Question 1

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

Accepted Answer

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

Question 2

Which of the following is the weakest oxidizing agent?

Accepted Answer

A)  H2O2(aq) 
B)  Fe3+(aq) 
C)  ClO2(g) 
D)  I2(s) 
E)  Fe(s) 
A)  H2O2(aq) 
B)  Fe3+(aq) 
C)  ClO2(g) 
D)  I2(s) 
E)  Fe(s)

Question 3

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu2+, Ag+, Sn4+, Fe3+, Au3+

Accepted Answer

A)  Cu2+ 
B)  Ag+ 
C)  Sn4+ 
D)  Fe3+ 
E)  Au3+ 
A)  Cu2+ 
B)  Ag+ 
C)  Sn4+ 
D)  Fe3+ 
E)  Au3+

Question 4

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn2+(aq, 1.8 mol L-1)   Ag+(aq, 0.055 mol L-1) ∣ Ag(s)
E°(Sn2+/Sn) = -0.14 V and E°(Ag+/Ag) = +0.80 V

Accepted Answer

A)  -0.94 V 
B)  -0.85 V 
C)  +1.02 V 
D)  +0.98 V 
E)  +0.86 V 
A)  -0.94 V 
B)  -0.85 V 
C)  +1.02 V 
D)  +0.98 V 
E)  +0.86 V

Question 5

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 mol L-1) ∣∣ Al3+(0.100 mol L-1) ∣ Al(s)

Accepted Answer

A)  E° = 0.00 V and E = +0.24 V 
B)  E° = 0.00 V and E = +0.0789 V 
C)  E° = -1.66 V and E = -1.42 V 
D)  E° = -1.66 V and E = -1.54 V 
A)  E° = 0.00 V and E = +0.24 V 
B)  E° = 0.00 V and E = +0.0789 V 
C)  E° = -1.66 V and E = -1.42 V 
D)  E° = -1.66 V and E = -1.54 V

Question 6

What is the oxidizing 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)  Pt(s) 
A)  Ni(s) 
B)  Ni2+(aq) 
C)  Ag+(aq) 
D)  Ag(s) 
E)  Pt(s)

Question 7

Which of the following is the weakest oxidizing agent?

Accepted Answer

A)  Sn2+(aq) 
B)  Cr3+(aq) 
C)  Sn4+(aq) 
D)  Cr(s) 
E)  Sn(s) 
A)  Sn2+(aq) 
B)  Cr3+(aq) 
C)  Sn4+(aq) 
D)  Cr(s) 
E)  Sn(s)

Question 8

What is the reaction at the anode in a breathalyzer?

Accepted Answer

A)  Ethanol is oxidized to acetic acid. 
B)  Acetic acid is reduced to ethanol. 
C)  Oxygen is reduced. 
D)  Hydrogen is oxidized. 
E)  Ethanol is oxidized to acetaldehyde. 
A)  Ethanol is oxidized to acetic acid. 
B)  Acetic acid is reduced to ethanol. 
C)  Oxygen is reduced. 
D)  Hydrogen is oxidized. 
E)  Ethanol is oxidized to acetaldehyde.

Question 9

What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? Al(s) ∣ Al3+(aq) ∣∣ Fe2+(aq) ∣ Fe(s)

Accepted Answer

A)  2Al(s) + 3 Fe2+(aq) → 2Al3+(aq) + 3 Fe(s) 
B)  3Al(s) + 2 Fe2+(aq) → 3Al3+(aq) + 2 Fe(s) 
C)  2 Fe(s) + 3Al3+(aq) → 2 Fe2+(aq) + 3Al(s) 
D)  3 Fe(s) + 2Al3+(aq) → 3 Fe2+(aq) + 2Al(s) 
A)  2Al(s) + 3 Fe2+(aq) → 2Al3+(aq) + 3 Fe(s) 
B)  3Al(s) + 2 Fe2+(aq) → 3Al3+(aq) + 2 Fe(s) 
C)  2 Fe(s) + 3Al3+(aq) → 2 Fe2+(aq) + 3Al(s) 
D)  3 Fe(s) + 2Al3+(aq) → 3 Fe2+(aq) + 2Al(s)

Question 10

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [   ] = 0.000612 M and [   ] = 1.29 M Mg(s) +   (aq) →   (aq) + Fe(s)
E°(Mg2+/Mg) = -2.37 V and E°(Fe3+/Fe) = -0.036 V

Accepted Answer

A)  -3.42 V 
B)  +3.42 V 
C)  -4.32 V 
D)  +2.43 V 
E)  +3.24 V 
A)  -3.42 V 
B)  +3.42 V 
C)  -4.32 V 
D)  +2.43 V 
E)  +3.24 V

Question 11

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 °C: 3I2(s) + 2Fe(s) → 2Fe3+(aq) + 6I⁻(aq)
E°(I2/I-) = + 0.54 V and E°(Fe3+/Fe) = -0.036 V

Accepted Answer

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

Question 12

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

Question 13

Which of the following is the weakest reducing agent?

