Question 1

Given the following two half-reactions,write the overall balanced reaction in the direction in which it is spontaneous and calculate the standard cell potential. 
 Ga3+(aq) +3e−→Ga(s) Ered∘=−0.53 VSn4+(aq) +2e−→Sn⁡2+(aq) Eox∘=+0.15 V\begin{array}{ll}\mathrm{Ga}^{3+}(a q) +3 e^{-} ightarrow \mathrm{Ga}(s)  & E_{\mathrm{red}}^{\circ}=-0.53 \mathrm{~V} \\mathrm{Sn}^{4+}(a q) +2 e^{-} ightarrow \operatorname{Sn}^{2+}(a q)  & E_{o x}^{\circ}=+0.15 \mathrm{~V} \\end{array}Ga3+(aq) +3e−→Ga(s) Sn4+(aq) +2e−→Sn2+(aq) ​Ered∘​=−0.53 VEox∘​=+0.15 V​

Accepted Answer

A)   2Ga3+(aq) + 3Sn2+(aq) ? 2Ga(s) + 3Sn4+(aq) E° = +0.68 V
B)   3Ga3+(aq) + 2Sn2+(aq) ? 3Ga(s) + 2Sn4+(aq) E° = -1.89 V
C)   2Ga(s) + 3Sn4+(aq) ? 2Ga3+(aq) + 3Sn2+(aq) E° = +0.68 V
D)   3Ga(s) + 2Sn4+(aq) ? 3Ga3+(aq) + 2Sn2+(aq) E° = +0.38 V
E)   2Ga(s) + 3Sn4+(aq) ? 2Ga3+(aq) + 3Sn2+(aq) E° = +1.89 V F) A) and B)
G) None of the above

Question 2

Using the reduction half-reactions,write an overall reaction in the direction that is spontaneous.Calculate E°. 
 AgI(s) +e−→Ag(s) +I−(aq) Ered0=−0.152 VCo3+(aq) +e−→Co2+(aq) Ered∘=+1.953 V\begin{array}{ll}\mathrm{AgI}(s) +e^{-} ightarrow \mathrm{Ag}(s) +\mathrm{I}-(a q)  & E_{\mathrm{red}}^{0}=-0.152 \mathrm{~V} \\mathrm{Co}^{3+}(a q) +e^{-} ightarrow \mathrm{Co}^{2+}(a q)  & E_{\mathrm{red}}^{\circ}=+1.953 \mathrm{~V}\end{array}AgI(s) +e−→Ag(s) +I−(aq) Co3+(aq) +e−→Co2+(aq) ​Ered0​=−0.152 VEred∘​=+1.953 V​

Accepted Answer

A)   Co2+(aq) + AgI(s) ? Co3+(aq) + Ag(s) + I?(aq) E° = ?2.105 V
B)   Co2+(aq) + Ag(s) + I?(aq) ? Co3+(aq) + AgI(s) E° = ?1.801 V
C)   Co3+(aq) + Ag(s) + I?(aq) ? Co2+(aq) + AgI(s) E° = +1.801 V
D)   Co3+(aq) + Ag(s) + I?(aq) ? Co2+(aq) + AgI(s) E° = +2.105 V
E)   Co3+(aq) + AgI(s) ? Co2+(aq) + Ag(s) + I?(aq) E° = ?2.105 V F) A) and C)
G) B) and C)

Question 3

For the lead storage battery,the products of the discharge reaction are

Accepted Answer

A)   Pb at the anode,H2O at the cathode.
B)   H2SO4 at the anode,H2O at the cathode.
C)   PbSO4 at both the anode and cathode.
D)   Pb at the cathode and PbO2 at the anode.
E)   Pb at both the anode and cathode.F) B) and D)
G) A) and E)

Question 4

Write a balanced chemical equation for the overall reaction represented below. Pt | Fe2+,Fe3+ || Cl− | AgCl | Ag

