Question 1

What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq)  3+(aq)    Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)  A) Fe(s)  B) Fe3+(aq)  C) Cl2(g)  D) Cl⁻(aq)  E) Pt(s) " class="answers-bank-image d-inline" rel="preload" > Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)

Accepted Answer

A)  Fe(s) 
B)  Fe3+(aq) 
C)  Cl2(g) 
D)  Cl⁻(aq) 
E)  Pt(s)

Question 2

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Al(s) ∣ Al3+(aq, 0.115 mol L-1)  3+(aq, 0.115 mol L-1)    Al3+(aq, 3.89 mol L-1) ∣ Al(s)  E°(Al3+/Al) = -1.66 V A) +1.66 V B) +0.060 V C) 0.00 V D) +0.090 V E) +0.030 V" class="answers-bank-image d-inline" rel="preload" > Al3+(aq, 3.89 mol L-1) ∣ Al(s) 
E°(Al3+/Al) = -1.66 V

Accepted Answer

A)  +1.66 V
B)  +0.060 V
C)  0.00 V
D)  +0.090 V
E)  +0.030 V

Question 3

Determine the cell notation for the redox reaction given below: 3Cl2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)

Accepted Answer

A)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)  2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)  
A)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)    Fe(s) ∣ Fe3+(aq)  
B)  Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)    Fe3+(aq)  ∣ Fe(s)  
C)  Fe3+(aq) ∣ Fe(s)    Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)  
D)  Fe(s) ∣ Cl2(g)    Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s)  
E)  Fe(s) ∣ Fe3+(aq)    Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Fe(s) ∣ Fe3+(aq) 
B)  Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)  2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)  
A)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)    Fe(s) ∣ Fe3+(aq)  
B)  Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)    Fe3+(aq)  ∣ Fe(s)  
C)  Fe3+(aq) ∣ Fe(s)    Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)  
D)  Fe(s) ∣ Cl2(g)    Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s)  
E)  Fe(s) ∣ Fe3+(aq)    Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Fe3+(aq)  ∣ Fe(s) 
C)  Fe3+(aq) ∣ Fe(s)  2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)  
A)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)    Fe(s) ∣ Fe3+(aq)  
B)  Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)    Fe3+(aq)  ∣ Fe(s)  
C)  Fe3+(aq) ∣ Fe(s)    Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)  
D)  Fe(s) ∣ Cl2(g)    Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s)  
E)  Fe(s) ∣ Fe3+(aq)    Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s) 
D)  Fe(s) ∣ Cl2(g)  2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)  
A)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)    Fe(s) ∣ Fe3+(aq)  
B)  Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)    Fe3+(aq)  ∣ Fe(s)  
C)  Fe3+(aq) ∣ Fe(s)    Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)  
D)  Fe(s) ∣ Cl2(g)    Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s)  
E)  Fe(s) ∣ Fe3+(aq)    Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s) 
E)  Fe(s) ∣ Fe3+(aq)  2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)  
A)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)    Fe(s) ∣ Fe3+(aq)  
B)  Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)    Fe3+(aq)  ∣ Fe(s)  
C)  Fe3+(aq) ∣ Fe(s)    Cl⁻(aq) ∣ Cl2(g) ∣ Pt(s)  
D)  Fe(s) ∣ Cl2(g)    Fe3+(aq) ∣ Cl⁻(aq) ∣ Pt(s)  
E)  Fe(s) ∣ Fe3+(aq)    Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)

Question 4

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Accepted Answer

A)  Sn4+(aq) + Mg(s) ; if Eo(Sn4+/Sn2+) = +0.15V and Eo(Mg2+/Mg) = -2.37V
B)  Cr3+(aq) + Ni(s) ; if Eo(Cr3+/Cr) = -0.73V and Eo(Ni2+/Ni) = -0.23V
C)  Zn(s) + Na+(aq) ; if Eo(Zn2+/Zn) = -0.76V and Eo(Na+/Na) = -2.71V
D)  Fe(s) + Ba2+(aq) ; if Eo(Fe3+/Fe) = -0.04V and Eo(Ba2+/Ba) = -2.90V
E)  Ni2+(aq) + NO(g) ; if Eo(Ni2+/Ni) = -0.23V and Eo(NO3-/NO) = +0.96V

Question 5

What element is being oxidized in the following (unbalanced) redox reaction? MnO4⁻ (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

Accepted Answer

A)  C
B)  O
C)  Mn
D)  H

Question 6

Which of the following metals will dissolve in HCl?

