Question 1

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu2+(aq)  + 2e− → Cu(s)  and Ag+(aq)  + e− → Ag(s) 
For every 1.00 g of copper produced in the first process, how many grams of silver will be produced in the second one?

Accepted Answer

A)  0.294 g
B)  0.588 g
C)  0.850 g
D)  1.70 g
E)  3.40 gF) C) and E)
G) A) and C)

Question 2

In a fuel cell, an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

Accepted Answer

A) True 
 B)False

Question 3

Which component of the following cell notation is the anode? P | Q || R | S

Accepted Answer

A)  P
B)  Q
C)  R
D)  S
E)  One of the | symbols is the anode.F) A) and B)
G) A) and C)

Question 4

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

Accepted Answer

A)  Fuel cell
B)  Nickel-metal hydride cell
C)  Dry cell
D)  Alkaline battery
E)  Lithium-ion batteryF) B) and E)
G) B) and D)

Question 5

The value of E°cell for the reaction 2Cr3+(aq)  + 6Hg(l)  → 2Cr(s)  + 3Hg22+(aq) 
Is 1.59 V. Calculate ΔG° for the reaction.

Accepted Answer

A)  −921 kJ
B)  −767 kJ
C)  −460 kJ
D)  −307 kJ
E)  None of these choices are correct.F) D) and E)
G) A) and B)

Question 6

A buried iron pipe can be protected against corrosion by connecting it to a rod of magnesium.

Accepted Answer

A) True 
 B)False

Question 7

Consider the nonaqueous cell reaction 2Na(l)  + FeCl2(s)  ⇄ 2NaCl(s)  + Fe(s) 
For which E°cell = 2.35 V at 200°C. ΔG° at this temperature is

Accepted Answer

A)  453 kJ.
B)  −453 kJ.
C)  907 kJ.
D)  −907 kJ.
E)  None of these choices are correct.F) A) and B)
G) B) and E)

Question 8

The line notation, Al(s)  | Al3+(aq)  || Co2+(aq)  | Co(s) , indicates that

Accepted Answer

A)  Co is the reducing agent.
B)  Co 2+ ions are oxidized.
C)  Al is the reducing agent.
D)  Al 3+ is the reducing agent.
E)  aluminum metal is the cathode.F) A) and C)
G) A) and B)

Question 9

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn2+(aq)  + 2H2O(l)  → MnO2(s)  + 4H+(aq)  + 2e−
What mass of MnO2 is deposited at this anode?

Accepted Answer

A)  19.5 kg
B)  12.9 kg
C)  4.87 kg
D)  2.43 kg
E)  None of these choices are correct.F) A) and C)
G) A) and E)

Question 10

Electrons are produced at the cathode of a voltaic cell.

Accepted Answer

A) True 
 B)False

Question 11

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O2(g)  + 4H+(aq)  + 4e− ⇄ 2H2O(l)  E° = 1.229 V
Al3+(aq)  + 3e− ⇄ Al(s)  E° = −1.662 V
Overall reaction:
4Al(s)  + 3O2(g)  + 12H+(aq)  → 4Al3+(aq)  + 6H2O(l)

Accepted Answer

A)  E° cell = −2.891 V, nonspontaneous
B)  E° cell = −2.891 V, spontaneous
C)  E° cell = 2.891 V, nonspontaneous
D)  E° cell = 2.891 V, spontaneous
E)  None of these choices are correct.F) B) and D)
G) A) and C)

Question 12

The lead-acid battery is an example of a secondary battery.

Accepted Answer

A) True 
 B)False

Question 13

How many grams of oxygen gas will be produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H2O(l)  → 2H2(g)  + O2(g)

Accepted Answer

A)  31.7 g
B)  15.9 g
C)  7.94 g
D)  3.97 g
E)  1.98 gF) B) and E)
G) A) and B)

Question 14

A battery is considered "dead" when

Accepted Answer

A)  Q 
B)  Q = 1.
C)  Q> 1.
D)  Q = K.
E)  Q/K = 0.F) D) and E)
G) A) and C)

Question 15

Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH) 3(s)  + 3e− ⇄ Cr(s)  + 3OH−(aq)  E° = −1.48 V
SnO2(s)  + 2H2O(l)  + 4e− ⇄ Sn(s)  + 4OH−(aq)  E° = −0.945 V
MnO2(s)  + 4H+(aq)  + 2e− ⇄ Mn2+(aq)  + 2H2O(l)  E° = 1.224 V
Hg2SO4(s)  + 2e− ⇄ 2Hg(l)  + SO42−(aq)  E° = 0.613 V

