Question 1

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl3 with an electrical current of 12.0 A?

Accepted Answer

A)  27.0
B)  9.00
C)  1.19 × 103
D)  2.90 × 105
E)  3.57 × 103F) C) and D)
G) A) and E)

Question 2

Given that E°red = -1.66 V for Al3+/Al at 25°C,find E° and E for the concentration cell expressed using shorthand notation below.
Al(s) ∣ Al3+(1.0 × 10-5 M) ∣∣ Al3+(0.100 M) ∣ Al(s)

Accepted Answer

A)  E° = 0.00 V and E = +0.24 V
B)  E° = 0.00 V and E = +0.12 V
C)  E° = -1.66 V and E = -1.42 V
D)  E° = -1.66 V and E = -1.54 VE) None of the above
F) B) and D)

Question 3

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Sn(s) ∣ Sn2+(aq,0.022 M) 2+(aq,0.022 M)  Ag+(aq,2.7 M) ∣ Ag(s)    A) 1.01 V B) -0.83 V C) 1.31 V D) 0.01 V E) -0.66 V" class="answers-bank-image d-inline" rel="preload" >Ag+(aq,2.7 M) ∣ Ag(s) 
2+(aq,0.022 M)  Ag+(aq,2.7 M) ∣ Ag(s)    A) 1.01 V B) -0.83 V C) 1.31 V D) 0.01 V E) -0.66 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  1.01 V
B)  -0.83 V
C)  1.31 V
D)  0.01 V
E)  -0.66 VF) None of the above
G) A) and E)

Question 4

Match the following.
-ΔG° < 0

Accepted Answer

A)  Ecell = E°cell
B)  Ecell = 0
C)  E°cell 
D)  Ecell 
E)  E°cell > 0F) Ecell > 0G) D) and F)
H) A) and B)

Question 5

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Cu(s) ∣ Cu2+(aq,0.0032 M) ∣∣ Cu2+(aq,4.48 M) ∣ Cu(s) 
2+(aq,0.0032 M) ∣∣ Cu2+(aq,4.48 M) ∣ Cu(s)    A) 0.00 V B) 0.093 V C) 0.34 V D) 0.186 V E) 0.052 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  0.00 V
B)  0.093 V
C)  0.34 V
D)  0.186 V
E)  0.052 VF) A) and D)
G) B) and C)

Question 6

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.
3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq) 
2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq)    A) 3.5 × 10-59 B) 1.1 × 1017 C) 2.4 × 1058 D) 8.9 × 10-18 E) 1.7 × 1029" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  3.5 × 10-59
B)  1.1 × 1017
C)  2.4 × 1058
D)  8.9 × 10-18
E)  1.7 × 1029F) B) and E)
G) D) and E)

Question 7

What is the oxidizing agent in the redox reaction represented by the following cell notation?
Sn(s) ∣ Sn2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

Accepted Answer

A)  Sn(s) 
B)  Ag+(aq) 
C)  Sn2+(aq) 
D)  Ag(s) 
E)  PtF) A) and D)
G) C) and D)

Question 8

Give the type of battery that most cars contain.

Accepted Answer

A)  lead-acid battery
B)  dry-cell battery
C)  alkaline battery
D)  nickel-cadmium battery
E)  nickel-metal hydride batteryF) A) and C)
G) A) and B)

Question 9

Give the criteria for a nonspontaneous reaction.

Accepted Answer

A) ΔG° cell > 0,K > 1 B) ΔG° > 0,E°cell > 0,K > 1 C) ΔG° > 0,E°cell 1 D) ΔG° cell > 0,K E) ΔG° > 0,E°cell < 0,K < 1F) A) and B) G) A) and C)

Question 10

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below?
Ni(s) ∣ Ni2+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s)

Accepted Answer

A)  Ni(s) + 2 Cl-(aq) → Ni2+(aq) + Cl2(g) 
B)  Ni(s) + Cl2(g) → Ni2+(aq) + 2 Cl-(aq) 
C)  Ni2+(aq) + 2 Cl-(aq) → Ni(s) + Cl2(g) 
D)  Ni2+(aq) + 2 Cl-(aq) → NiCl2(s) E) A) and D)
F) B) and D)

Question 11

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

Accepted Answer

A)  73.5 g
B)  24.5 g
C)  220.g
D)  147 g
E)  8.17 gF) B) and D)
G) A) and B)

Question 12

Identify oxidation.

Accepted Answer

A)  increase in oxidation number
B)  loss of electrons
C)  gain of electrons
D)  decrease in oxidation number
E)  both A and BF) B) and C)
G) A) and E)

Question 13

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) 
Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) 
2+(aq) → Cu(s) + Mg2+(aq)    A) 2.04 V B) -2.04 V C) 2.72 V D) -1.36 V E) 1.36 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  2.04 V
B)  -2.04 V
C)  2.72 V
D)  -1.36 V
E)  1.36 VF) A) and B)
G) A) and C)

Question 14

What is the reducing agent in the redox reaction represented by the following cell notation?
Ni(s) ∣ Ni2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

Accepted Answer

A)  Ni(s) 
B)  Ni2+(aq) 
C)  Ag+(aq) 
D)  Ag(s) 
E)  PtF) D) and E)
G) B) and D)

Question 15

Based on the following information,
Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V
Mg2+(aq) + 2 e- → 2 Mg(s) E° = -2.37 V
Which of the following chemical species is the strongest reducing agent?