Accepted Answer

A)  Au; Eo(Au3+/Au) = -1.50V
B)  Ag; Eo(Ag+/Ag) = +0.80V
C)  Cu; Eo(Cu2+/Cu) = +0.34V
D)  Al; Eo(Al3+/Al) = -1.66V
E)  Pt; Eo(Pt2+/Pt) = +1.19V

Question 7

Consider the following standard reduction potentials: Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V
I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V
Under standard conditions,

Accepted Answer

A)  Ni2+(aq) is a stronger oxidizing agent than I2(s) , and I-(aq) is a stronger reducing agent than Ni(s) .
B)  I2(s) is a stronger oxidizing agent than Ni2+(aq) , and Ni(s) is a stronger reducing agent than I-(aq) .
C)  Ni(s) is a stronger oxidizing agent than I-(aq) , and Ni2+(aq) is a stronger reducing agent than I2(s) .
D)  I-(aq) is a stronger oxidizing agent than Ni(s) , and I2(s) is a stronger reducing agent than Ni2+(aq) .

Question 8

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn (s) E° = -0.763 V
The concentrations of zinc ion in the two compartments are 5.50 mol L-1 and 1.11 × 10-2 mol L-1, respectively. The cell emf is ________ V.

Accepted Answer

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

Question 9

Determine the cell notation for the redox reaction given below: Pb(s) + 2H⁺(aq) → Pb2+(aq) + H2(g)

Accepted Answer

A)  H+(aq) ∣ H2(g) ∣ Pt(s)  2+(aq) + H2(g)  
A)  H+(aq) ∣ H2(g) ∣ Pt(s)    Pb(s) ∣ Pb2+(aq)  
B)  H2(g) ∣ H+(aq) ∣ Pt(s)    Pb2+(aq) ∣ Pb(s)  
C)  Pb2+(aq) ∣ Pb(s)    H2(g) ∣ H+(aq) ∣ Pt(s)  
D)  Pb(s) ∣ Pb2+(aq)    H+(aq) ∣ H2(g) ∣ Pt(s)  
E)  Pb(s) ∣ H2(g)    Pb2+(aq) ∣ H+(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Pb(s) ∣ Pb2+(aq) 
B)  H2(g) ∣ H+(aq) ∣ Pt(s)  2+(aq) + H2(g)  
A)  H+(aq) ∣ H2(g) ∣ Pt(s)    Pb(s) ∣ Pb2+(aq)  
B)  H2(g) ∣ H+(aq) ∣ Pt(s)    Pb2+(aq) ∣ Pb(s)  
C)  Pb2+(aq) ∣ Pb(s)    H2(g) ∣ H+(aq) ∣ Pt(s)  
D)  Pb(s) ∣ Pb2+(aq)    H+(aq) ∣ H2(g) ∣ Pt(s)  
E)  Pb(s) ∣ H2(g)    Pb2+(aq) ∣ H+(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Pb2+(aq) ∣ Pb(s) 
C)  Pb2+(aq) ∣ Pb(s)  2+(aq) + H2(g)  
A)  H+(aq) ∣ H2(g) ∣ Pt(s)    Pb(s) ∣ Pb2+(aq)  
B)  H2(g) ∣ H+(aq) ∣ Pt(s)    Pb2+(aq) ∣ Pb(s)  
C)  Pb2+(aq) ∣ Pb(s)    H2(g) ∣ H+(aq) ∣ Pt(s)  
D)  Pb(s) ∣ Pb2+(aq)    H+(aq) ∣ H2(g) ∣ Pt(s)  
E)  Pb(s) ∣ H2(g)    Pb2+(aq) ∣ H+(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > H2(g) ∣ H+(aq) ∣ Pt(s) 
D)  Pb(s) ∣ Pb2+(aq)  2+(aq) + H2(g)  
A)  H+(aq) ∣ H2(g) ∣ Pt(s)    Pb(s) ∣ Pb2+(aq)  
B)  H2(g) ∣ H+(aq) ∣ Pt(s)    Pb2+(aq) ∣ Pb(s)  
C)  Pb2+(aq) ∣ Pb(s)    H2(g) ∣ H+(aq) ∣ Pt(s)  
D)  Pb(s) ∣ Pb2+(aq)    H+(aq) ∣ H2(g) ∣ Pt(s)  
E)  Pb(s) ∣ H2(g)    Pb2+(aq) ∣ H+(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > H+(aq) ∣ H2(g) ∣ Pt(s) 
E)  Pb(s) ∣ H2(g)  2+(aq) + H2(g)  
A)  H+(aq) ∣ H2(g) ∣ Pt(s)    Pb(s) ∣ Pb2+(aq)  
B)  H2(g) ∣ H+(aq) ∣ Pt(s)    Pb2+(aq) ∣ Pb(s)  
C)  Pb2+(aq) ∣ Pb(s)    H2(g) ∣ H+(aq) ∣ Pt(s)  
D)  Pb(s) ∣ Pb2+(aq)    H+(aq) ∣ H2(g) ∣ Pt(s)  
E)  Pb(s) ∣ H2(g)    Pb2+(aq) ∣ H+(aq) ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Pb2+(aq) ∣ H+(aq) ∣ Pt(s)