Accepted Answer

A)   AgCl(s) + Fe3+(aq) + 2e− → Ag(s) + Fe2+(aq) + Cl−(aq) 
B)   AgCl(s) + Fe3+(aq) → Ag(s) + Fe2+(aq) + Cl−(aq) 
C)   AgCl(s) + Fe2+(aq) → Ag(s) + Fe3+(aq) + Cl−(aq) 
D)   Ag(s) + Fe3+(aq) + Cl−(aq) → AgCl(s) + Fe2+(aq) 
E)   Ag(s) + Fe2+(aq) + Cl−(aq) → AgCl(s) + Fe3+(aq) F) A) and D)
G) B) and E)

Question 5

Calculate E° for an electrochemical cell based on the following overall reaction: 2H+(aq) + Cd(s) ? H2(g) + Cd2+(aq) 
If  Ered o{E}_{	ext {red }}^{o}Ered o​  (H+) = 0.000 V and  Ered o{E}_{	ext {red }}^{o}Ered o​  (Cd2+) = ?0.402 V.

Accepted Answer

A)   ?0.402 V
B)   ?0.201 V
C)   0.000 V
D)   +0.201 V
E)   +0.402 V F) A) and B)
G) C) and E)

Question 6

Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag | AgI | I- || Fe2+,Fe3+ | Pt

Accepted Answer

A)   Fe3+(aq) + Ag(s) + I-(aq) → Fe2+(aq) + AgI(s) 
B)   Fe2+(aq) + Ag(s) + I-(aq) → Fe3+(aq) + AgI(s) 
C)   Fe3+(aq) + AgI(s) → Fe2+(aq) + Ag(s) + I-(aq) 
D)   Fe2+(aq) + AgI(s) → Fe3+(aq) + Ag(s) + I-(aq) 
E)   Fe3+(aq) + 2I-(aq) → Fe2+(aq) + I2(s) F) C) and D)
G) A) and B)

Question 7

The following reaction occurs spontaneously. 2 Fe(s) + 3 Cl2(aq) → 2 Fe3+(aq) + 6 Cl-(aq) 
Write the balanced reduction half-reaction.

Accepted Answer

A)   Fe(s) → Fe3+(aq) + e-
B)   Fe(s) + 3 e- → Fe3+(aq) 
C)   Fe(s) + 3/2 Cl2(aq) → FeCl3(aq) 
D)   Cl2(aq) → 2 Cl-(aq) + 2 e-
E)   Cl2(aq) + 2 e- → 2 Cl-(aq) F) A) and C)
G) A) and D)

Question 8

Which species is the best reducing agent?

Accepted Answer

A)   Sodium ion
B)   Sulfide ion
C)   Chlorine
D)   Sodium metal
E)   Silver metalF) A) and E)
G) None of the above

Question 9

What is the correct cell notation for the reaction below? 
Cd2+(aq) + Ni(s) → Cd(s) + Ni2+(aq)

Accepted Answer

A)   Cd2+ | Cd || Ni | Ni2+
B)   Cd | Cd2+ || Ni2+ | Ni
C)   Ni | Ni2+ || Cd2+ | Cd
D)   Ni | Cd2+ || Ni2+ | Cd
E)   Cd2+ | Cd || Ni | Ni2+..F) B) and C)
G) A) and C)

Question 10

Calculate E for the following electrochemical cell at 25°C, Pt | H2(g) (1.0 atm) | H+ (0.010 M) || Ag+ (0.020 M) | Ag
If E° (H+) = +0.000 V and E° (Ag+) = 0.799 V.

