Question 1

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

Accepted Answer

A)  K 
B)  L 
C)  M 
D)  N 
A)  K 
B)  L 
C)  M 
D)  N

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 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) 
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)

Question 3

Lithium-ion batteries can be recharged many times.

Accepted Answer

A) True 
 B)False

Question 4

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

Accepted Answer

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

Question 5

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

Question 6

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

Question 7

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:

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, nonspontaneous 
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 8

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

Question 9

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 V 
A)  2.36 V 
B)  1.56 V 
C)  0.04 V 
D)  -0.04 V 
E)  -2.36 V

Question 10

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

Accepted Answer

A)  Fe3+ 
B)  Fe2+ 
C)  Br- 
D)  Al3+ 
E)  Al(s) 
A)  Fe3+ 
B)  Fe2+ 
C)  Br- 
D)  Al3+ 
E)  Al(s)

Question 11

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)

Accepted Answer

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

Question 12

Reduction occurs at the anode of a galvanic cell.

Accepted Answer

A) True 
 B)False

Question 13

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. 
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.

Question 14

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. 
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.

Question 15

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

Accepted Answer

For gases, partial p

Question 16

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

Question 17

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

Question 18

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/Ecell 
A)  total charge = volts/coulombs 
B)  electrical energy = volts × coulombs 
C)  Faraday = coulombs/joules 
D)  coulombs = joules × volts 
E)  electrical work = Faraday's constant/Ecell

Question 19

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

Question 20

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

Exam 19: Electrochemistry

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

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?

Lithium-ion batteries can be recharged many times.

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

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?

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.

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:

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

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

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

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)

Reduction occurs at the anode of a galvanic cell.

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?

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

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

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.

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

Which of the following is correct?

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)

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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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?

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

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?

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.

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:

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)

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?

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

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.

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)

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?