Question 10

Identify the battery that is used as a common flashlight battery.

Accepted Answer

A)  dry-cell battery
B)  lithium-ion battery
C)  lead-acid storage battery
D)  NiCad battery
E)  fuel cell

Question 11

Which of the following reactions would be the most spontaneous at 298 K?

Accepted Answer

A)  A + 2 B → C; E°cell = +0.98 V
B)  A + B → 2 C; E°cell = -0.030 V
C)  A + B → 3 C; E°cell = +0.15 V
D)  A + B → C; E°cell = +1.22 V
E)  A + B → C; E°cell = -1.22 V

Question 12

Which of the following is the strongest reducing agent?

Accepted Answer

A)  Al(s) 
B)  Zn(s) 
C)  Mg(s) 
D)  Al3+(aq) 
E)  Mg2+(aq)

Question 13

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Mg(s) ∣ Mg2+(aq, 2.74 mol L-1)  2+(aq, 2.74 mol L-1)    Cu2+(aq, 0.0033 mol L-1) ∣ Cu(s)  E°(Mg2+/Mg) = -2.37 V and E°(Cu2+/Cu) = +0.34 V A) -2.80 V B) +2.62 V C) +2.71 V D) +2.12 V E) -1.94 V" class="answers-bank-image d-inline" rel="preload" > Cu2+(aq, 0.0033 mol L-1) ∣ Cu(s) 
E°(Mg2+/Mg) = -2.37 V and E°(Cu2+/Cu) = +0.34 V

Accepted Answer

A)  -2.80 V
B)  +2.62 V
C)  +2.71 V
D)  +2.12 V
E)  -1.94 V

Question 14

Match the following.

-Q = 1

Accepted Answer

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

Question 15

In the presence of which of the following would iron be under the highest risk of rusting?

Accepted Answer

A)  salt only
B)  moisture only
C)  acid only
D)  salt and moisture combined
E)  salt, moisture, and acid together

Question 16

Use the provided reduction potentials to calculate ΔrG° for the following balanced redox reaction: Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) 
E°(Pb2+/Pb) = -0.13 V and E°(Cu2+/Cu) = +0.34 V

Accepted Answer

A)  -41 kJ mol-1
B)  -0.47 kJ mol-1
C)  +46 kJ mol-1
D)  +91 kJ mol-1
E)  -21 kJ mol-1

Question 17

Match the following.

-Q > K

Accepted Answer

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

Question 18

Which of the following is the weakest reducing agent?

