Question 1

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

Accepted Answer

A)   Co is the reducing agent.
B)   Co2+ ions are oxidized.
C)   Al is the reducing agent.
D)   Al3+ is the reducing agent.
E)   aluminum metal is the cathode.F) A) and B)
G) C) and E)

Question 2

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Accepted Answer

A)   16.2 g
B)   33.4 g
C)   40.6 g
D)   81.3 g
E)   163 gF) A) and E)
G) D) and E)

Question 3

Examine the following half-reactions and select the strongest oxidizing agent among the substances. 4]2-(aq)  B)  RuO4(s)  C)  HFeO4- (aq)  D)  H4XeO6(aq)  E)  Cl-(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   [PtCl4]2-(aq) 
B)   RuO4(s) 
C)   HFeO4- (aq) 
D)   H4XeO6(aq) 
E)   Cl-(aq) F) B) and C)
G) C) and D)

Question 4

A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction occurs at one of the electrodes.
Mg2+ + 2e- F1F1F1S1F1F1F10 Mg
a. Calculate the charge, in coulombs, which passes through the circuit in this time.
b. Calculate the theoretical mass of Mg (magnesium metal) which is produced in this time.

Accepted Answer

a. 3.60 × ...

Question 5

Consider the reaction of iodine with manganese dioxide -7. Calculate E°cell for the reaction at 25°C. A)  -0.36 V B)  -0.18 V C)  -0.12 V D)  -0.060 V 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 E°cell for the reaction at 25°C.

Accepted Answer

A)   -0.36 V
B)   -0.18 V
C)   -0.12 V
D)   -0.060 V
E)   none of the aboveF) A) and E)
G) B) and D)

Question 6

A voltaic cell prepared using zinc and iodine has the following cell notation. 
Zn(s)  | Zn2+(aq)  || I-(aq)  | I2(s)  | C(graphite) 
Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Accepted Answer

A)   2I-(aq)  + Zn2+(aq)   I2(s)  + Zn(s) 
B)   I2(s)  + Zn(s)   2I-(aq)  + Zn2+(aq) 
C)   2I-(aq)  + Zn(s)   I2(s)  + Zn2+(aq) 
D)   I2(s)  + Zn2+(aq)   2I-(aq)  + Zn(s) 
E)   None of the above, since graphite must be in the equation.F) All of the above
G) C) and D)

Question 7

Manganese dioxide (MnO2) for use in dry cells is made by electrolyzing solutions of Mn2+, where the following reaction occurs at the anode:
Mn2+(aq) + 2H2O(l) F1F1F1S1F1F1F10 MnO2(s) + 4H+(aq) + 2e-
Using a current of 100. amperes (A), how many hours will it take to produce 5.00 kg of MnO2, according to the above reaction?

Accepted Answer

Question 8

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. 
Cu(s)  | Cu2+(aq)  || Ag+(aq)  | Ag(s) 
Which of the following processes occurs at the cathode?

Accepted Answer

A)   Cu(s)   Cu2+(aq)  + 2e-
B)   Cu2+(aq)  + 2e-  Cu(s) 
C)   Ag(s)   Ag+(aq)  + e-
D)   Ag+(aq)  + e-  Ag(s) 
E)   Cu(s)  + 2Ag+(aq)   Cu2+(aq)  + 2Ag(s) F) B) and E)
G) A) and D)

Question 9

What is the E°cell for the cell represented by the combination of the following half-reactions? ClO4-(aq)  + 8H+(aq)  + 8e- cell for the cell represented by the combination of the following half-reactions? ClO4-(aq)  + 8H+(aq)  + 8e-   Cl-(aq)  + 4H2O(l)  E° = 1.389 V VO2+(aq)  + 2H+(aq)  + e-   VO+(aq)  + H2O(l)  E° = 0.991 V A)  -0.398 V B)  -2.380 V C)  0.398 V D)  2.380 V E)  none of the above" class="answers-bank-image d-inline" rel="preload" > Cl-(aq)  + 4H2O(l)  E° = 1.389 V
VO2+(aq)  + 2H+(aq)  + e- cell for the cell represented by the combination of the following half-reactions? ClO4-(aq)  + 8H+(aq)  + 8e-   Cl-(aq)  + 4H2O(l)  E° = 1.389 V VO2+(aq)  + 2H+(aq)  + e-   VO+(aq)  + H2O(l)  E° = 0.991 V A)  -0.398 V B)  -2.380 V C)  0.398 V D)  2.380 V E)  none of the above" class="answers-bank-image d-inline" rel="preload" > VO+(aq)  + H2O(l)  E° = 0.991 V

Accepted Answer

A)   -0.398 V
B)   -2.380 V
C)   0.398 V
D)   2.380 V
E)   none of the aboveF) A) and E)
G) A) and D)

Question 10

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

Question 11

Calculate the potential of a voltaic cell (E°cell)  if it is required to do 5.43 × 10-3 kJ of work when a charge of 2.50 C is transferred.

Accepted Answer

A)   2.17 × 103 V
B)   2.17 × 10-3 V
C)   2.17 V
D)   13.6 V
E)   1.36 × 10-2 VF) D) and E)
G) C) and D)

Question 12

Calculate E°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: 4Al(s)  + 3O2(g)  + 12H+(aq)   4Al3+(aq)  + 6H2O(l)  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 the above values of E°cell is correct." class="answers-bank-image d-inline" rel="preload" >
 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)   Spontaneous, but none of the above values of E°cell is correct.F) B) and E)
G) C) and D)

Question 13

A galvanic cell is constructed using the two hypothetical half-reactions  a. Write down the balanced equation representing the cell reaction.
b. Calculate the standard potential of this cell, E°cell.
c. Calculate F1F1F1S1F1F1F10G° for the cell reaction.

