Question 1

Consider the reaction Fe + Sn2+(1 $\times$ 10-3 M)$\to$ Fe2+(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

Accepted Answer

The answer of Consider the reaction Fe + Sn2+(1 $\times$...

Question 2

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s)  →	o→  2Ag(s) + 2Cl-  + Zn2+.
If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Accepted Answer

A)  increase by 0.06 V.
B)  increase by 0.18 V.
C)  decrease by 0.06 V.
D)  decrease by 0.18 V.
E)  increase by 0.35 V. F) C) and D)
G) All of the above

Question 3

Given the following standard reduction potentials, -14 B) 2.3  	imes  1013 C) 2.1  	imes  10-14 D) 5.1  	imes  1013 E) None of these " class="answers-bank-image d-inline" rel="preload" > calculate the solubility product of AgCN at 25°C.

Accepted Answer

A)  4.3  ×	imes×  10-14
B)  2.3  ×	imes×  1013
C)  2.1  ×	imes×  10-14
D)  5.1  ×	imes×  1013
E)  None of these F) A) and B)
G) A) and C)

Question 4

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25°C?

Accepted Answer

A)  Al
B)  Fe
C)  Ag
D)  Ni
E)  MgF) None of the above
G) A) and E)

Question 5

Calculate the cell emf for the following reaction at 25°C:
2Ag+(0.010 M)+ H2(1 atm)$\to$ 2Ag(s)+ 2H+(pH = 6.0)

Accepted Answer

The answer of Calculate the cell emf for the following...

Question 6

The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl2 solution is

Accepted Answer

A)  Cu+ + e-  →	o→  Cu.
B)  Cu2+ + e-  →	o→ Cu+.
C)  2H2O + 2e-  →	o→  H2 + 2OH-.
D)  Cl2 + 2e-  →	o→  2Cl-.
E)  2Cl-  →	o→ Cl2 + 2e-. F) A) and B)
G) C) and D)

Question 7

Which one of the following reagents is capable of transforming Cu(s) to Cu2+ (1 M) ?

Accepted Answer

A)  I- (1 M) 
B)  Ni(s) 
C)  Ag+ (1 M) 
D)  Al3+ (1 M) 
E)  H+ (1 M) F) A) and C)
G) C) and D)

Question 8

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M) + H2(1 atm)  →	o→  2Ag(s) + 2H+(pH = 10.0)

Accepted Answer

A)  1.04 V
B)  1.27 V
C)  0.92 V
D)  0.56 V
E)  0.80 V F) A) and D)
G) A) and B)

Question 9

How long will it take to produce 78 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.0 A?

Accepted Answer

A)  0.01 s
B)  420 s
C)  13 h
D)  116 h
E)  1.0  ×	imes×  1012 s F) None of the above
G) D) and E)

Question 10

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.Calculate the mass of cadmium metal deposited.

Accepted Answer

A)  3.2  ×	imes×  10-7 g
B)  1.2  ×	imes×  10-3 g
C)  4.2 g
D)  8.4 g
E)  16.8 g F) C) and D)
G) B) and C)

Question 11

A certain electrochemical cell has for its cell reaction: Zn + HgO  →	o→  ZnO + Hg
Which is the half-reaction occurring at the anode?

Accepted Answer

A)  HgO + 2e- →	o→  Hg + O2-
B)  Zn2+ + 2e-  →	o→  Zn
C)  Zn  →	o→  Zn2+ + 2e-
D)  ZnO + 2e-  →	o→  Zn E) B) and C)
F) All of the above

Question 12

If the measured voltage of the cell Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s) is 1.37 V when the concentration of Zn2+ ion is 0.010 M, what is the Ag+ ion concentration?

Accepted Answer

A)  2.5 M
B)  4.0  ×	imes×  10-9 M
C)  6.2  ×	imes×  10-3 M
D)  2.6  ×	imes×  10-51 M
E)  6.2  ×	imes×  10-5 M F) B) and D)
G) B) and C)

Question 13

Which one of the following reagents is capable of transforming Fe3+ (1 M) to Fe2+ (1 M) ?

