Question 1

You make a cell with an aluminum electrode in a solution of aluminum nitrate and a zinc electrode in a solution of zinc nitrate.
-If you could increase the concentration of Al3+,which of the following is true about the cell potential?

Accepted Answer

A)  It would increase.
B)  It would decrease.
C)  It would remain constant.
D)  Cannot be determined.
E)  None of these (A-
D)  .F) C) and D)
G) C) and E) B

Question 2

What is the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn2+ concentration is 0.0103 M and the Ag+ concentration is 1.35 M? Zn2+(aq) + 2e-  →	o→  Zn(s) ; ε\varepsilonε ° = -0.76 V
Ag+(aq) + e-  →	o→  Ag(s) ; ε\varepsilonε ° = 0.80 V

Accepted Answer

A)  177
B)  131
C)   2+ concentration is 0.0103 M and the Ag+ concentration is 1.35 M? Zn2+(aq) + 2e-  	o  Zn(s) ; \varepsilon ° = -0.76 V Ag+(aq) + e-  	o  Ag(s) ; \varepsilon ° = 0.80 V 
A)  177 
B)  131 
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >
D)   2+ concentration is 0.0103 M and the Ag+ concentration is 1.35 M? Zn2+(aq) + 2e-  	o  Zn(s) ; \varepsilon ° = -0.76 V Ag+(aq) + e-  	o  Ag(s) ; \varepsilon ° = 0.80 V 
A)  177 
B)  131 
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" >
E)   2+ concentration is 0.0103 M and the Ag+ concentration is 1.35 M? Zn2+(aq) + 2e-  	o  Zn(s) ; \varepsilon ° = -0.76 V Ag+(aq) + e-  	o  Ag(s) ; \varepsilon ° = 0.80 V 
A)  177 
B)  131 
C)     
D)     
E)     " class="answers-bank-image d-inline" rel="preload" > F) All of the above
G) A) and B)

Question 3

A cell is set up with copper and lead electrodes in contact with CuSO4(aq) and Pb(NO3) 2(aq) ,respectively,at 25°C.The standard reduction potentials are: Pb2+ + 2e-  →	o→  Pb
 ε\varepsilonε ° = -0.13 V
Cu2+ + 2e-  →	o→  Cu
 ε\varepsilonε ° = +0.34 V
If sulfuric acid is added to the Pb(NO3) 2 solution,forming a precipitate of PbSO4,the cell potential:

Accepted Answer

A)  increases
B)  decreases
C)  is unchanged
D)  can't tell what will happen
E)  none of these F) A) and C)
G) A) and E)

Question 4

A common car battery consists of six identical cells,each of which carries out the reaction: Pb + PbO2 + 2HSO4- + 2H+  →	o→  2PbSO4 + 2H2O
The value of 2 + 2HSO4- + 2H+  	o  2PbSO4 + 2H2O The value of   for such a cell is 2.039 V.Calculate  \Delta G° at 25 °C for the reaction. A) -196.7 kJ B) -98.37 kJ C) -393.5 kJ D) -786.9 kJ E) -590.2 kJ " class="answers-bank-image d-inline" rel="preload" > for such a cell is 2.039 V.Calculate  Δ\DeltaΔ G° at 25 °C for the reaction.

Accepted Answer

A)  -196.7 kJ
B)  -98.37 kJ
C)  -393.5 kJ
D)  -786.9 kJ
E)  -590.2 kJ F) All of the above
G) B) and E)

Question 5

Which of the following reactions is possible at the anode of a galvanic cell?

