Question 1

A voltaic cell prepared using aluminum and nickel has the following cell notation.
Al(s)| Al3+(aq)|| Ni2+(aq)| Ni(s)
Which of the following reactions occurs at the anode?

Accepted Answer

A) Al(s) $\to$ Al3+(aq)+ 3e- 
B) Al3+(aq)+ 3e $\to$ Al(s) 
C) Ni(s) $\to$Ni2+(aq)+ 2e- 
D) Ni2+(aq)+ 2e- $\to$ Ni(s) 
E) None of these choices are correct.

Question 2

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

Accepted Answer

A) True 
 B)False

Question 3

A voltaic cell prepared using aluminum and nickel has the following cell notation.
Al(s)| Al3+(aq)|| Ni2+(aq)| Ni(s)
Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

Accepted Answer

A) Ni2+(aq)+ Al(s) $\to$ Al3+(aq)+ Ni(s) 
B) 3Ni2+(aq)+ 2Al(s) $\to$2Al3+(aq)+ 3Ni(s) 
C) Ni(s)+ Al3+(aq) $\to$Ni2+(aq)+ Al(s) 
D) 3Ni(s)+ 2Al3+(aq)  $\to$ 3Ni2+(aq)+ 2Al(s) 
E) None of these choices is correct.

Question 4

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) $\to$ Sn(OH)62-(aq)+ Bi(s)(basic solution)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 6 
E) None of these choices is correct.

Question 5

A current of 250.A flows for 24.0 hours at an anode where the reaction occurring is
Mn2+(aq)+ 2H2O(l) $\to$ 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 is correct.

Question 6

What is the E°cell for the cell represented by the combination of the following half-reactions?
2Hg2+(aq)+ 2e- 
Hg22+(aq);E°= 0.92 V
Cr3+ (aq)+ 3e- 
Cr(s);E°= -0.74 V

Accepted Answer

A) -0.18 V 
B) 0.18 V 
C) 1.28 V 
D) 1.66 V 
E) 2.12 V

Question 7

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for zinc will be _____.
Zn(s)+ ReO4-(aq) $\to$ Re(s)+ Zn2+(aq)(acidic solution)

Accepted Answer

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

Question 8

Which,if any,of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V;all E° values refer to the M2+/M half-cell reactions.

Accepted Answer

A) copper,Cu,E° = 0.15 V 
B) cobalt,Co,E° = -0.28 V 
C) chromium,Cr,E° = -0.74 V 
D) tin,Sn,E° = -0.14 V 
E) None of these metals would be capable of acting as a sacrificial anode with iron.

Question 9

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 10

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the iodide ion will be _____.
I-(aq)+ NO3-(aq) $\to$ NO(g)+ I2(s)(acidic solution)

Accepted Answer

A) 2 
B) 3 
C) 6 
D) 8 
E) None of these choices is correct.

Question 11

A much-studied cell in electrochemistry has the following cell notation: Ag(s)| AgCl(s)| HCl(aq)| H₂(g)| Pt(s) Bearing in mind that HCl(aq)consists of H⁺(aq)and Cl^-(aq),and that this solution is in contact with both electrodes (there is no salt bridge),write down balanced equations for a.the anode half-reaction. b.the cathode half-reaction. c.the cell reaction.

Accepted Answer

The answer of A much-studied cell in electrochemistry has the...

Question 12

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.61 V
2Cr(s)+ 3Pb2+(aq) 
3Pb(s)+ 2Cr3+(aq)

Accepted Answer

A) 4.1 $\times$ 1020 
B) 8.2 $\times$ 1030 
C) 3.3 $\times$ 1051 
D) 7.4 $\times$ 1061 
E) > 9.9 $\times$ 1099

Question 13

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) $\to$ 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) Spontaneous,but none of these values of E°cell is correct.

Question 14

Explain what is meant by a fuel cell.Provide a balanced equation to represent the reaction in any fuel cell of your choice.

Accepted Answer

The answer of Explain what is meant by a fuel...

Question 15

a.Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten KCl.
b.Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of aqueous KCl.
c.Clearly explain why the products of the two processes are not the same.

Accepted Answer

The answer of a.Write a balanced equation to represent the...

Question 16

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

Accepted Answer

A) Ecell = E°cell 
B) E°cell = 0 
C) Q = 1 
D) Q < K 
E) Q =K

Question 17

Consider the following balanced redox reaction
Mn2+(aq)+ S2O82-(aq)+ 2H2O(l) $\to$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.

Question 18

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Accepted Answer

A) 0.419 g 
B) 6.29 g 
C) 12.6 g 
D) 25.2 g 
E) 33.4 g

Question 19

Which one of the following statements about electrochemical cells is correct?

Accepted Answer

A) In a salt bridge,current is carried by cations moving toward the anode,and anions toward the cathode. 
B) In the external wire,electrons travel from cathode to anode. 
C) The anode of a voltaic cell is labeled minus (-). 
D) Oxidation occurs at the cathode,in an electrolytic cell. 
E) None of these statements is correct.

Question 20

Electrons are produced at the cathode of a voltaic cell.

Accepted Answer

A) True 
 B)False

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

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

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

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) $\to$ Sn(OH) ₆^2-(aq) + Bi(s) (basic solution)

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

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e^- Hg₂²⁺(aq) ;E°= 0.92 V Cr³⁺ (aq) + 3e^- Cr(s) ;E°= -0.74 V

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq) $\to$ Re(s) + Zn²⁺(aq) (acidic solution)

Which,if any,of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

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

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq) $\to$ NO(g) + I₂(s) (acidic solution)

Explain what is meant by a fuel cell.Provide a balanced equation to represent the reaction in any fuel cell of your choice.

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

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

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Which one of the following statements about electrochemical cells is correct?

Electrons are produced at the cathode of a voltaic cell.

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following reactions occurs at the anode?

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

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

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) →\to→ Sn(OH) 62-(aq) + Bi(s) (basic solution)

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

What is the E°cell for the cell represented by the combination of the following half-reactions? 2Hg2+(aq) + 2e- Hg22+(aq) ;E°= 0.92 V Cr3+ (aq) + 3e- Cr(s) ;E°= -0.74 V

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for zinc will be _____. Zn(s) + ReO4-(aq) →\to→ Re(s) + Zn2+(aq) (acidic solution)

Which,if any,of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V;all E° values refer to the M2+/M half-cell reactions.

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

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the iodide ion will be _____. I-(aq) + NO3-(aq) →\to→ NO(g) + I2(s) (acidic solution)

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.61 V 2Cr(s) + 3Pb2+(aq) 3Pb(s) + 2Cr3+(aq)

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) →\to→ 4Al3+(aq) + 6H2O(l)

Explain what is meant by a fuel cell.Provide a balanced equation to represent the reaction in any fuel cell of your choice.

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

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

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Which one of the following statements about electrochemical cells is correct?

Electrons are produced at the cathode of a voltaic cell.

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

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) $\to$ Sn(OH) ₆^2-(aq) + Bi(s) (basic solution)

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

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e^- Hg₂²⁺(aq) ;E°= 0.92 V Cr³⁺ (aq) + 3e^- Cr(s) ;E°= -0.74 V

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq) $\to$ Re(s) + Zn²⁺(aq) (acidic solution)

Which,if any,of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq) $\to$ NO(g) + I₂(s) (acidic solution)

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