Accepted Answer

A)  H2(1 atm) 
B)  NO3- (1 M) 
C)  O2(1 atm) 
D)  Br- (1 M) 
E)  H+ (1 M) F) A) and B)
G) B) and D)

Question 14

For the reaction Ni2+(aq) + 2Fe2+(aq)  →	o→  Ni(s) + 2Fe3+(aq) , the standard cell potential E°cell is

Accepted Answer

A)  +2.81 V.
B)  +1.02 V.
C)  +0.52 V.
D)  -1.02 V.
E)  -2.81 V. F) A) and C)
G) A) and E)

Question 15

Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. • an Al(s) electrode in 1.0 M Al(NO3) 3 solution
• a Pb(s) electrode in 1.0 M Pb(NO3) 2 solution
The balanced overall (net) cell reaction is

Accepted Answer

A)  Pb(s) + Al3+(aq)  →	o→  Pb2+(aq) + Al(s.) 
B)  3Pb(s) + 2Al3+(aq)  →	o→  3Pb2+(aq) + 2Al(s) .
C)  3Pb2+(aq) + 2Al(s)  →	o→  3Pb(s) + 2Al3+(aq) .
D)  Pb2+(aq) + Al(s)  →	o→  Pb(s) + Al3+(aq) . E) A) and B)
F) All of the above

Question 16

Consider the following standard reduction potentials in acid solution: 3+. B) Fe2+. C) Br-. D) Al3+. E) Al." class="answers-bank-image d-inline" rel="preload" > The strongest reducing agent among those shown above is

Accepted Answer

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

Question 17

For the electrochemical cell Pt(s) | H2(1 atm) | H+(1 M) || Cu2+(1 M) | Cu(s) , which one of the following changes will cause an increase in the cell voltage?

Accepted Answer

A)  Lower the H2(g) pressure.
B)  Increase the size/mass of the copper electrode.
C)  Lower the H+(aq) concentration.
D)  Decrease the concentration of Cu2+ ion.
E)  None of the above.F) None of the above
G) B) and E)

Question 18

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

Accepted Answer

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

Question 19

Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu2+(aq) + H2(g)  →	o→  Cu(s) + 2H+(aq) .Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Accepted Answer

A)  The emf will increase.
B)  The emf will decrease.
C)  No change in the emf will be observed. D) All of the above
E) A) and C)

Question 20

Predict the products obtained from electrolysis of a 1 M AlBr3 solution. Note that 2H2O(l) + 2e-  →	o→  H2(g) + 2OH-(aq) , E°red = -0.83 V, and
O2(g) + 4H+(aq) + 4e-  →	o→  2H2O(l) , E°red = +1.23 V

Accepted Answer

A)  Al and Br2
B)  Al and O2
C)  H2 and O2
D)  H2 and Br2
E)  Al and H2 F) A) and D)
G) A) and E)

Exam 19: Electrochemistry

Predict the products obtained from electrolysis of a 1 M AlBr₃solution. Note that 2H₂O(l) + 2e^- $\to$ H₂(g) + 2OH^-(aq) , E°_red = -0.83 V, and O₂(g) + 4H⁺(aq) + 4e^- $\to$ 2H₂O(l) , E°_red = +1.23 V

Correct Answer
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How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A?

Correct Answer
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Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\to$ 2Ag(s)+ 2H⁺(pH = 6.0)

Correct Answer
verified

Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. • an Al(s) electrode in 1.0 M Al(NO₃) ₃ solution • a Pb(s) electrode in 1.0 M Pb(NO₃) ₂ solution The balanced overall (net) cell reaction is

Correct Answer
verified

Correct Answer
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Which one of the following reagents is capable of transforming Fe³⁺(1 M) to Fe²⁺(1 M) ?

Correct Answer
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If the measured voltage of the cell Zn(s) | Zn²⁺(aq) || Ag⁺(aq) | Ag(s) is 1.37 V when the concentration of Zn²⁺ ion is 0.010 M, what is the Ag⁺ ion concentration?

