Question 1

A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V)  and a Fe/Fe2+ electrode (E° = -0.44 V) . If Ecell = 0 and the temperature is 25°C, what is the ratio [Fe2+]/[Cd2+]?

Accepted Answer

A)   2 × 101
B)   1 × 101
C)   1
D)   1 × 10-1
E)   5 × 10-2F) C) and D)
G) B) and E)

Question 2

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. 
2+(aq)  B)  Fe(s)  C)  Fe2+(aq)  D)  Sr2+(aq)  E)  Co2+(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Cr2+(aq) 
B)   Fe(s) 
C)   Fe2+(aq) 
D)   Sr2+(aq) 
E)   Co2+(aq) F) A) and B)
G) C) and D)

Question 3

Consider the reaction CuO(s)  + H2(g)   Cu(s)  + H2O(l) 
In this reaction, which substances are the oxidant and reductant, respectively?

Accepted Answer

A)   CuO and H2
B)   H2 and CuO
C)   CuO and Cu
D)   H2O and H2
E)   none of the aboveF) B) and C)
G) All of the above

Question 4

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 the aboveF) A) and B)
G) B) and C)

Question 5

What is the E°cell for the cell represented by the combination of the following half-reactions? cell for the cell represented by the combination of the following half-reactions?   A)  -0.18 V B)  0.18 V C)  1.28 V D)  1.66 V E)  2.12 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -0.18 V
B)   0.18 V
C)   1.28 V
D)   1.66 V
E)   2.12 VF) C) and E)
G) All of the above

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

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V)  and a Cu/Cu2+ electrode (E° = 0.34 V) . Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

Accepted Answer

A)   0.001 M
B)   0.002 M
C)   0.01 M
D)   0.02 M
E)   0.04 MF) D) and E)
G) None of the above

Question 8

Consider the following balanced redox reaction 
Mn2+(aq)  + S2O82-(aq)  + 2H2O(l)   MnO2(s)  + 4H+(aq)  + 2SO42-(aq) 
Which of the following statements is true?

Accepted Answer

A)   Mn2+(aq)  is the oxidizing agent and is reduced.
B)   Mn2+(aq)  is the oxidizing agent and is oxidized.
C)   Mn2+(aq)  is the reducing agent and is oxidized.
D)   Mn2+(aq)  is the reducing agent and is reduced.
E)   Manganese does not change its oxidation number in this reaction.F) C) and D)
G) B) and D)

Question 9

Consider the reaction of iodine with manganese dioxide 
-7. Calculate G° for the reaction at 25°C. A)  -15.1 kJ B)  -34.7 kJ C)  15.1 kJ D)  34.7 kJ E)  none of the above" class="answers-bank-image d-inline" rel="preload" >
The equilibrium constant for the overall reaction is 8.30 × 10-7. Calculate G° 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 the aboveF) All of the above
G) A) and B)

Question 10

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. 
4-(aq)  B)  Mn2+(aq)  C)  K+(aq)  D)  F2O(aq)  E)  H+(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   AuBr4-(aq) 
B)   Mn2+(aq) 
C)   K+(aq) 
D)   F2O(aq) 
E)   H+(aq) F) A) and B)
G) D) and E)

Question 11

A cell can be prepared from copper and tin. What is the E°cell for the cell that forms from the following half-reactions? 
Cu2+(aq)  + 2e- cell for the cell that forms from the following half-reactions?  Cu2+(aq)  + 2e-   Cu(s)  E° = 0.34 V Sn4+(aq)  + 2e-    Sn2+(aq)  E° = 0.13 V A)  0.47 V B)  0.21 V C)  -0.21 V D)  -0.47 V E)  0.42 V" class="answers-bank-image d-inline" rel="preload" > Cu(s)  E° = 0.34 V
Sn4+(aq)  + 2e-  cell for the cell that forms from the following half-reactions?  Cu2+(aq)  + 2e-   Cu(s)  E° = 0.34 V Sn4+(aq)  + 2e-    Sn2+(aq)  E° = 0.13 V A)  0.47 V B)  0.21 V C)  -0.21 V D)  -0.47 V E)  0.42 V" class="answers-bank-image d-inline" rel="preload" > Sn2+(aq)  E° = 0.13 V

Accepted Answer

A)   0.47 V
B)   0.21 V
C)   -0.21 V
D)   -0.47 V
E)   0.42 VF) B) and C)
G) A) and E)

Question 12

In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Accepted Answer

A) True 
 B)False

Question 13

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E°cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? 
S2O82-(aq)  + 2H+ + 2I-(aq)   2HSO4-(aq)  + I2(aq)

Accepted Answer

A)   -1.051 V
B)   -2.123 V
C)   1.051 V
D)   2.123 V
E)   none of the aboveF) B) and E)
G) A) and B)

Question 14

Which one of the following statements relating to the glass electrode is correct?

Accepted Answer

A)   The glass electrode detects hydrogen gas.
B)   The glass of a glass electrode serves to conduct electrons.
C)   When pH is measured, only a single electrode, the glass electrode, need be used.
D)   The potential of the glass electrode varies linearly with the pH of the solution.
E)   None of the above statements is correct.F) None of the above
G) A) and B)

Question 15

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 the aboveF) All of the above
G) D) and E)

Question 16

If the electrodes of a voltaic cell are connected with an external wire, electrons will flow in this wire from the cathode to the anode.