Accepted Answer

A)  Zn →	o→  Zn2+ + 2e-
B)  Zn2+ + 2e-  →	o→  Zn
C)  Zn2+ + Cu  →	o→  Zn + Cu2+
D)  Zn + Cu2+  →	o→  Zn2+ + Cu
E)  two of these F) A) and D)
G) A) and C) A

Question 6

Which of the following is the strongest oxidizing agent? MnO4- + 4H+ + 3e-  →	o→  MnO2 + 2H2O
 ε\varepsilonε  ∘\circ∘  = 1.68 V
I2 + 2e-  →	o→  2I-
 ε\varepsilonε  ∘\circ∘  = 0.54 V
Zn2+ + 2e-  →	o→  Zn
 ε\varepsilonε  ∘\circ∘  =-0.76 V

Accepted Answer

A)  MnO4-
B)  I2
C)  Zn2+
D)  Zn
E)  MnO2 F) A) and E)
G) A) and D)

Question 7

Nickel is electroplated from a NiSO4 solution.A constant current of 5.50 amp is applied by an external power supply.How long will it take to deposit 100.g of Ni? The atomic mass of Ni is 58.69.

Accepted Answer

A)  16.6 h
B)  8.30 h
C)  18.2 min
D)  55.4 s
E)  1.09 sF) None of the above
G) D) and E)

Question 8

Which statement is always true of the cathode in an electrochemical cell?

Accepted Answer

A)  It is considered the "negative" electrode.
B)  It is considered the "positive" electrode.
C)  Reduction occurs here.
D)  Metal is plated out here.
E)  Negative ions flow toward the cathode.F) A) and C)
G) A) and E)

Question 9

How many electrons are transferred in the following reaction?

Accepted Answer

A)  0
B)  1
C)  2
D)  4
E)  not enough information givenF) A) and C)
G) All of the above C

Question 10

In order to determine the identity of a particular lanthanide metal Sm,a voltaic cell is constructed at 25°C with the anode consisting of the lanthanide metal as the electrode immersed in a solution of 0.0819 M SmCl3,and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO3) 2 solution.The two half-reactions are as follows: Sm(s)  →	o→  Sm3+(aq) + 3e-
Cu2+(aq) + 2e-  →	o→  Cu(s) 
The potential measured across the cell is 2.67 V.What is the identity of the metal?
3,and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO3) 2 solution.The two half-reactions are as follows: Sm(s)  	o  Sm3+(aq) + 3e- Cu2+(aq) + 2e-  	o  Cu(s)  The potential measured across the cell is 2.67 V.What is the identity of the metal?    A) Ce B) Eu C) Dy D) Sm E) Gd " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  Ce
B)  Eu
C)  Dy
D)  Sm
E)  Gd F) D) and E)
G) A) and E)

Question 11

Which metal,Al or Ni could reduce Zn2+ to Zn(s) if placed in a Zn2+(aq) solution? Zn2+ + 2e-  →	o→  Zn
 ε\varepsilonε  ∘\circ∘  = -0.76 V
Al3+ + 3e-  →	o→  Al
 ε\varepsilonε  ∘\circ∘  = -1.66 V
Ni2+ + 2e-  →	o→  Ni
 ε\varepsilonε  ∘\circ∘  =-0.23 V

Accepted Answer

A)  Al
B)  Ni
C)  Both Al and Ni would work.
D)  Neither Al nor Ni would work.
E)  Cannot be determined. F) B) and E)
G) A) and E)

Question 12

In which direction do electrons flow in the external circuit?

Accepted Answer

A)  left to right
B)  right to left
C)  no current flows;the cell is at equilibrium
D)  cannot be determined.
E)  none of theseF) A) and B)
G) A) and C)

Question 13

The following reaction occurs in aqueous acid solution:
NO3- + I-  →	o→  IO3- + NO2
-In the balanced equation the coefficient of water is:

Accepted Answer

A)  1
B)  2
C)  3
D)  4
E)  5 F) D) and E)
G) A) and B)

Question 14

Balance the following oxidation-reduction reaction using the half-reaction method. Cr2O72- + I2  →	o→  Cr3+ + IO3-
In the balanced equation,the coefficient of water is:

Accepted Answer

A)  4
B)  17
C)  11
D)  7
E)  6 F) A) and D)
G) B) and D)

Question 15

For a certain reaction, Δ\DeltaΔ H° = -74.4 kJ and  Δ\DeltaΔ S° = -227 J/K.If n = 3,calculate  ε\varepsilonε  ∘\circ∘  for the reaction at 25°C.