Correct Answer
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Consider the reaction Fe + Sn²⁺(1 $\times$ 10^-3 M) $\to$ Fe²⁺(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

Correct Answer
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The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl₂ solution is

Correct Answer
verified

For the reaction Ni²⁺(aq) + 2Fe²⁺(aq) $\to$ Ni(s) + 2Fe³⁺(aq) , the standard cell potential E°_cell is

Correct Answer
verified

A certain electrochemical cell has for its cell reaction: Zn + HgO $\to$ ZnO + Hg Which is the half-reaction occurring at the anode?

Correct Answer
verified

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25°C?

Correct Answer
verified

Which one of the following reagents is capable of transforming Cu(s) to Cu²⁺(1 M) ?

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 $\to$ S + NO (acidic solution)

Correct Answer
verified

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M) + H₂(1 atm) $\to$ 2Ag(s) + 2H⁺(pH = 10.0)

Correct Answer
verified

Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu²⁺(aq) + H₂(g) $\to$ Cu(s) + 2H⁺(aq) .Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Correct Answer
verified

Consider the following standard reduction potentials in acid solution: The strongest reducing agent among those shown above is

Correct Answer
verified

For the electrochemical cell Pt(s) | H₂(1 atm) | H⁺(1 M) || Cu²⁺(1 M) | Cu(s) , which one of the following changes will cause an increase in the cell voltage?

Correct Answer
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Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) $\to$ 2Ag(s) + 2Cl^- + Zn²⁺. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct Answer
verified

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours.Calculate the mass of cadmium metal deposited.

Correct Answer
verified

Exam 19: Electrochemistry

Predict the products obtained from electrolysis of a 1 M AlBr3 solution. Note that 2H2O(l) + 2e- →\to→ H2(g) + 2OH-(aq) , E°red = -0.83 V, and O2(g) + 4H+(aq) + 4e- →\to→ 2H2O(l) , E°red = +1.23 V

Correct AnswerverifiedShow Answer

How long will it take to produce 78 g of Al metal by the reduction of Al3+ in an electrolytic cell with a current of 2.0 A?

Correct AnswerverifiedShow Answer

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M)+ H2(1 atm) →\to→ 2Ag(s)+ 2H+(pH = 6.0)

Correct AnswerverifiedShow Answer

Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. • an Al(s) electrode in 1.0 M Al(NO3) 3 solution • a Pb(s) electrode in 1.0 M Pb(NO3) 2 solution The balanced overall (net) cell reaction is

Correct AnswerverifiedShow Answer

Given the following standard reduction potentials, calculate the solubility product of AgCN at 25°C.

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Which one of the following reagents is capable of transforming Fe3+ (1 M) to Fe2+ (1 M) ?

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If the measured voltage of the cell Zn(s) | Zn2+(aq) || Ag+(aq) | Ag(s) is 1.37 V when the concentration of Zn2+ ion is 0.010 M, what is the Ag+ ion concentration?

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Consider the reaction Fe + Sn2+(1 ×\times× 10-3 M) →\to→ Fe2+(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

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The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl2 solution is

Correct AnswerverifiedShow Answer

For the reaction Ni2+(aq) + 2Fe2+(aq) →\to→ Ni(s) + 2Fe3+(aq) , the standard cell potential E°cell is

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A certain electrochemical cell has for its cell reaction: Zn + HgO →\to→ ZnO + Hg Which is the half-reaction occurring at the anode?

Correct AnswerverifiedShow Answer

Which of these metals will not be oxidized in hydrochloric acid under standard conditions at 25°C?

Correct AnswerverifiedShow Answer

Which one of the following reagents is capable of transforming Cu(s) to Cu2+ (1 M) ?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Calculate the cell emf for the following reaction at 25°C: 2Ag+(0.010 M) + H2(1 atm) →\to→ 2Ag(s) + 2H+(pH = 10.0)

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Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu2+(aq) + H2(g) →\to→ Cu(s) + 2H+(aq) .Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Correct AnswerverifiedShow Answer

Consider the following standard reduction potentials in acid solution: The strongest reducing agent among those shown above is

Correct AnswerverifiedShow Answer

For the electrochemical cell Pt(s) | H2(1 atm) | H+(1 M) || Cu2+(1 M) | Cu(s) , which one of the following changes will cause an increase in the cell voltage?