Accepted Answer

A)  Cl2(g) 
B)  Mg2+(aq) 
C)  Cl-(aq) 
D)  Mg(s) E) A) and C)
F) None of the above

Question 16

A voltaic cell is constructed with two Zn2+-Zn electrodes,where the half-reaction is
Zn2+(aq) + 2e- → Zn(s) E° = -0.763 V
The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M,respectively.The cell emf is ________ V.

Accepted Answer

A)  -1.54 × 10-3
B)  -378
C)  0.0798
D)  0.160
E)  -0.761F) B) and D)
G) A) and E)

Question 17

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H2C2O4 and H2O in the balanced reaction?
MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

Accepted Answer

A)  H2C2O4 = 5,H2O = 8
B)  H2C2O4 = 1,H2O = 1
C)  H2C2O4 = 5,H2O = 1
D)  H2C2O4 = 1,H2O = 4
E)  H2C2O4 = 3,H2O = 2F) A) and C)
G) A) and B)

Question 18

Match the following.
-Q < K

Accepted Answer

A)  Ecell = E°cell
B)  Ecell = 0
C)  E°cell 
D)  Ecell 
E)  E°cell > 0F) Ecell > 0G) All of the above
H) D) and F)

Question 19

Which of the following metals,if coated onto iron,would prevent the corrosion (oxidation) of iron?

Accepted Answer

A)  Zn
B)  Cu
C)  Ag
D)  AuE) A) and B)
F) B) and D)

Question 20

Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction.
2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s) 
2+(aq) → 2 Al3+(aq) + 3 Mg(s)    A) 4.1 × 102 kJ B) 1.4 × 102 kJ C) -2.3 × 102 kJ D) -7.8 × 102 kJ E) 6.8 × 102 kJ" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  4.1 × 102 kJ
B)  1.4 × 102 kJ
C)  -2.3 × 102 kJ
D)  -7.8 × 102 kJ
E)  6.8 × 102 kJF) A) and B)
G) B) and C)

Exam 18: Electrochemistry

Match the following. -ΔG° < 0

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) ∣ Cu2+(aq,0.0032 M) ∣∣ Cu2+(aq,4.48 M) ∣ Cu(s)

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ∣ Sn2+(aq,0.022 M) Ag+(aq,2.7 M) ∣ Ag(s)

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A voltaic cell is constructed with two Zn2+-Zn electrodes,where the half-reaction is Zn2+(aq) + 2e- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M,respectively.The cell emf is ________ V.

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Give the type of battery that most cars contain.

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What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s) ∣ Ni2+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s)

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Given that E°red = -1.66 V for Al3+/Al at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Al(s) ∣ Al3+(1.0 × 10-5 M) ∣∣ Al3+(0.100 M) ∣ Al(s)

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Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq)

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What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

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Give the criteria for a nonspontaneous reaction.

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Match the following. -Q < K

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Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq)

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What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

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Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

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Which of the following metals,if coated onto iron,would prevent the corrosion (oxidation) of iron?

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Identify oxidation.

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Based on the following information, Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V Mg2+(aq) + 2 e- → 2 Mg(s) E° = -2.37 V Which of the following chemical species is the strongest reducing agent?

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How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl3 with an electrical current of 12.0 A?

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What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

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Correct Answer
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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) ∣ Cu²⁺(aq,0.0032 M) ∣∣ Cu²⁺(aq,4.48 M) ∣ Cu(s)

Correct Answer
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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ∣ Sn²⁺(aq,0.022 M) Ag⁺(aq,2.7 M) ∣ Ag(s)

Correct Answer
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A voltaic cell is constructed with two Zn²⁺-Zn electrodes,where the half-reaction is Zn²⁺(aq) + 2e^- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-² M,respectively.The cell emf is ________ V.

Correct Answer
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Correct Answer
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What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s) ∣ Ni²⁺(aq) ∣∣ Cl₂(g) ∣ Cl^-(aq) ∣ C(s)

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Given that E°_red = -1.66 V for Al³⁺/Al at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Al(s) ∣ Al³⁺(1.0 × 10^-5 M) ∣∣ Al³⁺(0.100 M) ∣ Al(s)

Correct Answer
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Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3 Mg(s)

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Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced. ) Mg(s) + Cu²⁺(aq) → Cu(s) + Mg²⁺(aq)

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What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn²⁺(aq) ∣∣ Ag⁺(aq) ∣ Ag(s)

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Correct Answer
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Correct Answer
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Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I₂(s) + 2 Fe(s) → 2 Fe³⁺(aq) + 6 I⁻(aq)

Correct Answer
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Correct Answer
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Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H₂C₂O₄and H₂O in the balanced reaction? MnO₄⁻(aq) + H₂C₂O₄(aq) → Mn²⁺(aq) + CO₂(g)

Correct Answer
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Correct Answer
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Correct Answer
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Based on the following information, Cl₂(g) + 2 e^- → 2 Cl^-(aq) E° = +1.36 V Mg²⁺(aq) + 2 e^- → 2 Mg(s) E° = -2.37 V Which of the following chemical species is the strongest reducing agent?

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How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl₃ with an electrical current of 12.0 A?

Correct Answer
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What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni²⁺(aq) ∣∣ Ag⁺(aq) ∣ Ag(s)

Correct Answer
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