Question 1

Identify the battery that is in most automobiles.

Accepted Answer

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

Question 2

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.) Br2(l) + 2Cl-(aq) → 2Br-(aq) + Cl2 (g)
Br2(l) + 2 e → 2Br-(aq) E°= 1.09 V
2Cl- (aq) → Cl2(g) + 2 e - E°= -1.36 V

Accepted Answer

A)  +0.93 V 
B)  +2.24 V 
C)  +2.45 V 
D)  +5.47 V 
E)  +0.67 V 
A)  +0.93 V 
B)  +2.24 V 
C)  +2.45 V 
D)  +5.47 V 
E)  +0.67 V

Question 3

Describe how water can be made to be a good conductor of electrical current.

Accepted Answer

A)  use pure water 
B)  heat the water 
C)  add salt 
D)  chill the water 
E)  vaporize the water 
A)  use pure water 
B)  heat the water 
C)  add salt 
D)  chill the water 
E)  vaporize the water

Question 4

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s) ∣ Cu2+(aq, 0.0032 mol L-1)   Cu2+(aq, 4.48 mol L-1) ∣ Cu(s)
E°(Cu2+/Cu) = +0.34 V

Accepted Answer

A)  0.00 V 
B)  +0.093 V 
C)  +0.34 V 
D)  +0.186 V 
E)  +0.052 V 
A)  0.00 V 
B)  +0.093 V 
C)  +0.34 V 
D)  +0.186 V 
E)  +0.052 V

Question 5

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C. (The equation is balanced.) Pb(s) + Br2(l) → Pb2+(aq) + 2 Br⁻(aq)
Pb2+(aq) + 2 e⁻ → Pb(s) E° = -0.13 V
Br2(l) + 2 e⁻ → 2 Br⁻(aq) E° = +1.07 V

Accepted Answer

A)  +1.20 V 
B)  +0.94 V 
C)  -0.94 V 
D)  -1.20 V 
E)  -0.60 V 
A)  +1.20 V 
B)  +0.94 V 
C)  -0.94 V 
D)  -1.20 V 
E)  -0.60 V

Question 6

Determine the redox reaction represented by the following cell notation: 
Mg(s) ∣ Mg2+(aq)   Cu2+(aq) ∣ Cu(s)

Accepted Answer

A)  Cu(s) + Mg2+(aq) → Mg(s) + Cu2+(aq) 
B)  Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) 
C)  2Mg(s) + Cu2+(aq) → Cu(s) + 2Mg2+(aq) 
D)  2Cu(s) + Mg2+(aq) → Mg(s) + 2Cu2+(aq) 
E)  3Mg(s) + 2Cu2+(aq) → 2Cu(s) + 3Mg2+(aq) 
A)  Cu(s) + Mg2+(aq) → Mg(s) + Cu2+(aq) 
B)  Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) 
C)  2Mg(s) + Cu2+(aq) → Cu(s) + 2Mg2+(aq) 
D)  2Cu(s) + Mg2+(aq) → Mg(s) + 2Cu2+(aq) 
E)  3Mg(s) + 2Cu2+(aq) → 2Cu(s) + 3Mg2+(aq)

Question 7

Which of the following is the strongest oxidizing agent?

Accepted Answer

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

Question 8

A galvanic cell consists of a Zn2+/ Zn half-cell and a standard hydrogen electrode. If the Zn2+/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn2+/ Zn half-cell?

Accepted Answer

A)  -0.76 V 
B)  -0.38 V 
C)  +0.38 V 
D)  +0.76 V 
A)  -0.76 V 
B)  -0.38 V 
C)  +0.38 V 
D)  +0.76 V

Question 9

Explain the significance of the standard hydrogen electrode (SHE) in the tabulation of standard reduction potentials of other species.

