Question 1

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

Accepted Answer

A)   Li+(l) 
B)   Li(l) 
C)   I-(l) 
D)   I2(g) 
E)   I3-(l) F) A) and D)
G) A) and C)

Question 2

If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter?

Accepted Answer

A)   2.36 V
B)   1.56 V
C)   0.04 V
D)   -0.04 V
E)   -2.36 VF) A) and E)
G) A) and B)

Question 3

Based on the data presented below, which is the strongest oxidizing agent? 3+ B)  Fe2+ C)  Br- D)  Al3+ E)  Al(s) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Fe3+
B)   Fe2+
C)   Br-
D)   Al3+
E)   Al(s) F) None of the above
G) C) and D)

Question 4

What is E°cell for the following reaction, and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq)  + 2H2O(l)  → H2O2(aq)  + 2H+(aq)  + 2Fe2+(aq) 
Given: cell for the following reaction, and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq)  + 2H2O(l)  → H2O2(aq)  + 2H+(aq)  + 2Fe2+(aq)  Given:   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" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

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, nonspontaneousF) B) and C)
G) B) and D)

Question 5

Which component of the following cell is the cathode? K|L||M|N

Accepted Answer

A)   K
B)   L
C)   M
D)   NE) B) and C)
F) A) and D)

Question 6

What mass of nickel may be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Accepted Answer

A)   0.20 g Ni
B)   0.40 g Ni
C)   12 g Ni
D)   24 g Ni
E)   47 g NiF) A) and C)
G) A) and B)

Question 7

If E° for X + e- → Y is larger than E° for A + 2e- → B, then in a spontaneous process under standard-state conditions,

Accepted Answer

A)   X will oxidize A.
B)   Y will oxidize A.
C)   Y will reduce A.
D)   B will oxidize X.
E)   B will reduce X.F) A) and B)
G) A) and C)

Question 8

What is ΔG° at 298 K for the following reaction? (F = 96,500 C • mol -1)   -1)    A)  -921 kJ/mol B)  -767 kJ/mol C)  -460 kJ/mol D)  -307 kJ/mol E)  -1840 kJ/mol" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -921 kJ/mol
B)   -767 kJ/mol
C)   -460 kJ/mol
D)   -307 kJ/mol
E)   -1840 kJ/molF) A) and C)
G) B) and D)

Question 9

What is the cell potential at 25°C for the following reaction if [Zn2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol, F = 96,500 C • mol -1)  2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol, F = 96,500 C • mol -1)    A)  -0.62 V B)  +0.52 V C)  -0.52 V D)  -0.72 V E)  +0.72 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -0.62 V
B)   +0.52 V
C)   -0.52 V
D)   -0.72 V
E)   +0.72 VF) C) and D)
G) A) and B)

Question 10

Consider the following redox equation. Mn(OH) 2(s)  + MnO4-(aq)  → MnO42-(aq)  (basic solution) 
When the equation is balanced with the smallest whole number coefficients, what is the coefficient for OH-(aq)  and on which side of the equation is OH-(aq)  present?

Accepted Answer

A)   4, reactant side
B)   4, product side
C)   6, reactant side
D)   6, product side
E)   8, reactant sideF) D) and E)
G) C) and E)

Question 11

When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Zn(s) ? Zn(s)  + ReO4-(aq)  → Re(s)  + Zn2+(aq)  (acidic solution)

Accepted Answer

A)   2
B)   7
C)   8
D)   16
E)   None of these choices is correct.F) A) and D)
G) B) and E)

Question 12

For E° and ΔG° the zero (superscript) represents the standard state. What is the standard state?

Accepted Answer

For gases, partial p...

Question 13

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 Ecell = 1.15 V at 25°C.

Accepted Answer

A)   0.0010 M
B)   0.0020 M
C)   0.010 M
D)   0.020 M
E)   0.41 MF) B) and E)
G) C) and D)

Question 14

Lithium-ion batteries can be recharged many times.

Accepted Answer

A) True 
 B)False

Question 15

Which of the following is correct?

Accepted Answer

A)   total charge = volts/coulombs
B)   electrical energy = volts × coulombs
C)   Faraday = coulombs/joules
D)   coulombs = joules × volts
E)   electrical work = Faraday's constant/EcellF) All of the above
G) B) and E)

Question 16

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

Accepted Answer

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

Question 17

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Accepted Answer

A)   Pb.
B)   Ag.
C)   Sn.
D)   Mg.
E)   Cu.F) B) and E)
G) B) and C)

Question 18

Reduction occurs at the anode of a galvanic cell.

