Question 1

What is E°cell for the following reaction,and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq) 
Given:
H2O2(aq) + 2H+(aq) + 2e-
  cell for the following reaction,and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq)  Given: H2O2(aq) + 2H+(aq) + 2e-     2H2O(l) E° = 1.77V Fe3+(aq) + e-   Fe2+(aq) E° = 0.77V A) E°cell = -1.00 V,nonspontaneous B) E°cell = -1.00 V,spontaneous C) E°cell = 1.00 V,nonspontaneous D) E°cell = 1.00 V,spontaneous E) E°cell = -0.23 V,nonspontaneous" class="answers-bank-image d-inline" rel="preload" > 2H2O(l) E° = 1.77V
Fe3+(aq) + e- cell for the following reaction,and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq)  Given: H2O2(aq) + 2H+(aq) + 2e-     2H2O(l) E° = 1.77V Fe3+(aq) + e-   Fe2+(aq) E° = 0.77V A) E°cell = -1.00 V,nonspontaneous B) E°cell = -1.00 V,spontaneous C) E°cell = 1.00 V,nonspontaneous D) E°cell = 1.00 V,spontaneous E) E°cell = -0.23 V,nonspontaneous" class="answers-bank-image d-inline" rel="preload" > Fe2+(aq) E° = 0.77V

Accepted Answer

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

Question 2

Based on the data presented below,which is the strongest reducing agent? E°(V) 
Al3+ + 3e- → Al(s) -1.66
AgBr(s) + e- → Ag(s) +Br-  +0.07
Sn4+ + 2e- → Sn2+ +0.14
Fe3+ + e- → Fe2+ +0.77

Accepted Answer

A)  Fe3+
B)  Fe2+
C)  Br-
D)  Al3+
E)  Al(s) F) A) and D)
G) B) and E)

Question 3

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Accepted Answer

A)  Pb.
B)  Ag.
C)  Sn.
D)  Mg.
E)  Cu.F) A) and C)
G) A) and E)

Question 4

Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? 2+(aq) + 2e- →Ni(s) -0.25 A) -1.40 V B) -0.80 V C) +0.25 V D) +0.80 V E) +1.40 V" class="answers-bank-image d-inline" rel="preload" > Half-Reaction E° (V)  Ni2+(aq) + 2e- →Ni(s) -0.25

Accepted Answer

A)  -1.40 V
B)  -0.80 V
C)  +0.25 V
D)  +0.80 V
E)  +1.40 VF) A) and B)
G) A) and C)

Question 5

Consider the following redox equation. Mn(OH) 2(s) + MnO4-(aq) → MnO42-(aq)  (basic solution) 
When the equation is balanced with the smallest whole number coefficients,what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

Accepted Answer

A)  4,reactant side
B)  4,product side
C)  6,reactant side
D)  6,product side
E)  8,reactant sideF) C) and D)
G) A) and E)

Question 6

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

Accepted Answer

A)  0.47 V
B)  0.21 V
C)  -0.21 V
D)  -0.47 V
E)  0.42 VF) None of the above
G) B) and E)

Question 7

Complete and balance the following redox equation.When properly balanced using the smallest whole-number coefficients,the coefficient of S is H2S + HNO3 → S + NO + H2O (acidic solution)

Accepted Answer

A)  1.
B)  2.
C)  3.
D)  5.
E)  6.F) D) and E)
G) C) and E)

Question 8

In the electrolyte of an electrochemical cell,current is carried by electrons moving from the anode to the cathode.