Accepted Answer

The SHE is used to construct an electroc

Question 10

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.) Sn(s) + 2Ag⁺(aq) → Sn2+(aq) + 2Ag(s)
Sn2+(aq) + 2 e⁻ → Sn(s) E° = -0.14 V
Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V

Accepted Answer

A)  +1.74 V 
B)  +0.94 V 
C)  +1.08 V 
D)  -1.08 V 
E)  -1.74 V 
A)  +1.74 V 
B)  +0.94 V 
C)  +1.08 V 
D)  -1.08 V 
E)  -1.74 V

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 
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

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

Accepted Answer

A)  Pb2+(aq) + Cu(s); if E°(Pb2+/Pb) = -0.13V and E°(Cu2+/Cu) = +0.16V 
B)  Ag+(aq) + Br⁻(aq); if E°(Ag+/Ag) = 0.80V and E°(Br2/Br-) = +1.09V 
C)  Li+(aq) + Al(s); if E°(Li+/Li) = -3.04V and E°(Al3+/Al) = -1.66V 
D)  Fe3+(aq) + Ni(s); if E°(Fe3+/Fe) = -0.04V and E°(Ni2+/Ni) = -0.23V 
E)  Cd2+(aq) + I-(aq); if E°(Cd2+/Cd) = -0.40V and E°(I2/I-) = + 0.54V 
A)  Pb2+(aq) + Cu(s); if E°(Pb2+/Pb) = -0.13V and E°(Cu2+/Cu) = +0.16V 
B)  Ag+(aq) + Br⁻(aq); if E°(Ag+/Ag) = 0.80V and E°(Br2/Br-) = +1.09V 
C)  Li+(aq) + Al(s); if E°(Li+/Li) = -3.04V and E°(Al3+/Al) = -1.66V 
D)  Fe3+(aq) + Ni(s); if E°(Fe3+/Fe) = -0.04V and E°(Ni2+/Ni) = -0.23V 
E)  Cd2+(aq) + I-(aq); if E°(Cd2+/Cd) = -0.40V and E°(I2/I-) = + 0.54V

Question 13

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

Accepted Answer

A)  Cd; E°(Cd2+/Cd) = -0.40V 
B)  Cr; E°(Cr3+/Cr) = -0.73V 
C)  Mn; E°(Mn2+/Mn) = -1.18V 
D)  Ag; E°(Ag+/Ag) = +0.80V 
E)  Al; E°(Al3+/Al) = -1.66V 
A)  Cd; E°(Cd2+/Cd) = -0.40V 
B)  Cr; E°(Cr3+/Cr) = -0.73V 
C)  Mn; E°(Mn2+/Mn) = -1.18V 
D)  Ag; E°(Ag+/Ag) = +0.80V 
E)  Al; E°(Al3+/Al) = -1.66V

Question 14

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn2+(aq) ∣∣ Ni2+(aq) ∣ Ni(s)

Accepted Answer

A)  Zn(s) → Zn2+(aq) + 2 e- 
B)  Zn2+(aq) + 2 e- → Zn(s) 
C)  Ni(s) → Ni2+(aq) + 2 e- 
D)  Ni2+(aq) + 2 e- → Ni(s) 
A)  Zn(s) → Zn2+(aq) + 2 e- 
B)  Zn2+(aq) + 2 e- → Zn(s) 
C)  Ni(s) → Ni2+(aq) + 2 e- 
D)  Ni2+(aq) + 2 e- → Ni(s)

Question 15

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb2+(aq)   H+(aq) ∣ H2(g) ∣ Pt(s)

Accepted Answer

A)  H2(g) 
B)  H+(aq) 
C)  Pb2+(aq) 
D)  Pb(s) 
E)  Pt(s) 
A)  H2(g) 
B)  H+(aq) 
C)  Pb2+(aq) 
D)  Pb(s) 
E)  Pt(s)

Question 16

Which of the following is TRUE about standard electrode potentials?