Accepted Answer

A)   +0.275 V
B)   +0.799 V
C)   +0.817 V
D)   +0.911 V
E)   +1.01 VF) A) and B)
G) C) and D)

Question 11

A voltaic cell is based upon the following overall reaction: 2Ag+(aq) + Sn(s) → 2Ag(s) + Sn2+(aq)  Where E° = +0.940 V.Calculate the equilibrium constant at 25°C? (R = 8.31 J/K⋅mol,F = 96480 C/mol e−)

Accepted Answer

A)   6.1 × 1012
B)   8.0 × 1015
C)   1.6 × 1023
D)   6.5 × 1031
E)   9.1 × 1043F) A) and C)
G) D) and E)

Question 12

Use the standard reduction potentials below to determine which element or ion is the best reducing agent.  NO3−(aq) +4H+(aq) +3e−→NO(g) +2H2O(t) E∘=+0.955 VPd2+(aq) +2e−→Pd(s) E∘=+0.90 V2H+(aq) +2e−→H2(g) E∘=0.00 V\begin{array}{ll}\mathrm{NO}_{3}^{-}(a q) +4 \mathrm{H}^{+}(a q) +3 e^{-} ightarrow \mathrm{NO}(g) +2 \mathrm{H}_{2} \mathrm{O}(t)  & E^{\circ}=+0.955 \mathrm{~V} \\mathrm{Pd}^{2+}(a q) +2 \mathrm{e}^{-} ightarrow \mathrm{Pd}(s)  & E^{\circ}=+0.90 \mathrm{~V} \2 \mathrm{H}^{+}(a q) +2 \mathrm{e}^{-} ightarrow \mathrm{H}_{2}(g)  & E^{\circ}=0.00 \mathrm{~V}\end{array}NO3−​(aq) +4H+(aq) +3e−→NO(g) +2H2​O(t) Pd2+(aq) +2e−→Pd(s) 2H+(aq) +2e−→H2​(g) ​E∘=+0.955 VE∘=+0.90 VE∘=0.00 V​

Accepted Answer

A)   Pd2+(aq) 
B)   Pd(s) 
C)   H+(aq) 
D)   H2(g) 
E)   NO3-(aq)  F) B) and E)
G) None of the above

Question 13

Given the following half-reactions, Pb(s) + 2I−(aq) → PbI2(s) + 2e−
I2(aq) + 2e− → 2I−(aq)  Write the balanced overall reaction.

Accepted Answer

A)   Pb(s) + I2(aq) + 2e− → PbI (s) + I−(aq) 
B)   Pb(s) + I2(aq) → PbI2(s) 
C)   Pb(s) + Cl2(aq) → Pb2+(aq) + 2I−(aq) 
D)   2Pb(s) + 4e− → 2PbI(s) + I2(aq) 
E)   Pb(s) + e− + 2I−(aq) → PbI2(aq) F) C) and E)
G) B) and D)

Question 14

Given the following standard reduction potentials,  Pb2+(aq) +2e−→Pb(s) E∘=−0.126 VPbSO4(s) +2e−→Pb(s) +SO42−(aq) E∘=−0.355 V\begin{array}{ll}\mathrm{Pb}^{2+}(a q) +2 e^{-} ightarrow \mathrm{Pb}(s)  & E^{\circ}=-0.126 \mathrm{~V} \\mathrm{PbSO}_{4}(s) +2 e^{-} ightarrow \mathrm{Pb}(\mathrm{s}) +\mathrm{SO}_{4}^{2-}(a q)  & E^{\circ}=-0.355 \mathrm{~V}\end{array}Pb2+(aq) +2e−→Pb(s) PbSO4​(s) +2e−→Pb(s) +SO42−​(aq) ​E∘=−0.126 VE∘=−0.355 V​ 
Determine Ksp for PbSO4(s) at 25°C.(R = 8.31 J/K?mol,F = 96480 C/mol e?)

Accepted Answer

A)   3.4 × 10-28
B)   1.8 × 10-8
C)   5.6 × 10-5
D)   5.6 × 107
E)   2.9 × 1037 F) D) and E)
G) None of the above

Question 15

In an electrochemical cell,if E > E° then

Accepted Answer

A)   Q > 1.
B)   Q 
C)   n = 1.
D)   F > 9.648 × 104.
E)   the system has reached equilibrium.F) A) and E)
G) All of the above

Question 16

The standard reduction potentials for F2(g) and Br2(l) are +2.889 V and 1.077 V,respectively.Write the chemical equation and calculate E° for a voltaic cell based on fluorine and bromine.

