Question 1

A cell can be prepared from copper and tin. What is the E °\degree° cell for the cell that forms from the following half-reactions? cell for the cell that forms from the following half-reactions?   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" >

Accepted Answer

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

Question 2

A voltaic cell consists of a Mn/Mn2+ electrode (E °\degree° = -1.18 V)  and a Fe/Fe2+ electrode (E °\degree° = -0.44 V) . Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25 °\degree° C.

Accepted Answer

A)   0.040 M
B)   0.24 M
C)   1.1 M
D)   1.8 M
E)   None of these choices is correct. F) A) and C)
G) B) and E)

Question 3

Consider the reaction: CuO(s)  + H2(g)   →\rightarrow→  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 these choices is correct. F) C) and E)
G) B) and E)

Question 4

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Accepted Answer

A) True 
 B)False

Question 5

A voltaic cell prepared using zinc and iodine has the following cell notation. 2+(aq)   \rightarrow  I2(s)  + Zn(s)  B)  I2(s)  + Zn(s)   \rightarrow  2I¯(aq)  + Zn2+(aq)  C)  2I¯(aq)  + Zn(s)   \rightarrow I2(s)  + Zn2+(aq)  D)  I2(s)  + Zn2+(aq)   \rightarrow  2I¯(aq)  + Zn(s)  E)  None of these choices, since graphite must be in the equation. " class="answers-bank-image d-inline" rel="preload" > Which of the following equations correctly represents the balanced, spontaneous cell reaction?

Accepted Answer

A)   2I¯(aq)  + Zn2+(aq)   →\rightarrow→  I2(s)  + Zn(s) 
B)   I2(s)  + Zn(s)   →\rightarrow→  2I¯(aq)  + Zn2+(aq) 
C)   2I¯(aq)  + Zn(s)   →\rightarrow→ I2(s)  + Zn2+(aq) 
D)   I2(s)  + Zn2+(aq)   →\rightarrow→  2I¯(aq)  + Zn(s) 
E)   None of these choices, since graphite must be in the equation. F) A) and E)
G) B) and E)

Question 6

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.   Overall reaction:   A)  E \degree cell = -1.00 V, nonspontaneous B)  E \degree cell = -1.00 V, spontaneous C)  E \degree cell = 1.00 V, nonspontaneous D)  E \degree cell = 1.00 V, spontaneous E)  E \degree cell = -0.23 V, nonspontaneous " class="answers-bank-image d-inline" rel="preload" > Overall reaction: cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.   Overall reaction:   A)  E \degree cell = -1.00 V, nonspontaneous B)  E \degree cell = -1.00 V, spontaneous C)  E \degree cell = 1.00 V, nonspontaneous D)  E \degree cell = 1.00 V, spontaneous E)  E \degree cell = -0.23 V, nonspontaneous " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   E °\degree° cell = -1.00 V, nonspontaneous
B)   E °\degree° cell = -1.00 V, spontaneous
C)   E °\degree° cell = 1.00 V, nonspontaneous
D)   E °\degree° cell = 1.00 V, spontaneous
E)   E °\degree° cell = -0.23 V, nonspontaneous F) A) and B)
G) B) and D)

Question 7

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____.

Accepted Answer

A)   2
B)   7
C)   8
D)   16
E)   None of these choices is correct.F) A) and E)
G) C) and D)

Question 8

For the reaction occurring in a voltaic (galvanic) cell, $\Delta$G > 0.

Accepted Answer

A) True 
 B)False

Question 9

A concentration cell is based on the aqueous reaction  The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Accepted Answer

Question 10

When metal A is placed in a solution of metal ions B2+, a reaction occurs between A and B2+, and metal ions A2+ appear in the solution. When metal B is placed in acid solution, gas bubbles form on its surface. When metal A is placed in a solution of metal ions C2+, no reaction occurs. Which of the following reactions would not occur spontaneously?

Accepted Answer

A)   C(s)  + 2H+(aq)   →\rightarrow→ H2(g)  + C2+(aq) 
B)   C(s)  + A2+(aq)   →\rightarrow→  A(s)  + C2+(aq) 
C)   B(s)  + C2+(aq)   →\rightarrow→  C(s)  + B2+(aq) 
D)   A(s)  + 2H+(aq)   →\rightarrow→  H2(g)  + A2+(aq) 
E)   B(s)  + 2H+(aq)   →\rightarrow→ H2(g)  + B2+(aq)  F) All of the above
G) B) and C)

Question 11

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

A)   The anode will definitely gain weight in a voltaic cell.
B)   Oxidation occurs at the cathode of both cells.
C)   The free energy change,  Δ\DeltaΔ G, is negative for the voltaic cell.
D)   The electrons in the external wire flow from cathode to anode in an electrolytic cell.
E)   None of these choices is correct. F) A) and B)
G) A) and C)

Question 12

A battery is considered "dead" when:

Accepted Answer

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

Question 13

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______.