Accepted Answer

a. 2A + D <font face="symbol">F...

Question 14

A voltaic cell consists of a Ag/Ag+ electrode (E° = 0.80 V)  and a Fe2+/Fe3+ electrode (E° = 0.77 V)  with the following initial molar concentrations: [Fe2+] = 0.30 M;
[Fe3+] = 0.10 M; [Ag+] = 0.30 M. What is the equilibrium concentration of Fe3+? (Assume the anode and cathode solutions are of equal volume, and a temperature of 25°C.)

Accepted Answer

A)   0.030 M
B)   0.043 M
C)   0.085 M
D)   0.11 M
E)   0.17 MF) A) and E)
G) A) and D)

Question 15

A voltaic cell consists of a Hg/Hg22+ electrode (E°  = 0.85 V)  and a Sn/Sn2+ electrode (E°  = -0.14 V) . Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C.

Accepted Answer

A)   0.0001 M
B)   0.0007 M
C)   0.005 M
D)   0.03 M
E)   0.05 MF) A) and E)
G) A) and B)

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 
E)   Q = KF) C) and E)
G) D) and E)

Question 17

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.30 V Sn2+(aq)  + Fe(s)  cell = 0.30 V Sn2+(aq)  + Fe(s)    Sn(s)  + Fe2+(aq)  A)  1.2 × 105 B)  1.4 × 1010 C)  8.6 × 10-6 D)  7.1 × 10-11 E)  2.3 × 1023" class="answers-bank-image d-inline" rel="preload" > Sn(s)  + Fe2+(aq)

Accepted Answer

A)   1.2 × 105
B)   1.4 × 1010
C)   8.6 × 10-6
D)   7.1 × 10-11
E)   2.3 × 1023F) B) and E)
G) None of the above

Question 18

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) All of the above

Question 19

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 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

Correct Answer
verified

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq)  4Al³⁺(aq) + 6H₂O(l)

Correct Answer
verified

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

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

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

Correct Answer
verified

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E° = 0.85 V) and a Sn/Sn²⁺ electrode (E° = -0.14 V) . Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

Correct Answer
verified

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²⁺(aq) || I^-(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Correct Answer
verified

A galvanic cell is constructed using the two hypothetical half-reactions a. Write down the balanced equation representing the cell reaction. b. Calculate the standard potential of this cell, E°_cell. c. Calculate G° for the cell reaction.

Correct Answer
verified
a. 2A + D F...
View Answer

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

Correct Answer
verified

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified
a. 3.60 × ...
View Answer

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄^-(aq) + 8H⁺(aq) + 8e^- Cl^-(aq) + 4H₂O(l) E°= 1.389 V VO₂⁺(aq) + 2H⁺(aq) + e^- VO⁺(aq) + H₂O(l) E°= 0.991 V

Correct Answer
verified

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

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

Correct Answer
verified

Electrons are produced at the cathode of a voltaic cell.

Correct Answer
verified

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Correct AnswerverifiedShow Answer

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 4Al(s) + 3O2(g) + 12H+(aq)  4Al3+(aq) + 6H2O(l)

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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 AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

A voltaic cell consists of a Hg/Hg22+ electrode (E° = 0.85 V) and a Sn/Sn2+ electrode (E° = -0.14 V) . Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C.

Correct AnswerverifiedShow Answer

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn2+(aq) || I-(aq) | I2(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Correct AnswerverifiedShow Answer

A galvanic cell is constructed using the two hypothetical half-reactions a. Write down the balanced equation representing the cell reaction. b. Calculate the standard potential of this cell, E°cell. c. Calculate G° for the cell reaction.

Correct Answerverifieda. 2A + D F...View AnswerShow Answer

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

Correct AnswerverifiedShow Answer

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct Answerverifieda. 3.60 × ...View AnswerShow Answer

Calculate the potential of a voltaic cell (E°cell) if it is required to do 5.43 × 10-3 kJ of work when a charge of 2.50 C is transferred.

Correct AnswerverifiedShow Answer

What is the E°cell for the cell represented by the combination of the following half-reactions? ClO4-(aq) + 8H+(aq) + 8e- Cl-(aq) + 4H2O(l) E° = 1.389 V VO2+(aq) + 2H+(aq) + e- VO+(aq) + H2O(l) E° = 0.991 V

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq)

Correct AnswerverifiedShow Answer

Electrons are produced at the cathode of a voltaic cell.

Correct AnswerverifiedShow Answer

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode?

Correct AnswerverifiedShow Answer

Correct Answer
verified

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq)  4Al³⁺(aq) + 6H₂O(l)

Correct Answer
verified

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

Correct Answer
verified

A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E° = 0.85 V) and a Sn/Sn²⁺ electrode (E° = -0.14 V) . Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

Correct Answer
verified

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²⁺(aq) || I^-(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Correct Answer
verified

A galvanic cell is constructed using the two hypothetical half-reactions a. Write down the balanced equation representing the cell reaction. b. Calculate the standard potential of this cell, E°_cell. c. Calculate G° for the cell reaction.

Correct Answer
verified
a. 2A + D F...
View Answer

Correct Answer
verified

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
a. 3.60 × ...
View Answer

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄^-(aq) + 8H⁺(aq) + 8e^- Cl^-(aq) + 4H₂O(l) E°= 1.389 V VO₂⁺(aq) + 2H⁺(aq) + e^- VO⁺(aq) + H₂O(l) E°= 0.991 V

Correct Answer
verified

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

Correct Answer
verified

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

Correct Answer
verified

Correct Answer
verified

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

Correct Answer
verified