Accepted Answer

A)   F2(g) + 2Br−(aq) → 2F−(aq) + Br2(g) E° = +1.812 V
B)   F2(g) + Br2(g) → 2F−(aq) + 2Br−(aq) E° = −1.812 V
C)   F2(g) + Br2(g) → 2F−(aq) + 2Br−(aq) E° = +1.812 V
D)   2F−(aq) + 2Br−(aq) → F2(g) + Br2(g) E° = +1.812 V
E)   Br2(g) + 2F−(aq) → 2Br−(aq) + F2(g) E° = −1.812 VF) A) and E)
G) B) and C)

Question 17

What is the pH of the solution at the cathode if E = -0.362 V for the following electrochemical cell at 25°C? 
Pt | H2(1.0 atm) | H+(1.00 M) || H+(aq) | H2(1.0 atm) | Pt

Accepted Answer

A)   1.77
B)   3.06
C)   6.11
D)   7.89
E)   12.23F) D) and E)
G) B) and C)

Question 18

Calculate E for the following electrochemical cell at 25°C 
Pt | Fe3+(0.100 M) ,Fe2+(0.040 M) || Cl-(0.50 M) | AgCl | Ag
Given the following standard reduction potentials.
 AgCl(s) +e−→Ag2+) +Cl−(aq) E∘=+0.222 VFe3+(aq) +e−→Fe2+(aq) E∘=+0.771 V\begin{array}{ll}\left.\mathrm{AgCl}(s) +e^{-} ightarrow \mathrm{Ag}^{2+}ight) +\mathrm{Cl}^{-}(a q)  & E^{\circ}=+0.222 \mathrm{~V} \\mathrm{Fe}^{3+}(a q) +e^{-} ightarrow \mathrm{Fe}^{2+}(a q)  & E^{\circ}=+0.771 \mathrm{~V}\end{array}AgCl(s) +e−→Ag2+) +Cl−(aq) Fe3+(aq) +e−→Fe2+(aq) ​E∘=+0.222 VE∘=+0.771 V​

Accepted Answer

A)   -1.034 V
B)   -0.590 V
C)   -0.508 V
D)   -0.555 V
E)   +1.034 V F) A) and E)
G) C) and E)

Question 19

What is the relationship between E° and the equilibrium constant,K?

Accepted Answer

A)    E∘=RTnFln⁡KE^{\circ}=\frac{R T}{n F} \ln KE∘=nFRT​lnK 
B)    E∘=nFRTln⁡KE^{\circ}=\frac{n F}{R T} \ln KE∘=RTnF​lnK 
C)   E° = RT ln K
D)   E° = ?RT ln K
E)    E∘=nFRTlog⁡KE^{\circ}=\frac{n F}{R T} \log KE∘=RTnF​logKF) None of the above
G) C) and D)

Question 20

Which of the following species are likely to behave as oxidizing agents: Li(s) ,H2(g) ,MnO4-(aq) ,and Cl-(aq) ?

Accepted Answer

A)   Li(s) only
B)   MnO4-(aq) only
C)   H2(g) and Cl-(aq) 
D)   Li(s) and MnO4-(aq) 
E)   Cl-(aq) onlyF) A) and E)
G) A) and B)

Exam 17: Electrochemistry

What is the correct cell notation for the reaction below? Cd²⁺(aq) + Ni(s) → Cd(s) + Ni²⁺(aq)

Correct Answer
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What is the pH of the solution at the cathode if E = -0.362 V for the following electrochemical cell at 25°C? Pt | H₂(1.0 atm) | H⁺(1.00 M) || H⁺(aq) | H₂(1.0 atm) | Pt