Accepted Answer

A)  0.0233 V
B)  0.491 V
C)  0.277 V
D)  0.0700 V
E)  0.237 V F) A) and E)
G) A) and B)

Question 16

Consider the galvanic cell shown below (the contents of each half-cell are written beneath each compartment) : 2 0.20 M Cr3+ 0.10 M Br- The standard reduction potentials are as follows: Cr3+(aq) + 3e-  	o  Cr(s)   \varepsilon  \circ  =-0.727 V Br2(aq) + 2e-  	o 2Br-(aq)   \varepsilon  \circ  = +1.090 V What is  \varepsilon  \circ   for this cell? A) 1.817 V B) 0.363 V C) -0.363 V D) 4.724 V E) 1.316 V " class="answers-bank-image d-inline" rel="preload" > 0.50 M Br2 0.20 M Cr3+ 0.10 M Br-
The standard reduction potentials are as follows:
Cr3+(aq) + 3e-  →	o→  Cr(s)   ε\varepsilonε  ∘\circ∘  =-0.727 V
Br2(aq) + 2e-  →	o→ 2Br-(aq)   ε\varepsilonε  ∘\circ∘  = +1.090 V
What is  ε\varepsilonε  ∘\circ∘   for this cell?

Accepted Answer

A)  1.817 V
B)  0.363 V
C)  -0.363 V
D)  4.724 V
E)  1.316 V F) B) and E)
G) B) and D)

Question 17

What is the cell potential at 25°C as read on the digital voltmeter?

Accepted Answer

A)  0.18 V
B)  2.58 V
C)  0.10 V
D)  0.59 V
E)  0.26 VF) All of the above
G) A) and D)

Question 18

What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4) 3 for 145 minutes using a constant current of 11.0 amperes?

Accepted Answer

A)  0.187 g
B)  154.7 g
C)  0.287 g
D)  25.8 g
E)  17.2 gF) None of the above
G) A) and D)

Question 19

Consider a galvanic cell based in the reaction Fe2+ + Cr2O72-  →	o→ Fe3+ + Cr3+ in acidic solution.
-What is the coefficient of Fe3+ in the balanced equation?

Accepted Answer

A)  6
B)  2
C)  3
D)  4
E)  none of these F) B) and D)
G) A) and C)

Question 20

Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.39 M Ni2+. Zn2+ + 2e-  →	o→  Zn
 ε\varepsilonε ° = -0.76 V
Ni2+ + 2e-  →	o→  Ni
 ε\varepsilonε ° = -0.23 V
Calculate  ε\varepsilonε  for this cell.

Accepted Answer

A)  0.54 V
B)  0.52 V
C)  0.51 V
D)  0.53 V
E)  0.98 V F) B) and D)
G) C) and E)

Exam 18: Electrochemistry

You make a cell with an aluminum electrode in a solution of aluminum nitrate and a zinc electrode in a solution of zinc nitrate. -If you could increase the concentration of Al³⁺,which of the following is true about the cell potential?

Correct Answer
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B

Correct Answer
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Correct Answer
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Correct Answer
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Which of the following reactions is possible at the anode of a galvanic cell?

Correct Answer
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A

Which of the following is the strongest oxidizing agent? MnO₄^- + 4H⁺ + 3e^- $\to$ MnO₂ + 2H₂O $\varepsilon$ ^$\circ$ = 1.68 V I₂ + 2e^- $\to$ 2I^- $\varepsilon$ ^$\circ$ = 0.54 V Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ^$\circ$ =-0.76 V

Correct Answer
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Nickel is electroplated from a NiSO₄ solution.A constant current of 5.50 amp is applied by an external power supply.How long will it take to deposit 100.g of Ni? The atomic mass of Ni is 58.69.

Correct Answer
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Which statement is always true of the cathode in an electrochemical cell?

Correct Answer
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How many electrons are transferred in the following reaction?

