Question 1

What is undergoing reduction in the redox reaction represented by the following cell notation?
Mn(s) ∣ Mn2+(aq)  2+(aq)    H+(aq) ∣ H2(g) ∣ Pt A)  H2(g)  B)  H+(aq)  C)  Mn2+(aq)  D)  Mn(s)  E)  Pt" class="answers-bank-image d-inline" rel="preload" > H+(aq) ∣ H2(g) ∣ Pt

Accepted Answer

A)   H2(g) 
B)   H+(aq) 
C)   Mn2+(aq) 
D)   Mn(s) 
E)   PtF) C) and E)
G) A) and B)

Question 2

Which of the following reactions would have the smallest value of K at 298 K?

Accepted Answer

A)   A + B → C; E°cell = +1.22 V
B)   A + 2 B → C; E°cell = +0.98 V
C)   A + B → 2 C; E°cell = -0.030 V
D)   A + B → 3 C; E°cell = +0.15 V
E)   More information is needed to determine.F) A) and C)
G) B) and C)

Question 3

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. 4 F⁻(aq) + Mn2+(aq) → 2F2(g) + Mn(s) 
F2(g) + 2e⁻ → 2 F⁻(aq) E° = +2.87 V
Mn2+(aq) + 2 e⁻ → Mn(s) E° = -1.18 V

Accepted Answer

A)   1.69 V
B)   4.05 V
C)   -4.05 V
D)   +2.87 VE) A) and C)
F) A) and D)

Question 4

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)   MnO2(s) 
B)   Cl⁻(aq) 
C)   Ag⁺(aq) 
D)   SO42-(aq) 
E)   MnO4⁻(aq) F) C) and D)
G) A) and B)

Question 5

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 4.50 V?

Accepted Answer

A)   0.0288
B)   0.0347
C)   8.7
D)   34.7
E)   17.4F) C) and D)
G) A) and B)

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 cellF) C) and D)
G) A) and B)

Question 7

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

Accepted Answer

A)   +4.1 × 102 kJ
B)   +1.4 × 102 kJ
C)   -2.3 × 102 kJ
D)   -7.8 × 102 kJ
E)   +6.8 × 102 kJF) All of the above
G) A) and B)

Question 8

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s) + Pb2+(aq) → Ag+(aq) + Pb(s)

Accepted Answer

A)   179 kJ
B)   89.5 kJ
C)   -328 kJ
D)   -107 kJ
E)   212 kJF) All of the above
G) B) and D)

Exam 20: Electrochemistry

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

Correct Answer
verified

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s) + Pb²⁺(aq) → Ag⁺(aq) + Pb(s)

Correct Answer
verified

Correct Answer
verified

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

Correct Answer
verified

Which of the following reactions would have the smallest value of K at 298 K?

Correct Answer
verified

What is undergoing reduction in the redox reaction represented by the following cell notation? Mn(s) ∣ Mn²⁺(aq) H⁺(aq) ∣ H₂(g) ∣ Pt

Correct Answer
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Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3 Mg(s)

Correct Answer
verified

Which of the following is the strongest oxidizing agent?

Correct Answer
verified

Exam 20: Electrochemistry

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

Correct AnswerverifiedShow Answer

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s) + Pb2+(aq) → Ag+(aq) + Pb(s)

Correct AnswerverifiedShow Answer

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. 4 F⁻(aq) + Mn2+(aq) → 2F2(g) + Mn(s) F2(g) + 2e⁻ → 2 F⁻(aq) E° = +2.87 V Mn2+(aq) + 2 e⁻ → Mn(s) E° = -1.18 V

Correct AnswerverifiedShow Answer

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl2 with an applied emf of 4.50 V?

Correct AnswerverifiedShow Answer

Which of the following reactions would have the smallest value of K at 298 K?

Correct AnswerverifiedShow Answer

What is undergoing reduction in the redox reaction represented by the following cell notation? Mn(s) ∣ Mn2+(aq) H+(aq) ∣ H2(g) ∣ Pt

Correct AnswerverifiedShow Answer

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

Correct AnswerverifiedShow Answer

Which of the following is the strongest oxidizing agent?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Ag(s) + Pb²⁺(aq) → Ag⁺(aq) + Pb(s)

Correct Answer
verified

Correct Answer
verified

How many kilowatt-hours of electricity are used to produce 3.50 kg of magnesium in the electrolysis of molten MgCl₂ with an applied emf of 4.50 V?

Correct Answer
verified

Correct Answer
verified

What is undergoing reduction in the redox reaction represented by the following cell notation? Mn(s) ∣ Mn²⁺(aq) H⁺(aq) ∣ H₂(g) ∣ Pt

Correct Answer
verified

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3 Mg(s)

Correct Answer
verified

Correct Answer
verified