Correct Answer
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A voltaic cell is based upon the following overall reaction: 2Ag⁺(aq) + Sn(s) → 2Ag(s) + Sn²⁺(aq) Where E° = +0.940 V.Calculate the equilibrium constant at 25°C? (R = 8.31 J/K⋅mol,F = 96480 C/mol e−)

Correct Answer
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Correct Answer
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Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag | AgI | I^- || Fe²⁺,Fe³⁺ | Pt

Correct Answer
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The following reaction occurs spontaneously. 2 Fe(s) + 3 Cl₂(aq) → 2 Fe³⁺(aq) + 6 Cl^-(aq) Write the balanced reduction half-reaction.

Correct Answer
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Correct Answer
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For the lead storage battery,the products of the discharge reaction are

Correct Answer
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Calculate E for the following electrochemical cell at 25°C, Pt | H₂(g) (1.0 atm) | H⁺ (0.010 M) || Ag⁺ (0.020 M) | Ag If E° (H⁺) = +0.000 V and E° (Ag⁺) = 0.799 V.

Correct Answer
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Correct Answer
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The standard reduction potentials for F₂(g) and Br₂(l) are +2.889 V and 1.077 V,respectively.Write the chemical equation and calculate E° for a voltaic cell based on fluorine and bromine.

Correct Answer
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What is the relationship between E° and the equilibrium constant,K?

Correct Answer
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Write a balanced chemical equation for the overall reaction represented below. Pt | Fe²⁺,Fe³⁺ || Cl− | AgCl | Ag

Correct Answer
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Correct Answer
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Given the following half-reactions, Pb(s) + 2I−(aq) → PbI₂(s) + 2e− I₂(aq) + 2e− → 2I−(aq) Write the balanced overall reaction.

Correct Answer
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Correct Answer
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In an electrochemical cell,if E > E° then

Correct Answer
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Calculate E° for an electrochemical cell based on the following overall reaction: 2H⁺(aq) + Cd(s) ? H₂(g) + Cd²⁺(aq) If ${E}_{\text {red }}^{o}$ (H⁺) = 0.000 V and ${E}_{\text {red }}^{o}$ (Cd²⁺) = ?0.402 V.

Correct Answer
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Which species is the best reducing agent?

Correct Answer
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Which of the following species are likely to behave as oxidizing agents: Li(s) ,H₂(g) ,MnO₄^-(aq) ,and Cl^-(aq) ?

Correct Answer
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Exam 17: Electrochemistry

What is the correct cell notation for the reaction below? Cd2+(aq) + Ni(s) → Cd(s) + Ni2+(aq)

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What is the pH of the solution at the cathode if E = -0.362 V for the following electrochemical cell at 25°C? Pt | H2(1.0 atm) | H+(1.00 M) || H+(aq) | H2(1.0 atm) | Pt

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A voltaic cell is based upon the following overall reaction: 2Ag+(aq) + Sn(s) → 2Ag(s) + Sn2+(aq) Where E° = +0.940 V.Calculate the equilibrium constant at 25°C? (R = 8.31 J/K⋅mol,F = 96480 C/mol e−)

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Correct AnswerverifiedShow Answer

Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag | AgI | I- || Fe2+,Fe3+ | Pt

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The following reaction occurs spontaneously. 2 Fe(s) + 3 Cl2(aq) → 2 Fe3+(aq) + 6 Cl-(aq) Write the balanced reduction half-reaction.

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Correct AnswerverifiedShow Answer

For the lead storage battery,the products of the discharge reaction are

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Calculate E for the following electrochemical cell at 25°C, Pt | H2(g) (1.0 atm) | H+ (0.010 M) || Ag+ (0.020 M) | Ag If E° (H+) = +0.000 V and E° (Ag+) = 0.799 V.