Accepted Answer

A)  E°cell is negative for spontaneous reactions. 
B)  Electrons will flow from a more positive electrode to a more negative electrode. 
C)  The electrode potential of the standard hydrogen electrode is exactly zero. 
D)  E°cell is the sum between standard reduction potentials of the anode and the cathode. 
E)  The electrode in any half-cell with a greater tendency to undergo reduction is negatively charged relative to the standard hydrogen electrode and therefore has E° < 0. 
A)  E°cell is negative for spontaneous reactions. 
B)  Electrons will flow from a more positive electrode to a more negative electrode. 
C)  The electrode potential of the standard hydrogen electrode is exactly zero. 
D)  E°cell is the sum between standard reduction potentials of the anode and the cathode. 
E)  The electrode in any half-cell with a greater tendency to undergo reduction is negatively charged relative to the standard hydrogen electrode and therefore has E° < 0.

Question 17

Use the provided reduction potentials to calculate ΔrG° for the following redox reaction: 2Al(s) + 3Mg2+(aq) → 2Al3+(aq) + 3Mg(s)
E°(Al3+/Al) = -1.66 V and E°(Mg2+/Mg) = -2.37 V

Accepted Answer

A)  +4.1 × 102 kJ mol-1 
B)  +1.4 × 102 kJ mol-1 
C)  -2.3 × 102 kJ mol-1 
D)  -7.8 × 102 kJ mol-1 
E)  +6.8 × 102 kJ mol-1 
A)  +4.1 × 102 kJ mol-1 
B)  +1.4 × 102 kJ mol-1 
C)  -2.3 × 102 kJ mol-1 
D)  -7.8 × 102 kJ mol-1 
E)  +6.8 × 102 kJ mol-1

Question 18

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

Question 19

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

Accepted Answer

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

Question 20

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)  Pt(s) 
A)  Ni(s) 
B)  Ni2+(aq) 
C)  Ag+(aq) 
D)  Ag(s) 
E)  Pt(s)

Exam 18: Electrochemistry

Identify the battery that is in most automobiles.

Describe how water can be made to be a good conductor of electrical current.

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s) ∣ Cu2+(aq, 0.0032 mol L-1) Cu2+(aq, 4.48 mol L-1) ∣ Cu(s) E°(Cu2+/Cu) = +0.34 V

Determine the redox reaction represented by the following cell notation: Mg(s) ∣ Mg2+(aq) Cu2+(aq) ∣ Cu(s)

Which of the following is the strongest oxidizing agent?

A galvanic cell consists of a Zn2+/ Zn half-cell and a standard hydrogen electrode. If the Zn2+/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn2+/ Zn half-cell?

Explain the significance of the standard hydrogen electrode (SHE) in the tabulation of standard reduction potentials of other species.

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

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

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn2+(aq) ∣∣ Ni2+(aq) ∣ Ni(s)

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb2+(aq) H+(aq) ∣ H2(g) ∣ Pt(s)

Which of the following is TRUE about standard electrode potentials?

Use the provided reduction potentials to calculate ΔrG° for the following redox reaction: 2Al(s) + 3Mg2+(aq) → 2Al3+(aq) + 3Mg(s) E°(Al3+/Al) = -1.66 V and E°(Mg2+/Mg) = -2.37 V

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

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

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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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s) ∣ Cu²⁺(aq, 0.0032 mol L^-1) Cu²⁺(aq, 4.48 mol L^-1) ∣ Cu(s) E°(Cu²⁺/Cu) = +0.34 V

Determine the redox reaction represented by the following cell notation: Mg(s) ∣ Mg²⁺(aq) Cu²⁺(aq) ∣ Cu(s)

A galvanic cell consists of a Zn²⁺/ Zn half-cell and a standard hydrogen electrode. If the Zn²⁺/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn²⁺/ Zn half-cell?

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn²⁺(aq) ∣∣ Ni²⁺(aq) ∣ Ni(s)

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb²⁺(aq) H⁺(aq) ∣ H₂(g) ∣ Pt(s)

Use the provided reduction potentials to calculate Δ_rG° for the following redox reaction: 2Al(s) + 3Mg²⁺(aq) → 2Al³⁺(aq) + 3Mg(s) E°(Al³⁺/Al) = -1.66 V and E°(Mg²⁺/Mg) = -2.37 V

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

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