Correct Answer
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C

Correct Answer
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Which metal,Al or Ni could reduce Zn²⁺ to Zn(s) if placed in a Zn²⁺(aq) solution? Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ^$\circ$ = -0.76 V Al³⁺ + 3e^- $\to$ Al $\varepsilon$ ^$\circ$ = -1.66 V Ni²⁺ + 2e^- $\to$ Ni $\varepsilon$ ^$\circ$ =-0.23 V

Correct Answer
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In which direction do electrons flow in the external circuit?

Correct Answer
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The following reaction occurs in aqueous acid solution: NO₃^- + I^- $\to$ IO₃^- + NO₂ -In the balanced equation the coefficient of water is:

Correct Answer
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Balance the following oxidation-reduction reaction using the half-reaction method. Cr₂O₇²^- + I₂ $\to$ Cr³⁺ + IO₃^- In the balanced equation,the coefficient of water is:

Correct Answer
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For a certain reaction, $\Delta$ H° = -74.4 kJ and $\Delta$ S° = -227 J/K.If n = 3,calculate $\varepsilon$ ^$\circ$ for the reaction at 25°C.

Correct Answer
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Correct Answer
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What is the cell potential at 25°C as read on the digital voltmeter?

Correct Answer
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What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr₂(SO₄) ₃ for 145 minutes using a constant current of 11.0 amperes?

Correct Answer
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Consider a galvanic cell based in the reaction Fe²⁺ + Cr₂O₇²^- $\to$ Fe³⁺ + Cr³⁺ in acidic solution. -What is the coefficient of Fe³⁺ in the balanced equation?

Correct Answer
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Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a nickel electrode immersed in 0.39 M Ni²⁺. Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ° = -0.76 V Ni²⁺ + 2e^- $\to$ Ni $\varepsilon$ ° = -0.23 V Calculate $\varepsilon$ for this cell.

Correct Answer
verified

Exam 18: Electrochemistry

You make a cell with an aluminum electrode in a solution of aluminum nitrate and a zinc electrode in a solution of zinc nitrate. -If you could increase the concentration of Al3+,which of the following is true about the cell potential?

Correct AnswerverifiedB

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A common car battery consists of six identical cells,each of which carries out the reaction: Pb + PbO2 + 2HSO4- + 2H+ →\to→ 2PbSO4 + 2H2O The value of for such a cell is 2.039 V.Calculate Δ\DeltaΔ G° at 25 °C for the reaction.

Correct AnswerverifiedShow Answer

Which of the following reactions is possible at the anode of a galvanic cell?

Correct AnswerverifiedA

Which of the following is the strongest oxidizing agent? MnO4- + 4H+ + 3e- →\to→ MnO2 + 2H2O ε\varepsilonε ∘\circ∘ = 1.68 V I2 + 2e- →\to→ 2I- ε\varepsilonε ∘\circ∘ = 0.54 V Zn2+ + 2e- →\to→ Zn ε\varepsilonε ∘\circ∘ =-0.76 V

Correct AnswerverifiedShow Answer

Nickel is electroplated from a NiSO4 solution.A constant current of 5.50 amp is applied by an external power supply.How long will it take to deposit 100.g of Ni? The atomic mass of Ni is 58.69.

Correct AnswerverifiedShow Answer

Which statement is always true of the cathode in an electrochemical cell?

Correct AnswerverifiedShow Answer

How many electrons are transferred in the following reaction?

Correct AnswerverifiedC

Correct AnswerverifiedShow Answer

Which metal,Al or Ni could reduce Zn2+ to Zn(s) if placed in a Zn2+(aq) solution? Zn2+ + 2e- →\to→ Zn ε\varepsilonε ∘\circ∘ = -0.76 V Al3+ + 3e- →\to→ Al ε\varepsilonε ∘\circ∘ = -1.66 V Ni2+ + 2e- →\to→ Ni ε\varepsilonε ∘\circ∘ =-0.23 V

Correct AnswerverifiedShow Answer

In which direction do electrons flow in the external circuit?