Accepted Answer

A) True 
 B)False

Question 9

What is E°cell for a galvanic cell represented by the combination of the following half-reactions? ClO4-(aq) + 8 H+(aq) +8e-
  cell for a galvanic cell represented by the combination of the following half-reactions? ClO4-(aq) + 8 H+(aq) +8e-     Cl-(aq) +4H2O(l) E° = 1.389V VO2+(aq) + 2H+(aq) +e-     VO+(aq) +H2O(l) E° = 0.991V A) -0.398 V B) -2.380 V C) 0.398 V D) 2.380 V E) 6.539 V" class="answers-bank-image d-inline" rel="preload" > Cl-(aq) +4H2O(l) E° = 1.389V
VO2+(aq) + 2H+(aq) +e-
  cell for a galvanic cell represented by the combination of the following half-reactions? ClO4-(aq) + 8 H+(aq) +8e-     Cl-(aq) +4H2O(l) E° = 1.389V VO2+(aq) + 2H+(aq) +e-     VO+(aq) +H2O(l) E° = 0.991V A) -0.398 V B) -2.380 V C) 0.398 V D) 2.380 V E) 6.539 V" class="answers-bank-image d-inline" rel="preload" > VO+(aq) +H2O(l) E° = 0.991V

Accepted Answer

A)  -0.398 V
B)  -2.380 V
C)  0.398 V
D)  2.380 V
E)  6.539 VF) B) and D)
G) B) and C)

Question 10

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)  0.00010 M
B)  0.00070 M
C)  0.0049 M
D)  0.030 M
E)  0.050 MF) A) and B)
G) A) and C)

Question 11

The voltaic cell composed of Co(s) ,Co2+(aq) ,Cu(s) ,and Cu2+(aq) has E°cell = 0.62 V.If E° of the cathode half-cell is 0.34 V,what is E° of the anode half-cell? Cu2+(aq) + Co(s) → Cu(s) + Co2+(aq)

Accepted Answer

A)  -0.28 V
B)  -0.96 V
C)  0.28 V
D)  0.96 V
E)  0.21 VF) A) and E)
G) All of the above

Question 12

Complete and balance the following redox equation using the set of smallest whole numbers coefficients.What is the sum of the coefficients? HI + HNO3 → I2 + NO (acidic solution)

Accepted Answer

A)  5
B)  7
C)  14
D)  17
E)  None of these choices is correct.F) B) and E)
G) C) and D)

Question 13

What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) 
Sn2+(aq) + Fe(s)  -1)  Sn2+(aq) + Fe(s)    Sn(s) + Fe2+(aq) E°cell = 0.30V 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) E°cell = 0.30V

Accepted Answer

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

Question 14

At equilibrium E° = 0.

Accepted Answer

A) True 
 B)False

Question 15

What is the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution? 2H2O + 2Cl- (1.0 M) → H2(1 atm) + Cl2(1 atm) + 2OH-(1 × 10-7 M) 
Note that
2H2O(l) + 2e- → H2(g) +2OH-(aq) ,E° = -0.83 V,
2H2O(l) + 2e- → H2(g) +2OH-(aq) ,E = -0.41 V([OH-] = 1 × 10-7M) ,
O2(g) + 4H+(aq) + 4e- →2H2O(l) ,E° = +1.23 V,
Cl2(g) + 2e- → 2Cl-(aq) E° = +1.36 V,and
Na+(aq) + e- → Na(s) E° = -2.71 V

Accepted Answer

A)  2.19 V
B)  1.77 V
C)  0.41 V
D)  -0.41 V
E)  -1.78 VF) None of the above
G) A) and B)

Question 16

What is the oxidizing agent in the (unbalanced) reaction? Cu(s) + H+(aq) + NO3-(aq) → NO(g) + H2O(l) + Cu2+(aq)

Accepted Answer

A)  Cu
B)  H+
C)  NO3-
D)  NO
E)  Cu2+F) A) and B)
G) All of the above

Question 17

The Faraday constant represents the charge of 1 mole of electrons.

Accepted Answer

A) True 
 B)False

Question 18

When the following redox equation is balanced with the smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO4-(aq) + OH-(aq) → Al2O3(s) + S2-(aq) + H2O(l)

Accepted Answer

A)  1
B)  3
C)  4
D)  6
E)  8F) A) and C)
G) All of the above

Question 19

What would you observe if you set up the following electrochemical cell: Ag|AgNO3(0.001 M) ||AgNO3(1 M) |Ag?