Accepted Answer

A)  Br2(l) 
B)  Au3+(aq) 
C)  Ag(s) 
D)  Br⁻(aq) 
E)  Au(s)

Question 19

How many electrons are transferred in the following reaction? (The reaction is unbalanced.)  Fe2+(aq) + K(s) → Fe(s) + K+(aq)

Accepted Answer

A)  1
B)  2
C)  3
D)  4
E)  6

Question 20

What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn2+(aq)  2+(aq)    Ag+(aq) ∣ Ag(s)  A) Sn(s)  B) Ag+(aq)  C) Sn2+(aq)  D) Ag(s)  E) Pt(s) " class="answers-bank-image d-inline" rel="preload" > Ag+(aq) ∣ Ag(s)

Accepted Answer

A)  Sn(s) 
B)  Ag+(aq) 
C)  Sn2+(aq) 
D)  Ag(s) 
E)  Pt(s)

Exam 18: Electrochemistry

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Fe2+(aq) + K(s) → Fe(s) + K+(aq)

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Determine the cell notation for the redox reaction given below: Pb(s) + 2H⁺(aq) → Pb2+(aq) + H2(g)

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Consider the following standard reduction potentials: Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Under standard conditions,

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What element is being oxidized in the following (unbalanced) redox reaction? MnO4⁻ (aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

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Match the following. -Q > K

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Al(s) ∣ Al3+(aq, 0.115 mol L-1) Al3+(aq, 3.89 mol L-1) ∣ Al(s) E°(Al3+/Al) = -1.66 V

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What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt(s)

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Use the provided reduction potentials to calculate ΔrG° for the following balanced redox reaction: Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) E°(Pb2+/Pb) = -0.13 V and E°(Cu2+/Cu) = +0.34 V

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Which of the following is the strongest reducing agent?

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Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

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In the presence of which of the following would iron be under the highest risk of rusting?

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Mg(s) ∣ Mg2+(aq, 2.74 mol L-1) Cu2+(aq, 0.0033 mol L-1) ∣ Cu(s) E°(Mg2+/Mg) = -2.37 V and E°(Cu2+/Cu) = +0.34 V

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A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn (s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 mol L-1 and 1.11 × 10-2 mol L-1, respectively. The cell emf is ________ V.

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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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Which of the following metals will dissolve in HCl?

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Which of the following reactions would be the most spontaneous at 298 K?

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Match the following. -Q = 1

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Identify the battery that is used as a common flashlight battery.

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Determine the cell notation for the redox reaction given below: 3Cl2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)

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Which of the following is the weakest reducing agent?

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How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Fe²⁺(aq) + K(s) → Fe(s) + K⁺(aq)

Correct Answer
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Determine the cell notation for the redox reaction given below: Pb(s) + 2H⁺(aq) → Pb²⁺(aq) + H₂(g)

Correct Answer
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Consider the following standard reduction potentials: Ni²⁺(aq) + 2 e^- → Ni(s) E° = -0.26 V I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Under standard conditions,

Correct Answer
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What element is being oxidized in the following (unbalanced) redox reaction? MnO₄⁻ (aq) + H₂C₂O₄(aq) → Mn²⁺(aq) + CO₂(g)

Correct Answer
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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: Al(s) ∣ Al³⁺(aq, 0.115 mol L^-1) Al³⁺(aq, 3.89 mol L^-1) ∣ Al(s) E°(Al³⁺/Al) = -1.66 V

Correct Answer
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What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe³⁺(aq) Cl₂(g) ∣ Cl⁻(aq) ∣ Pt(s)

Correct Answer
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Use the provided reduction potentials to calculate Δ_rG° for the following balanced redox reaction: Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq) E°(Pb²⁺/Pb) = -0.13 V and E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
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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: Mg(s) ∣ Mg²⁺(aq, 2.74 mol L^-1) Cu²⁺(aq, 0.0033 mol L^-1) ∣ Cu(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
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A voltaic cell is constructed with two Zn²⁺-Zn electrodes, where the half-reaction is Zn²⁺ + 2e^- → Zn (s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 mol L^-1 and 1.11 × 10^-² mol L^-1, respectively. The cell emf is ________ V.

Correct Answer
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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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Determine the cell notation for the redox reaction given below: 3Cl₂(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe³⁺(aq)

Correct Answer
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Correct Answer
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