Accepted Answer

A)  Cr( s) 
B)  Sn( s) 
C)  Mn 2+( aq) 
D)  Hg( l) 
E)  OH −( aq) F) A) and D)
G) C) and E)

Question 16

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3− will be Bi(OH) 3(s)  + Sn(OH) 3(aq)  → Sn(OH) 62−(aq)  + Bi(s)  (basic solution)

Accepted Answer

A)  1.
B)  2.
C)  3.
D)  6.
E)  None of these choices are correct.F) A) and B)
G) B) and D)

Question 17

Calculate E°cell for the reaction of nickel(II)  ions with cadmium metal at 25°C. K = 1.17 × 105Ni2+(aq)  + Cd(s)  → Cd2+(aq)  + Ni(s)

Accepted Answer

A)  0.075 V
B)  0.10 V
C)  0.12 V
D)  0.15 V
E)  0.30 VF) C) and E)
G) D) and E)

Question 18

The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu2+(aq)  + Co(s)  → Cu(s)  + Co2+(aq)

Accepted Answer

A)  −0.28 V
B)  −0.96 V
C)  0.28 V
D)  0.96 V
E)  None of these choices are correct.F) B) and D)
G) A) and B)

Question 19

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s)  + 2e− ⇄ Pb(s)  + 2I−(aq)  E° = −0.365 V
Ca2+(aq)  + 2e− ⇄ Ca(s)  E° = −2.868 V
Pt2+(aq)  + 2e− ⇄ Pt(s)  E° = 1.18 V
Br2(l)  + 2e− ⇄ 2Br−(aq)  E° = 1.066 V

Accepted Answer

A)  Pb( s) 
B)  Ca( s) 
C)  Pt( s) 
D)  Br −( aq) 
E)  Pt 2+( aq) F) D) and E)
G) A) and E)

Question 20

Consider the reaction of iodine with manganese dioxide 3I2(s)  + 2MnO2(s)  + 8OH−(aq) ⇄ 6I−(aq)  + 2MnO4(aq)  + 4H2O(l) 
The equilibrium constant for the overall reaction is 8.30 × 10−7. Calculate ΔG° for the reaction at 25°C.

Accepted Answer

A)  −15.1 kJ
B)  −34.7 kJ
C)  15.1 kJ
D)  34.7 kJ
E)  None of these choices are correct.F) C) and D)
G) B) and D)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

The lead-acid battery is an example of a secondary battery.

Correct Answer
verified

Which component of the following cell notation is the anode? P | Q || R | S

Correct Answer
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The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l) → 2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V. Calculate ΔG° for the reaction.

Correct Answer
verified

In a fuel cell, an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

Correct Answer
verified

Correct Answer
verified

Consider the reaction of iodine with manganese dioxide 3I₂(s) + 2MnO₂(s) + 8OH⁻(aq) ⇄ 6I⁻(aq) + 2MnO₄(aq) + 4H₂O(l) The equilibrium constant for the overall reaction is 8.30 × 10⁻⁷. Calculate ΔG° for the reaction at 25°C.

Correct Answer
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Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O₂(g) + 4H⁺(aq) + 4e⁻⇄ 2H₂O(l) E° = 1.229 V Al³⁺(aq) + 3e⁻ ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq) → 4Al³⁺(aq) + 6H₂O(l)

Correct Answer
verified

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s) + 2e⁻ ⇄ Pb(s) + 2I⁻(aq) E° = −0.365 V Ca²⁺(aq) + 2e⁻ ⇄ Ca(s) E° = −2.868 V Pt²⁺(aq) + 2e⁻ ⇄ Pt(s) E° = 1.18 V Br₂(l) + 2e⁻ ⇄ 2Br⁻(aq) E° = 1.066 V

Correct Answer
verified

Correct Answer
verified

Electrons are produced at the cathode of a voltaic cell.

Correct Answer
verified

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s) , indicates that

Correct Answer
verified

The voltaic cell made up of cobalt, copper, and their M²⁺ ions, has E°_cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

Correct Answer
verified

A battery is considered "dead" when

Correct Answer
verified

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) ₃⁻will be Bi(OH) ₃(s) + Sn(OH) ₃(aq) → Sn(OH) ₆²⁻(aq) + Bi(s) (basic solution)

Correct Answer
verified

A buried iron pipe can be protected against corrosion by connecting it to a rod of magnesium.

Correct Answer
verified

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) → MnO₂(s) + 4H⁺(aq) + 2e⁻ What mass of MnO₂ is deposited at this anode?