Correct AnswerverifiedShow Answer

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) →\to→ 2Ag(s) + 2Cl- + Zn2+. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct AnswerverifiedShow Answer

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.Calculate the mass of cadmium metal deposited.

Correct AnswerverifiedShow Answer

Predict the products obtained from electrolysis of a 1 M AlBr₃solution. Note that 2H₂O(l) + 2e^- $\to$ H₂(g) + 2OH^-(aq) , E°_red = -0.83 V, and O₂(g) + 4H⁺(aq) + 4e^- $\to$ 2H₂O(l) , E°_red = +1.23 V

Correct Answer
verified

How long will it take to produce 78 g of Al metal by the reduction of Al³⁺ in an electrolytic cell with a current of 2.0 A?

Correct Answer
verified

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M)+ H₂(1 atm) $\to$ 2Ag(s)+ 2H⁺(pH = 6.0)

Correct Answer
verified

Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. • an Al(s) electrode in 1.0 M Al(NO₃) ₃ solution • a Pb(s) electrode in 1.0 M Pb(NO₃) ₂ solution The balanced overall (net) cell reaction is

Correct Answer
verified

Correct Answer
verified

Which one of the following reagents is capable of transforming Fe³⁺(1 M) to Fe²⁺(1 M) ?

Correct Answer
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If the measured voltage of the cell Zn(s) | Zn²⁺(aq) || Ag⁺(aq) | Ag(s) is 1.37 V when the concentration of Zn²⁺ ion is 0.010 M, what is the Ag⁺ ion concentration?

Correct Answer
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Consider the reaction Fe + Sn²⁺(1 $\times$ 10^-3 M) $\to$ Fe²⁺(1.0 M)+ Sn. Calculate the voltage theoretically generated by the cell.

Correct Answer
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The half-reaction that occurs at the cathode during electrolysis of an aqueous CuCl₂ solution is

Correct Answer
verified

For the reaction Ni²⁺(aq) + 2Fe²⁺(aq) $\to$ Ni(s) + 2Fe³⁺(aq) , the standard cell potential E°_cell is

Correct Answer
verified

A certain electrochemical cell has for its cell reaction: Zn + HgO $\to$ ZnO + Hg Which is the half-reaction occurring at the anode?

Correct Answer
verified

Correct Answer
verified

Which one of the following reagents is capable of transforming Cu(s) to Cu²⁺(1 M) ?

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 $\to$ S + NO (acidic solution)

Correct Answer
verified

Calculate the cell emf for the following reaction at 25°C: 2Ag⁺(0.010 M) + H₂(1 atm) $\to$ 2Ag(s) + 2H⁺(pH = 10.0)

Correct Answer
verified

Consider an electrochemical cell with the following cell reaction where all reactants and products are at standard-state conditions: Cu²⁺(aq) + H₂(g) $\to$ Cu(s) + 2H⁺(aq) .Predict the effect on the emf of this cell of adding NaOH solution to the hydrogen half-cell until the pH equals 7.0.

Correct Answer
verified

Correct Answer
verified

For the electrochemical cell Pt(s) | H₂(1 atm) | H⁺(1 M) || Cu²⁺(1 M) | Cu(s) , which one of the following changes will cause an increase in the cell voltage?

Correct Answer
verified

Consider an electrochemical cell based on the spontaneous reaction 2AgCl(s) + Zn(s) $\to$ 2Ag(s) + 2Cl^- + Zn²⁺. If the zinc ion concentration is kept constant at 1 M, and the chlorine ion concentration is decreased from 1 M to 0.001 M, the cell voltage should

Correct Answer
verified

A current of 0.80 A was applied to an electrolytic cell containing molten CdCl₂ for 2.5 hours.Calculate the mass of cadmium metal deposited.

Correct Answer
verified