. Calculate ΔG° for the reaction at 25°C.

A) -15.1 kJ
B) -34.7 kJ
C) 15.1 kJ
D) 34.7 kJ
E) None of these choices are correct.

Question 58

What is the value of the equilibrium constant for the cell reaction below at 25°C? E° _cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

A) 1.2 × 10⁵
B) 1.4 × 10¹⁰
C) 8.6 × 10^-6
D) 7.1 × 10^-11
E) 2.3 × 10²³

Question 59

Calculate ΔG° for the oxidation of 3 moles of copper by nitric acid. Cu²⁺(aq) + 2e^-
Cu(s) E° = 0.34 V
NO₃^-(aq) + 4H⁺(aq) + 3e^-
NO(g) + 2H²O(l) E° = 0.957 V

A) -120 kJ
B) -180 kJ
C) -240 kJ
D) -300 kJ
E) -360 kJ

Question 60

Calculate E° _cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 10⁵ Ni²⁺(aq) + Cd(s) → Cd²⁺(aq) + Ni(s)

A) 0.075 V
B) 0.10 V
C) 0.12 V
D) 0.15 V
E) 0.30 V

Question 61

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

A) copper, Cu, E° = 0.15 V
B) cobalt, Co, E° = -0.28 V
C) chromium, Cr, E° = -0.74 V
D) tin, Sn, E° = -0.14 V
E) None of these metals would be capable of acting as a sacrificial anode with iron.

Question 62

Which one of the following statements relating to the glass electrode is correct?

A) The glass electrode detects hydrogen gas.
B) The glass of a glass electrode serves to conduct electrons.
C) When pH is measured, only a single electrode, the glass electrode, need be used.
D) The potential of the glass electrode varies linearly with the pH of the solution.
E) None of these choices are correct.

Question 63

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

A) sodium from Na₃PO₄(aq)
B) sulfur from K₂SO₄(aq)
C) oxygen from H₂SO₄(aq)
D) potassium from KCl(aq)
E) nitrogen from AgNO₃(aq)

Question 64

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

A) 16.2 g
B) 33.4 g
C) 40.6 g
D) 81.3 g
E) 163 g

Question 65

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products).

A) calcium and bromine
B) sodium and fluorine
C) calcium bromide
D) calcium and fluorine
E) sodium and bromine

Question 66

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

A) 1.1 A
B) 2.2 A
C) 3.3 A
D) 4.4 A
E) 5.5 A

Question 67

Electrolytic cells utilize electrical energy to drive nonspontaneous redox reactions.

Question 68

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr₂O7^2-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

A) 6.2 minutes
B) 12.4 minutes
C) 18.6 minutes
D) 24.7 minutes
E) 37.1 minutes

Question 69

What product forms at the cathode during the electrolysis of molten lithium iodide?

A) Li⁺(l)
B) Li(l)
C) I^-(l)
D) I₂(g)
E) I₃^-(l)

Question 70

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) → MnO₂(s) + 4H⁺(aq) + 2e^- What mass of MnO2 is deposited at this anode?

A) 19.5 kg
B) 12.9 kg
C) 4.87 kg
D) 2.43 kg
E) None of these choices are correct.

Question 71

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

A) potassium ion
B) nitrate ion
C) water
D) oxygen
E) hydronium ion

Question 72

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

A) phosphorus from K₃PO₄(aq)
B) sodium from NaBr(aq)
C) aluminum from AlCl₃(aq)
D) fluorine from KF(aq)
E) iodine from NaI(aq)

Question 73

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

A) manganese, Mn, E° = -1.18 V
B) cadmium, Cd, E° = -0.40 V
C) magnesium, Mg, E° = -2.37 V
D) zinc, Zn, E° = -0.76 V
E) All of these metals are capable of acting as sacrificial anodes with iron.

Question 74

A battery that cannot be recharged is a

A) fuel cell.
B) primary battery.
C) secondary battery.
D) simple battery.
E) flow battery.

Question 75

What product forms at the anode during the electrolysis of molten NaBr?

A) Na⁺(l)
B) Na(l)
C) Br^-(l)
D) Br3^-(l)
E) Br₂(g)

Question 76

A concentration cell consists of two Al/Al³⁺electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃)₃ and in compartment B is 1.25 M Al(NO₃)₃. What is the voltage of the cell at 25°C?

A) 0.083 V
B) 0.062 V
C) 0.041 V
D) 0.028 V
E) None of these choices are correct.

Question 77

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

A) sodium and sulfur
B) hydrogen and sulfur
C) oxygen and sulfur
D) oxygen and sulfuric acid
E) hydrogen and oxygen

Question 78

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu²⁺(aq) + 2e^- → Cu(s) and Ag⁺(aq) + e_- → Ag(s)
For every 1.00 g of copper produced in the first process, how many grams of silver will be
Produced in the second one?

A) 0.294 g
B) 0.588 g
C) 0.850 g
D) 1.70 g
E) 3.40 g

Question 79

How many grams of oxygen gas will be produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H₂O(l) → 2H₂(g) + O₂(g)

A) 31.7 g
B) 15.9 g
C) 7.94 g
D) 3.97 g
E) 1.98 g

Question 80

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

A) 0.419 g
B) 6.29 g
C) 12.6 g
D) 25.2 g
E) 33.4 g