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Correct AnswerverifiedShow Answer

The standard reduction potentials for F2(g) and Br2(l) are +2.889 V and 1.077 V,respectively.Write the chemical equation and calculate E° for a voltaic cell based on fluorine and bromine.

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What is the relationship between E° and the equilibrium constant,K?

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Write a balanced chemical equation for the overall reaction represented below. Pt | Fe2+,Fe3+ || Cl− | AgCl | Ag

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Correct AnswerverifiedShow Answer

Given the following half-reactions, Pb(s) + 2I−(aq) → PbI2(s) + 2e− I2(aq) + 2e− → 2I−(aq) Write the balanced overall reaction.

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Correct AnswerverifiedShow Answer

In an electrochemical cell,if E > E° then

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Calculate E° for an electrochemical cell based on the following overall reaction: 2H+(aq) + Cd(s) ? H2(g) + Cd2+(aq) If Ered o{E}_{\text {red }}^{o}Ered o​ (H+) = 0.000 V and Ered o{E}_{\text {red }}^{o}Ered o​ (Cd2+) = ?0.402 V.

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Which species is the best reducing agent?

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Which of the following species are likely to behave as oxidizing agents: Li(s) ,H2(g) ,MnO4-(aq) ,and Cl-(aq) ?

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What is the correct cell notation for the reaction below? Cd²⁺(aq) + Ni(s) → Cd(s) + Ni²⁺(aq)

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What is the pH of the solution at the cathode if E = -0.362 V for the following electrochemical cell at 25°C? Pt | H₂(1.0 atm) | H⁺(1.00 M) || H⁺(aq) | H₂(1.0 atm) | Pt

Correct Answer
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A voltaic cell is based upon the following overall reaction: 2Ag⁺(aq) + Sn(s) → 2Ag(s) + Sn²⁺(aq) Where E° = +0.940 V.Calculate the equilibrium constant at 25°C? (R = 8.31 J/K⋅mol,F = 96480 C/mol e−)

Correct Answer
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Correct Answer
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Write a balanced net ionic equation for the overall reaction represented by the cell notation below. Ag | AgI | I^- || Fe²⁺,Fe³⁺ | Pt

Correct Answer
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The following reaction occurs spontaneously. 2 Fe(s) + 3 Cl₂(aq) → 2 Fe³⁺(aq) + 6 Cl^-(aq) Write the balanced reduction half-reaction.

Correct Answer
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Correct Answer
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Correct Answer
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Calculate E for the following electrochemical cell at 25°C, Pt | H₂(g) (1.0 atm) | H⁺ (0.010 M) || Ag⁺ (0.020 M) | Ag If E° (H⁺) = +0.000 V and E° (Ag⁺) = 0.799 V.

Correct Answer
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Correct Answer
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The standard reduction potentials for F₂(g) and Br₂(l) are +2.889 V and 1.077 V,respectively.Write the chemical equation and calculate E° for a voltaic cell based on fluorine and bromine.

Correct Answer
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Correct Answer
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Write a balanced chemical equation for the overall reaction represented below. Pt | Fe²⁺,Fe³⁺ || Cl− | AgCl | Ag

Correct Answer
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Correct Answer
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Given the following half-reactions, Pb(s) + 2I−(aq) → PbI₂(s) + 2e− I₂(aq) + 2e− → 2I−(aq) Write the balanced overall reaction.

Correct Answer
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Correct Answer
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Correct Answer
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Calculate E° for an electrochemical cell based on the following overall reaction: 2H⁺(aq) + Cd(s) ? H₂(g) + Cd²⁺(aq) If ${E}_{\text {red }}^{o}$ (H⁺) = 0.000 V and ${E}_{\text {red }}^{o}$ (Cd²⁺) = ?0.402 V.

Correct Answer
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Correct Answer
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Which of the following species are likely to behave as oxidizing agents: Li(s) ,H₂(g) ,MnO₄^-(aq) ,and Cl^-(aq) ?

Correct Answer
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