Correct AnswerverifiedShow Answer

The following reaction occurs in aqueous acid solution: NO3- + I- →\to→ IO3- + NO2 -In the balanced equation the coefficient of water is:

Correct AnswerverifiedShow Answer

Balance the following oxidation-reduction reaction using the half-reaction method. Cr2O72- + I2 →\to→ Cr3+ + IO3- In the balanced equation,the coefficient of water is:

Correct AnswerverifiedShow Answer

For a certain reaction, Δ\DeltaΔ H° = -74.4 kJ and Δ\DeltaΔ S° = -227 J/K.If n = 3,calculate ε\varepsilonε ∘\circ∘ for the reaction at 25°C.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the cell potential at 25°C as read on the digital voltmeter?

Correct AnswerverifiedShow Answer

What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr2(SO4) 3 for 145 minutes using a constant current of 11.0 amperes?

Correct AnswerverifiedShow Answer

Consider a galvanic cell based in the reaction Fe2+ + Cr2O72- →\to→ Fe3+ + Cr3+ in acidic solution. -What is the coefficient of Fe3+ in the balanced equation?

Correct AnswerverifiedShow Answer

Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn2+ and a nickel electrode immersed in 0.39 M Ni2+. Zn2+ + 2e- →\to→ Zn ε\varepsilonε ° = -0.76 V Ni2+ + 2e- →\to→ Ni ε\varepsilonε ° = -0.23 V Calculate ε\varepsilonε for this cell.

Correct AnswerverifiedShow Answer

You make a cell with an aluminum electrode in a solution of aluminum nitrate and a zinc electrode in a solution of zinc nitrate. -If you could increase the concentration of Al³⁺,which of the following is true about the cell potential?

Correct Answer
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B

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

Which of the following is the strongest oxidizing agent? MnO₄^- + 4H⁺ + 3e^- $\to$ MnO₂ + 2H₂O $\varepsilon$ ^$\circ$ = 1.68 V I₂ + 2e^- $\to$ 2I^- $\varepsilon$ ^$\circ$ = 0.54 V Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ^$\circ$ =-0.76 V

Correct Answer
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Nickel is electroplated from a NiSO₄ solution.A constant current of 5.50 amp is applied by an external power supply.How long will it take to deposit 100.g of Ni? The atomic mass of Ni is 58.69.

Correct Answer
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Correct Answer
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Correct Answer
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C

Correct Answer
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Which metal,Al or Ni could reduce Zn²⁺ to Zn(s) if placed in a Zn²⁺(aq) solution? Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ^$\circ$ = -0.76 V Al³⁺ + 3e^- $\to$ Al $\varepsilon$ ^$\circ$ = -1.66 V Ni²⁺ + 2e^- $\to$ Ni $\varepsilon$ ^$\circ$ =-0.23 V

Correct Answer
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Correct Answer
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The following reaction occurs in aqueous acid solution: NO₃^- + I^- $\to$ IO₃^- + NO₂ -In the balanced equation the coefficient of water is:

Correct Answer
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Balance the following oxidation-reduction reaction using the half-reaction method. Cr₂O₇²^- + I₂ $\to$ Cr³⁺ + IO₃^- In the balanced equation,the coefficient of water is:

Correct Answer
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For a certain reaction, $\Delta$ H° = -74.4 kJ and $\Delta$ S° = -227 J/K.If n = 3,calculate $\varepsilon$ ^$\circ$ for the reaction at 25°C.

Correct Answer
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Correct Answer
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Correct Answer
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What mass of chromium could be deposited by electrolysis of an aqueous solution of Cr₂(SO₄) ₃ for 145 minutes using a constant current of 11.0 amperes?

Correct Answer
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Consider a galvanic cell based in the reaction Fe²⁺ + Cr₂O₇²^- $\to$ Fe³⁺ + Cr³⁺ in acidic solution. -What is the coefficient of Fe³⁺ in the balanced equation?

Correct Answer
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Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a nickel electrode immersed in 0.39 M Ni²⁺. Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ° = -0.76 V Ni²⁺ + 2e^- $\to$ Ni $\varepsilon$ ° = -0.23 V Calculate $\varepsilon$ for this cell.

Correct Answer
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