Question 1

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)

Question 2

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 3

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 4

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 5

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 6

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 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

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 9

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 10

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 11

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 12

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 13

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 14

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 15

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 16

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 17

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 18

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 19

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 20

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

Exam 18: Electrochemistry

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

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Match the following. -Q = 1

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

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

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

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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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Which of the following metals will dissolve in HCl?

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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)

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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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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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Which of the following is the weakest reducing agent?

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

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Match the following. -Q > K

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Which of the following is the strongest reducing agent?

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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,

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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

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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

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

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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)

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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)

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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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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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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)

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Correct Answer
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Correct Answer
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Correct Answer
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