Accepted Answer

A)  Electrons will flow from left to right,causing a decrease in the AgNO3 concentration in the left cell,and an increase in the AgNO3 concentration in the right cell.
B)  Electrons will flow from right to left,causing an increase in the AgNO3 concentration in the left cell,and a decrease in the AgNO3 concentration in the right cell.
C)  Electrons will flow from left to right,causing an increase in the AgNO3 concentration in the left cell,and a decrease in AgNO3 concentration in the right cell.
D)  Electrons will flow from right to left,causing a decrease in the AgNO3 concentration in the left cell,and an increase in the AgNO3 concentration in the right cell.
E)  There will be no electron flow because the reduction potential at both electrodes is the same.F) A) and E)
G) B) and C)

Question 20

A salt bridge allows movement of cations and anions from one half-cell to the other.

Accepted Answer

A) True 
 B)False

Exam 19: Electrochemistry

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Correct Answer
verified

Consider the following redox equation. Mn(OH) ₂(s) + MnO₄^-(aq) → MnO₄^2-(aq) (basic solution) When the equation is balanced with the smallest whole number coefficients,what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

Correct Answer
verified

The voltaic cell composed of Co(s) ,Co²⁺(aq) ,Cu(s) ,and Cu²⁺(aq) has E°_cell = 0.62 V.If E° of the cathode half-cell is 0.34 V,what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

Correct Answer
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What would you observe if you set up the following electrochemical cell: Ag|AgNO₃(0.001 M) ||AgNO₃(1 M) |Ag?

Correct Answer
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In the electrolyte of an electrochemical cell,current is carried by electrons moving from the anode to the cathode.

Correct Answer
verified

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

Correct Answer
verified

What is E°_cell for the following reaction,and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq) Given: H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l) E° = 1.77V Fe³⁺(aq) + e^- Fe²⁺(aq) E° = 0.77V

Correct Answer
verified

What is the oxidizing agent in the (unbalanced) reaction? Cu(s) + H⁺(aq) + NO₃^-(aq) → NO(g) + H₂O(l) + Cu²⁺(aq)

Correct Answer
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When the following redox equation is balanced with the smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO₄^-(aq) + OH^-(aq) → Al₂O₃(s) + S^2-(aq) + H₂O(l)

Correct Answer
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What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq) E°_cell = 0.30V

Correct Answer
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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
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At equilibrium E° = 0.

Correct Answer
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Complete and balance the following redox equation.When properly balanced using the smallest whole-number coefficients,the coefficient of S is H₂S + HNO₃ → S + NO + H₂O (acidic solution)

Correct Answer
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Complete and balance the following redox equation using the set of smallest whole numbers coefficients.What is the sum of the coefficients? HI + HNO₃ → I₂ + NO (acidic solution)

Correct Answer
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The Faraday constant represents the charge of 1 mole of electrons.

Correct Answer
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A salt bridge allows movement of cations and anions from one half-cell to the other.

Correct Answer
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Based on the data presented below,which is the strongest reducing agent? E°(V) Al³⁺ + 3e^- → Al(s) -1.66 AgBr(s) + e^- → Ag(s) +Br^- +0.07 Sn⁴⁺ + 2e^- → Sn²⁺ +0.14 Fe³⁺ + e^- → Fe²⁺ +0.77

Correct Answer
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Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? Half-Reaction E° (V) Ni²⁺(aq) + 2e^- →Ni(s) -0.25

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

Correct Answer
verified

Correct Answer
verified

Exam 19: Electrochemistry

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

Correct AnswerverifiedShow Answer

Consider the following redox equation. Mn(OH) 2(s) + MnO4-(aq) → MnO42-(aq) (basic solution) When the equation is balanced with the smallest whole number coefficients,what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

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The voltaic cell composed of Co(s) ,Co2+(aq) ,Cu(s) ,and Cu2+(aq) has E°cell = 0.62 V.If E° of the cathode half-cell is 0.34 V,what is E° of the anode half-cell? Cu2+(aq) + Co(s) → Cu(s) + Co2+(aq)

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What would you observe if you set up the following electrochemical cell: Ag|AgNO3(0.001 M) ||AgNO3(1 M) |Ag?

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In the electrolyte of an electrochemical cell,current is carried by electrons moving from the anode to the cathode.