Accepted Answer

A)  Cl2(g) 
B)  Au+3 (aq) 
C)  F2(g) 
D)  O2(g) 
E)  Fe(s) 
A)  Cl2(g) 
B)  Au+3 (aq) 
C)  F2(g) 
D)  O2(g) 
E)  Fe(s)

Question 14

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)  Al(s) 
B)  Zn2+(aq) 
C)  Mg(s) 
D)  Al3+(aq) 
E)  Mg2+(aq) 
A)  Al(s) 
B)  Zn2+(aq) 
C)  Mg(s) 
D)  Al3+(aq) 
E)  Mg2+(aq)

Question 15

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.) 3Cl2(g) + 2Fe(s) → 6Cl⁻(aq) + 2Fe3+(aq)
Cl2(g) + 2 e⁻ → 2Cl⁻(aq) E° = +1.36 V
Fe3+(aq) + 3 e⁻ → Fe(s) E° = -0.04 V

Accepted Answer

A)  +4.16 V 
B)  -1.40 V 
C)  -1.32 V 
D)  +1.32 V 
E)  +1.40 V 
A)  +4.16 V 
B)  -1.40 V 
C)  -1.32 V 
D)  +1.32 V 
E)  +1.40 V

Question 16

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

Accepted Answer

A)  10.9 g 
B)  16.4 g 
C)  32.8 g 
D)  36.3 g 
A)  10.9 g 
B)  16.4 g 
C)  32.8 g 
D)  36.3 g

Question 17

Identify the components of a fuel cell.

Accepted Answer

A)  nickel-metal hydride 
B)  lithium-ion 
C)  hydrogen-oxygen 
D)  nickel-cadmium 
E)  zinc-manganese 
A)  nickel-metal hydride 
B)  lithium-ion 
C)  hydrogen-oxygen 
D)  nickel-cadmium 
E)  zinc-manganese

Question 18

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO3)2(aq) → Pb(NO3)2(aq) + Cu(s)

Accepted Answer

A)  Pb(s) ∣ Pb2+(aq) ∣∣ Cu2+(aq) ∣ Cu(s) 
B)  Cu(s) ∣ Cu2+(aq) ∣∣ Pb2+(aq) ∣ Pb(s) 
C)  Pb(s) ∣ NO3-(aq) ∣∣ NO3-(aq) ∣ Cu(s) 
D)  Cu(s) ∣ Cu(NO3)2(aq) ∣∣ Pb(NO3)2(aq) ∣ Pb(s) 
A)  Pb(s) ∣ Pb2+(aq) ∣∣ Cu2+(aq) ∣ Cu(s) 
B)  Cu(s) ∣ Cu2+(aq) ∣∣ Pb2+(aq) ∣ Pb(s) 
C)  Pb(s) ∣ NO3-(aq) ∣∣ NO3-(aq) ∣ Cu(s) 
D)  Cu(s) ∣ Cu(NO3)2(aq) ∣∣ Pb(NO3)2(aq) ∣ Pb(s)

Question 19

How much chromium, in g, can be plated from a solution of   if 2.72 A is applied for 15 minutes?

Accepted Answer

A)  1.32 g 
B)  6.51 ×   g 
C)  0.937 g 
D)  0.440 g 
E)  4.67 g 
A)  1.32 g 
B)  6.51 ×   g 
C)  0.937 g 
D)  0.440 g 
E)  4.67 g

Question 20

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.) 2K(s) + I2(s) → 2K⁺(aq) + 2I⁻(aq)
K+(aq) + e⁻ → K (s) E° = -2.93 V
I2(s) + 2 e⁻ → 2 I⁻(aq) E° = +0.54 V

Accepted Answer

A)  +6.40 V 
B)  +1.85 V 
C)  -5.32 V 
D)  +3.47 V 
E)  +5.32 V 
A)  +6.40 V 
B)  +1.85 V 
C)  -5.32 V 
D)  +3.47 V 
E)  +5.32 V

Exam 18: Electrochemistry

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

Which of the following is the weakest oxidizing agent?

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu2+, Ag+, Sn4+, Fe3+, Au3+

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn2+(aq, 1.8 mol L-1) Ag+(aq, 0.055 mol L-1) ∣ Ag(s) E°(Sn2+/Sn) = -0.14 V and E°(Ag+/Ag) = +0.80 V

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 mol L-1) ∣∣ Al3+(0.100 mol L-1) ∣ Al(s)

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

Which of the following is the weakest oxidizing agent?

What is the reaction at the anode in a breathalyzer?

What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? Al(s) ∣ Al3+(aq) ∣∣ Fe2+(aq) ∣ Fe(s)

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.000612 M and [ ] = 1.29 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg2+/Mg) = -2.37 V and E°(Fe3+/Fe) = -0.036 V

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 °C: 3I2(s) + 2Fe(s) → 2Fe3+(aq) + 6I⁻(aq) E°(I2/I-) = + 0.54 V and E°(Fe3+/Fe) = -0.036 V

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

Which of the following is the weakest reducing agent?

Which of the following is the strongest oxidizing agent?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

Identify the components of a fuel cell.

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO3)2(aq) → Pb(NO3)2(aq) + Cu(s)

How much chromium, in g, can be plated from a solution of if 2.72 A is applied for 15 minutes?

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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)

Predict the species that will be reduced first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu²⁺, Ag⁺, Sn⁴⁺, Fe³⁺, Au³⁺

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s) ∣ Sn²⁺(aq, 1.8 mol L^-1) Ag⁺(aq, 0.055 mol L^-1) ∣ Ag(s) E°(Sn²⁺/Sn) = -0.14 V and E°(Ag⁺/Ag) = +0.80 V

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 mol L^-1) ∣∣ Al³⁺(0.100 mol L^-1) ∣ Al(s)

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

What is the balanced chemical equation for the galvanic cell reaction expressed using shorthand notation below? Al(s) ∣ Al³⁺(aq) ∣∣ Fe²⁺(aq) ∣ Fe(s)

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.000612 M and [ ] = 1.29 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25 °C: 3I₂(s) + 2Fe(s) → 2Fe³⁺(aq) + 6I⁻(aq) E°(I₂/I^-) = + 0.54 V and E°(Fe³⁺/Fe) = -0.036 V

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO₃)₂(aq) → Pb(NO₃)₂(aq) + Cu(s)