Accepted Answer

A) True 
 B)False

Question 19

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 Ecell = 1.04 V at 25°C.

Accepted Answer

A)   0.00010 M
B)   0.00070 M
C)   0.0049 M
D)   0.030 M
E)   0.050 MF) A) and E)
G) A) and B)

Question 20

Given Cu2+(aq)  + 2e- → Cu(s)  E° = +0.34 V Al3+(aq)  + 3e- → Al(s)  E° = -1.66 V
Na+(aq)  + e- → Na(s)  E° = -2.71 V
Which of the following reactions will occur?

Accepted Answer

A)   2Na+(aq)  + Cu(s)  → Cu2+(aq)  + 2Na(s) 
B)   Al(s)  + 3Na+(aq)  → Al3+(aq)  + 3Na(s) 
C)   2Na(s)  + Cu2+(aq)  → Cu(s)  + 2Na+(aq) 
D)   2Al3+(aq)  + 3Cu(s)  → 3Cu2+(aq)  + 2Al(s) 
E)   None of these will occur.F) B) and D)
G) A) and C)

Exam 19: Electrochemistry

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

Correct AnswerverifiedShow Answer

What is ΔG° at 298 K for the following reaction? (F = 96,500 C • mol -1)

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Reduction occurs at the anode of a galvanic cell.

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When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Zn(s) ? Zn(s) + ReO4-(aq) → Re(s) + Zn2+(aq) (acidic solution)

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Consider the following redox equation. Mn(OH) 2(s) + MnO4-(aq) → MnO42-(aq) (basic solution) When the equation is balanced with the smallest whole number coefficients, what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

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What is the cell potential at 25°C for the following reaction if [Zn2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol, F = 96,500 C • mol -1)

Correct AnswerverifiedShow Answer

What mass of nickel may be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Correct AnswerverifiedShow Answer

Lithium-ion batteries can be recharged many times.

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For E° and ΔG° the zero (superscript) represents the standard state. What is the standard state?

Correct AnswerverifiedFor gases, partial p...View AnswerShow Answer

If E° for X + e- → Y is larger than E° for A + 2e- → B, then in a spontaneous process under standard-state conditions,

Correct AnswerverifiedShow Answer

Based on the data presented below, which is the strongest oxidizing agent?

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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 Ecell = 1.04 V at 25°C.

Correct AnswerverifiedShow Answer

Given Cu2+(aq) + 2e- → Cu(s) E° = +0.34 V Al3+(aq) + 3e- → Al(s) E° = -1.66 V Na+(aq) + e- → Na(s) E° = -2.71 V Which of the following reactions will occur?

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If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter?

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What is E°cell for the following reaction, and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq) Given:

Correct AnswerverifiedShow Answer

Which component of the following cell is the cathode? K|L||M|N

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Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Correct AnswerverifiedShow Answer

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 Ecell = 1.15 V at 25°C.

Correct AnswerverifiedShow Answer

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

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Which of the following is correct?

Correct AnswerverifiedShow Answer

Correct Answer
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What is ΔG° at 298 K for the following reaction? (F = 96,500 C • mol^-1)

Correct Answer
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Correct Answer
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When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Zn(s) ? Zn(s) + ReO₄^-(aq) → Re(s) + Zn²⁺(aq) (acidic solution)

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

Correct Answer
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What is the cell potential at 25°C for the following reaction if [Zn²⁺] = 1.0 × 10^-4^M and [Sn²⁺] = 0.20 M ? (R = 8.314 J/K • mol, F = 96,500 C • mol^-1)

Correct Answer
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What mass of nickel may be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min?

Correct Answer
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Correct Answer
verified

Correct Answer
verified
For gases, partial p...
View Answer

If E° for X + e^- → Y is larger than E° for A + 2e^- → B, then in a spontaneous process under standard-state conditions,

Correct Answer
verified

Correct Answer
verified

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.

Correct Answer
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Given Cu²⁺(aq) + 2e^- → Cu(s) E° = +0.34 V Al³⁺(aq) + 3e^- → Al(s) E° = -1.66 V Na⁺(aq) + e^- → Na(s) E° = -2.71 V Which of the following reactions will occur?

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Correct Answer
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What is E°_cell for the following reaction, and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq) Given:

Correct Answer
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Correct Answer
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Correct Answer
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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 = 1.15 V at 25°C.

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

Correct Answer
verified

Correct Answer
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