Accepted Answer

A)   1
B)   3
C)   4
D)   8
E)   None of these choices is correct.F) C) and D)
G) A) and C)

Question 14

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Accepted Answer

A) True 
 B)False

Question 15

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

Accepted Answer

A) True 
 B)False

Question 16

A concentration cell is based on the aqueous reaction  The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Draw a neat diagram to represent this cell, showing and labeling all necessary components including: anode, cathode, electron flow, cation flow and anion flow.

Accepted Answer

Question 17

What product forms at the anode during the electrolysis of molten NaBr?

Accepted Answer

A)   Na+(l) 
B)   Na(l) 
C)   Br¯(l) 
D)   Br3¯(l) 
E)   Br2(g) F) A) and B)
G) All of the above

Question 18

The value of E  °\degree° cell for the reaction cell for the reaction   is 1.59 V. Calculate  \Delta G  \degree  for the reaction. A)  -921 kJ B)  -767 kJ C)  -460 kJ D)  -307 kJ E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > is 1.59 V. Calculate  Δ\DeltaΔ G  °\degree°  for the reaction.

Accepted Answer

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

Question 19

Consider the reaction of iodine with manganese dioxide: 
3I2(s)  + 2MnO2(s)  + 8OH¯(aq)  2(s)  + 2MnO2(s)  + 8OH¯(aq)    6I¯(aq)  + 2MnO4¯(aq)  + 4H2O(l)  The equilibrium constant for the overall reaction is 8.30 *10¯7. Calculate E \degree cell for the reaction at 25 \degree C. A)  -0.36 V B)  -0.18 V C)  -0.12 V D)  -0.060 V E)  None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" > 6I¯(aq)  + 2MnO4¯(aq)  + 4H2O(l) 
The equilibrium constant for the overall reaction is 8.30 *10¯7. Calculate E °\degree° cell for the reaction at 25 °\degree° C.

Accepted Answer

A)   -0.36 V
B)   -0.18 V
C)   -0.12 V
D)   -0.060 V
E)   None of these choices is correct. F) A) and D)
G) B) and D)

Question 20

What product forms at the cathode during the electrolysis of molten lithium iodide?

Accepted Answer

A)   Li+(l) 
B)   Li(l) 
C)   I¯(l) 
D)   I2(g) 
E)   I3¯(l) F) C) and E)
G) A) and B)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

Correct Answer
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Which of the following statements about voltaic and electrolytic cells is correct?

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

Correct Answer
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Correct Answer
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A concentration cell is based on the aqueous reaction The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Correct Answer
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Correct Answer
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A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Correct Answer
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Correct Answer
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What product forms at the cathode during the electrolysis of molten lithium iodide?

Correct Answer
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A voltaic cell consists of a Mn/Mn²⁺ electrode (E $\degree$ = -1.18 V) and a Fe/Fe²⁺ electrode (E $\degree$ = -0.44 V) . Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25 $\degree$ C.

Correct Answer
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Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____.

Correct Answer
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A battery is considered "dead" when:

Correct Answer
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When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______.

Correct Answer
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Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Correct Answer
verified

For the reaction occurring in a voltaic (galvanic) cell, $\Delta$ G > 0.

Correct Answer
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What product forms at the anode during the electrolysis of molten NaBr?

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

The value of E °\degree° cell for the reaction is 1.59 V. Calculate Δ\DeltaΔ G °\degree° for the reaction.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Which of the following statements about voltaic and electrolytic cells is correct?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A voltaic cell prepared using zinc and iodine has the following cell notation. Which of the following equations correctly represents the balanced, spontaneous cell reaction?

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A concentration cell is based on the aqueous reaction The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

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Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

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A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What product forms at the cathode during the electrolysis of molten lithium iodide?

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A voltaic cell consists of a Mn/Mn2+ electrode (E °\degree° = -1.18 V) and a Fe/Fe2+ electrode (E °\degree° = -0.44 V) . Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25 °\degree° C.

Correct AnswerverifiedShow Answer

A cell can be prepared from copper and tin. What is the E °\degree° cell for the cell that forms from the following half-reactions?

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____.

Correct AnswerverifiedShow Answer

A battery is considered "dead" when:

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______.

Correct AnswerverifiedShow Answer

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Correct AnswerverifiedShow Answer

For the reaction occurring in a voltaic (galvanic) cell, Δ\DeltaΔ G > 0.

Correct AnswerverifiedShow Answer

What product forms at the anode during the electrolysis of molten NaBr?

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 E °\degree° cell for the reaction at 25 °\degree° C.

Correct AnswerverifiedShow Answer

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

Correct Answer
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Correct Answer
verified

A concentration cell is based on the aqueous reaction The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

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 voltaic cell consists of a Mn/Mn²⁺ electrode (E $\degree$ = -1.18 V) and a Fe/Fe²⁺ electrode (E $\degree$ = -0.44 V) . Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25 $\degree$ C.

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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Correct Answer
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For the reaction occurring in a voltaic (galvanic) cell, $\Delta$ G > 0.

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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