Accepted Answer

A) True 
 B)False

Question 17

Consider the following balanced redox reaction 
3CuO(s)  + 2NH3(aq)   N2(g)  + 3H2O(l)  + 3Cu(s) 
Which of the following statements is true?

Accepted Answer

A)   CuO(s)  is the oxidizing agent and copper is reduced.
B)   CuO(s)  is the oxidizing agent and copper is oxidized.
C)   CuO(s)  is the reducing agent and copper is oxidized.
D)   CuO(s)  is the reducing agent and copper is reduced.
E)   CuO(s)  is the oxidizing agent and N2(g)  is the reducing agent.F) All of the above
G) B) and C)

Question 18

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

Accepted Answer

A)   -921 kJ
B)   -767 kJ
C)   -460 kJ
D)   -307 kJ
E)   none of the aboveF) All of the above
G) B) and D)

Question 19

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Accepted Answer

A)   zinc
B)   graphite
C)   copper
D)   iron
E)   sodiumF) C) and E)
G) B) and C)

Question 20

In the shorthand notation for cells, a single vertical line represents a salt bridge.

Accepted Answer

A) True 
 B)False

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

Correct Answer
verified

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V) . Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

Correct Answer
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If the electrodes of a voltaic cell are connected with an external wire, electrons will flow in this wire from the cathode to the anode.

Correct Answer
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Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈^2-(aq) + 2H₂O(l)  MnO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) Which of the following statements is true?

Correct Answer
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Consider the reaction CuO(s) + H₂(g)  Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Correct Answer
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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) ₆^2-(aq) + Bi(s) (basic solution)

Correct Answer
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Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Correct Answer
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Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Correct Answer
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Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

Correct Answer
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Which one of the following statements relating to the glass electrode is correct?

Correct Answer
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A cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e^- Cu(s) E°= 0.34 V Sn⁴⁺(aq) + 2e^- Sn²⁺(aq) E°= 0.13 V

Correct Answer
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Consider the reaction of iodine with manganese dioxide The equilibrium constant for the overall reaction is 8.30 × 10^-7. Calculate G°for the reaction at 25°C.

Correct Answer
verified

The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l)  2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V. Calculate G°for the reaction.

Correct Answer
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In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Correct Answer
verified

In the shorthand notation for cells, a single vertical line represents a salt bridge.

Correct Answer
verified

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq)  N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
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A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V) and a Fe/Fe²⁺ electrode (E°= -0.44 V) . If E_cell = 0 and the temperature is 25°C, what is the ratio [Fe²⁺]/[Cd²⁺]?

Correct Answer
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What is the E°_cell for the cell represented by the combination of the following half-reactions?

Correct Answer
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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 Answer
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Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

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A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V) . Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

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If the electrodes of a voltaic cell are connected with an external wire, electrons will flow in this wire from the cathode to the anode.

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Consider the following balanced redox reaction Mn2+(aq) + S2O82-(aq) + 2H2O(l)  MnO2(s) + 4H+(aq) + 2SO42-(aq) Which of the following statements is true?

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Consider the reaction CuO(s) + H2(g)  Cu(s) + H2O(l) In this reaction, which substances are the oxidant and reductant, respectively?

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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)

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Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

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Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

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Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

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Which one of the following statements relating to the glass electrode is correct?

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A cell can be prepared from copper and tin. What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq) + 2e- Cu(s) E° = 0.34 V Sn4+(aq) + 2e- Sn2+(aq) E° = 0.13 V

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Consider the reaction of iodine with manganese dioxide The equilibrium constant for the overall reaction is 8.30 × 10-7. Calculate G° for the reaction at 25°C.

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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 G° for the reaction.

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In the shorthand notation for cells, a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Correct AnswerverifiedShow Answer

In the shorthand notation for cells, a single vertical line represents a salt bridge.

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Consider the following balanced redox reaction 3CuO(s) + 2NH3(aq)  N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true?

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A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V) and a Fe/Fe2+ electrode (E° = -0.44 V) . If Ecell = 0 and the temperature is 25°C, what is the ratio [Fe2+]/[Cd2+]?

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What is the E°cell for the cell represented by the combination of the following half-reactions?

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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?

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Correct Answer
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Correct Answer
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A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V) . Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

Correct Answer
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Correct Answer
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Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈^2-(aq) + 2H₂O(l)  MnO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) Which of the following statements is true?

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Consider the reaction CuO(s) + H₂(g)  Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Correct Answer
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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) ₆^2-(aq) + Bi(s) (basic solution)

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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A cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e^- Cu(s) E°= 0.34 V Sn⁴⁺(aq) + 2e^- Sn²⁺(aq) E°= 0.13 V

Correct Answer
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Consider the reaction of iodine with manganese dioxide The equilibrium constant for the overall reaction is 8.30 × 10^-7. Calculate G°for the reaction at 25°C.

Correct Answer
verified

The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l)  2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V. Calculate G°for the reaction.

Correct Answer
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Correct Answer
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Correct Answer
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Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq)  N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
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A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V) and a Fe/Fe²⁺ electrode (E°= -0.44 V) . If E_cell = 0 and the temperature is 25°C, what is the ratio [Fe²⁺]/[Cd²⁺]?

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions?

Correct Answer
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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 Answer
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