Correct Answer
verified

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Correct Answer
verified

How many grams of oxygen gas will be produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H₂O(l) → 2H₂(g) + O₂(g)

Correct Answer
verified

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 10⁵Ni²⁺(aq) + Cd(s) → Cd²⁺(aq) + Ni(s)

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

The lead-acid battery is an example of a secondary battery.

Correct AnswerverifiedShow Answer

Which component of the following cell notation is the anode? P | Q || R | S

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The value of E°cell for the reaction 2Cr3+(aq) + 6Hg(l) → 2Cr(s) + 3Hg22+(aq) Is 1.59 V. Calculate ΔG° for the reaction.

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In a fuel cell, an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH−(aq) ⇄ 6I−(aq) + 2MnO4(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 × 10−7. Calculate ΔG° for the reaction at 25°C.

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Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O2(g) + 4H+(aq) + 4e− ⇄ 2H2O(l) E° = 1.229 V Al3+(aq) + 3e− ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O2(g) + 12H+(aq) → 4Al3+(aq) + 6H2O(l)

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Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s) + 2e− ⇄ Pb(s) + 2I−(aq) E° = −0.365 V Ca2+(aq) + 2e− ⇄ Ca(s) E° = −2.868 V Pt2+(aq) + 2e− ⇄ Pt(s) E° = 1.18 V Br2(l) + 2e− ⇄ 2Br−(aq) E° = 1.066 V

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Electrons are produced at the cathode of a voltaic cell.

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The line notation, Al(s) | Al3+(aq) || Co2+(aq) | Co(s) , indicates that

Correct AnswerverifiedShow Answer

The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu2+(aq) + Co(s) → Cu(s) + Co2+(aq)

Correct AnswerverifiedShow Answer

A battery is considered "dead" when

Correct AnswerverifiedShow Answer

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3− will be Bi(OH) 3(s) + Sn(OH) 3(aq) → Sn(OH) 62−(aq) + Bi(s) (basic solution)

Correct AnswerverifiedShow Answer

A buried iron pipe can be protected against corrosion by connecting it to a rod of magnesium.

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A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn2+(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2e− What mass of MnO2 is deposited at this anode?

Correct AnswerverifiedShow Answer

Consider the nonaqueous cell reaction 2Na(l) + FeCl2(s) ⇄ 2NaCl(s) + Fe(s) For which E°cell = 2.35 V at 200°C. ΔG° at this temperature is

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How many grams of oxygen gas will be produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H2O(l) → 2H2(g) + O2(g)

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Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 105Ni2+(aq) + Cd(s) → Cd2+(aq) + Ni(s)

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Correct Answer
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Correct Answer
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The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l) → 2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V. Calculate ΔG° for the reaction.

Correct Answer
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Correct Answer
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Correct Answer
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Consider the reaction of iodine with manganese dioxide 3I₂(s) + 2MnO₂(s) + 8OH⁻(aq) ⇄ 6I⁻(aq) + 2MnO₄(aq) + 4H₂O(l) The equilibrium constant for the overall reaction is 8.30 × 10⁻⁷. Calculate ΔG° for the reaction at 25°C.

Correct Answer
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Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O₂(g) + 4H⁺(aq) + 4e⁻⇄ 2H₂O(l) E° = 1.229 V Al³⁺(aq) + 3e⁻ ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq) → 4Al³⁺(aq) + 6H₂O(l)

Correct Answer
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Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s) + 2e⁻ ⇄ Pb(s) + 2I⁻(aq) E° = −0.365 V Ca²⁺(aq) + 2e⁻ ⇄ Ca(s) E° = −2.868 V Pt²⁺(aq) + 2e⁻ ⇄ Pt(s) E° = 1.18 V Br₂(l) + 2e⁻ ⇄ 2Br⁻(aq) E° = 1.066 V

Correct Answer
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Correct Answer
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Correct Answer
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The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s) , indicates that

Correct Answer
verified

The voltaic cell made up of cobalt, copper, and their M²⁺ ions, has E°_cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) ₃⁻will be Bi(OH) ₃(s) + Sn(OH) ₃(aq) → Sn(OH) ₆²⁻(aq) + Bi(s) (basic solution)

Correct Answer
verified

Correct Answer
verified

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) → MnO₂(s) + 4H⁺(aq) + 2e⁻ What mass of MnO₂ is deposited at this anode?

Correct Answer
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Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Correct Answer
verified

How many grams of oxygen gas will be produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H₂O(l) → 2H₂(g) + O₂(g)

Correct Answer
verified

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 10⁵Ni²⁺(aq) + Cd(s) → Cd²⁺(aq) + Ni(s)

Correct Answer
verified