Correct AnswerverifiedShow Answer

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

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What is E°cell for the following reaction,and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq) Given: H2O2(aq) + 2H+(aq) + 2e- 2H2O(l) E° = 1.77V Fe3+(aq) + e- Fe2+(aq) E° = 0.77V

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What is the oxidizing agent in the (unbalanced) reaction? Cu(s) + H+(aq) + NO3-(aq) → NO(g) + H2O(l) + Cu2+(aq)

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When the following redox equation is balanced with the smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO4-(aq) + OH-(aq) → Al2O3(s) + S2-(aq) + H2O(l)

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What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq) E°cell = 0.30V

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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.

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At equilibrium E° = 0.

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Complete and balance the following redox equation.When properly balanced using the smallest whole-number coefficients,the coefficient of S is H2S + HNO3 → S + NO + H2O (acidic solution)

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Complete and balance the following redox equation using the set of smallest whole numbers coefficients.What is the sum of the coefficients? HI + HNO3 → I2 + NO (acidic solution)

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The Faraday constant represents the charge of 1 mole of electrons.

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A salt bridge allows movement of cations and anions from one half-cell to the other.

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Based on the data presented below,which is the strongest reducing agent? E°(V) Al3+ + 3e- → Al(s) -1.66 AgBr(s) + e- → Ag(s) +Br- +0.07 Sn4+ + 2e- → Sn2+ +0.14 Fe3+ + e- → Fe2+ +0.77

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Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? Half-Reaction E° (V) Ni2+(aq) + 2e- →Ni(s) -0.25

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

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Correct AnswerverifiedShow Answer

Correct Answer
verified

Consider the following redox equation. Mn(OH) ₂(s) + MnO₄^-(aq) → MnO₄^2-(aq) (basic solution) When the equation is balanced with the smallest whole number coefficients,what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

Correct Answer
verified

The voltaic cell composed of Co(s) ,Co²⁺(aq) ,Cu(s) ,and Cu²⁺(aq) has E°_cell = 0.62 V.If E° of the cathode half-cell is 0.34 V,what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

Correct Answer
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What would you observe if you set up the following electrochemical cell: Ag|AgNO₃(0.001 M) ||AgNO₃(1 M) |Ag?

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 galvanic cell that forms from the following half-reactions? Cu²⁺(aq) + 2e^- Cu(s) E° = 0.34V Sn⁴⁺(aq) + 2e^- Sn²⁺(aq) E° = 0.13V

Correct Answer
verified

What is E°_cell for the following reaction,and is it spontaneous or nonspontaneous under standard-state conditions? 2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq) Given: H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l) E° = 1.77V Fe³⁺(aq) + e^- Fe²⁺(aq) E° = 0.77V

Correct Answer
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What is the oxidizing agent in the (unbalanced) reaction? Cu(s) + H⁺(aq) + NO₃^-(aq) → NO(g) + H₂O(l) + Cu²⁺(aq)

Correct Answer
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When the following redox equation is balanced with the smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO₄^-(aq) + OH^-(aq) → Al₂O₃(s) + S^2-(aq) + H₂O(l)

Correct Answer
verified

What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq) E°_cell = 0.30V

Correct Answer
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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
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Correct Answer
verified

Complete and balance the following redox equation.When properly balanced using the smallest whole-number coefficients,the coefficient of S is H₂S + HNO₃ → S + NO + H₂O (acidic solution)

Correct Answer
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Complete and balance the following redox equation using the set of smallest whole numbers coefficients.What is the sum of the coefficients? HI + HNO₃ → I₂ + NO (acidic solution)

Correct Answer
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Correct Answer
verified

Correct Answer
verified

Based on the data presented below,which is the strongest reducing agent? E°(V) Al³⁺ + 3e^- → Al(s) -1.66 AgBr(s) + e^- → Ag(s) +Br^- +0.07 Sn⁴⁺ + 2e^- → Sn²⁺ +0.14 Fe³⁺ + e^- → Fe²⁺ +0.77

Correct Answer
verified

Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? Half-Reaction E° (V) Ni²⁺(aq) + 2e^- →Ni(s) -0.25

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

Correct Answer
verified

Correct Answer
verified