Question 1

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). 
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 2

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 3

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

Accepted Answer

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

Question 4

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

Question 5

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)   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) 
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)

Question 6

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 7

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 
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 8

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 9

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 10

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

Question 11

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 
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 12

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

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

Question 14

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

Question 15

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

Question 16

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)   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) 
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)

Question 17

Match the following.

-Q > K

Accepted Answer

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

Question 18

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 19

Match the following.

-Q = 1

Accepted Answer

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

Question 20

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 
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

Exam 18: Electrochemistry

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,

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

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

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

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

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

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

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

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

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.

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

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

Which of the following is the strongest reducing agent?

Which of the following is the weakest reducing agent?

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

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

Match the following. -Q > K

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

Match the following. -Q = 1

Which of the following metals will dissolve in HCl?

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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,

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

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

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

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

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

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.

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

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

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

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