Question 1

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

Accepted Answer

A)  0.47 V
B)  0.21 V
C)  -0.21 V
D)  -0.47 V
E)  0.42 V

Question 2

Which component of the following cell notation is the anode?
P | Q || R | S

Accepted Answer

A)  P
B)  Q
C)  R
D)  S
E)  One of the | symbols is the anode.

Question 3

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

A)  The electrons in the external wire flow from cathode to anode in both types of cell.
B)  Oxidation occurs at the cathode only in a voltaic cell.
C)  The free energy change, Δ\DeltaΔ G,is negative for an electrolytic cell.
D)  The cathode is labeled as positive (+) in a voltaic cell but negative (-) in an electrolytic cell.
E)  Reduction occurs at the anode in an electrolytic cell.

Question 4

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V) .Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

Accepted Answer

A)  0.001 M
B)  0.002 M
C)  0.01 M
D)  0.02 M
E)  0.04 M

Question 5

Two cells are connected in series,so that the same current flows through two electrodes where the following half-reactions occur
Cu2+(aq) + 2e-  →	o→  Cu(s) and Ag+(aq) + e-  →	o→  Ag(s) 
For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

Accepted Answer

A)  0.294 g
B)  0.588 g
C)  0.850 g
D)  1.70 g
E)  3.40 g

Question 6

Calculate  Δ\DeltaΔ G° for the oxidation of 3 moles of copper by nitric acid.
Cu2+(aq) + 2e- 2+(aq) + 2e-   Cu(s) ;E° = 0.34 V NO3-(aq) + 4H+(aq) + 3e-   NO(g) + 2H2O(l) ;E° = 0.957 V A) -120 kJ B) -180 kJ C) -240 kJ D) -300 kJ E) -360 kJ " class="answers-bank-image d-inline" rel="preload" >
Cu(s) ;E° = 0.34 V
NO3-(aq) + 4H+(aq) + 3e- 2+(aq) + 2e-   Cu(s) ;E° = 0.34 V NO3-(aq) + 4H+(aq) + 3e-   NO(g) + 2H2O(l) ;E° = 0.957 V A) -120 kJ B) -180 kJ C) -240 kJ D) -300 kJ E) -360 kJ " class="answers-bank-image d-inline" rel="preload" >
NO(g) + 2H2O(l) ;E° = 0.957 V

Accepted Answer

A)  -120 kJ
B)  -180 kJ
C)  -240 kJ
D)  -300 kJ
E)  -360 kJ

Question 7

Examine the following half-reactions and select the strongest oxidizing agent among the substances.
[PtCl4]2-(aq) + 2e- 4]2-(aq) + 2e-   Pt(s) + 4Cl-(aq) ;E° = 0.755 V RuO4(s) + 8H+(aq) + 8e-   Ru(s) + 4H2O(l) ;E° = 1.038 V FeO42-(aq) + 8H+(aq) + 3e-   Fe3+(aq) + 4H2O(l) ;E° = 2.07 V H4XeO6(aq) + 2H+(aq) + 2e-   XeO3(aq) + 3H2O(l) ;E° = 2.42 V A) [PtCl4]2-(aq)  B) RuO4(s)  C) HFeO4- (aq)  D) H4XeO6(aq)  E) Cl-(aq) " class="answers-bank-image d-inline" rel="preload" >
Pt(s) + 4Cl-(aq) ;E° = 0.755 V
RuO4(s) + 8H+(aq) + 8e- 4]2-(aq) + 2e-   Pt(s) + 4Cl-(aq) ;E° = 0.755 V RuO4(s) + 8H+(aq) + 8e-   Ru(s) + 4H2O(l) ;E° = 1.038 V FeO42-(aq) + 8H+(aq) + 3e-   Fe3+(aq) + 4H2O(l) ;E° = 2.07 V H4XeO6(aq) + 2H+(aq) + 2e-   XeO3(aq) + 3H2O(l) ;E° = 2.42 V A) [PtCl4]2-(aq)  B) RuO4(s)  C) HFeO4- (aq)  D) H4XeO6(aq)  E) Cl-(aq) " class="answers-bank-image d-inline" rel="preload" >
Ru(s) + 4H2O(l) ;E° = 1.038 V
FeO42-(aq) + 8H+(aq) + 3e- 4]2-(aq) + 2e-   Pt(s) + 4Cl-(aq) ;E° = 0.755 V RuO4(s) + 8H+(aq) + 8e-   Ru(s) + 4H2O(l) ;E° = 1.038 V FeO42-(aq) + 8H+(aq) + 3e-   Fe3+(aq) + 4H2O(l) ;E° = 2.07 V H4XeO6(aq) + 2H+(aq) + 2e-   XeO3(aq) + 3H2O(l) ;E° = 2.42 V A) [PtCl4]2-(aq)  B) RuO4(s)  C) HFeO4- (aq)  D) H4XeO6(aq)  E) Cl-(aq) " class="answers-bank-image d-inline" rel="preload" >
Fe3+(aq) + 4H2O(l) ;E° = 2.07 V
H4XeO6(aq) + 2H+(aq) + 2e- 4]2-(aq) + 2e-   Pt(s) + 4Cl-(aq) ;E° = 0.755 V RuO4(s) + 8H+(aq) + 8e-   Ru(s) + 4H2O(l) ;E° = 1.038 V FeO42-(aq) + 8H+(aq) + 3e-   Fe3+(aq) + 4H2O(l) ;E° = 2.07 V H4XeO6(aq) + 2H+(aq) + 2e-   XeO3(aq) + 3H2O(l) ;E° = 2.42 V A) [PtCl4]2-(aq)  B) RuO4(s)  C) HFeO4- (aq)  D) H4XeO6(aq)  E) Cl-(aq) " class="answers-bank-image d-inline" rel="preload" >
XeO3(aq) + 3H2O(l) ;E° = 2.42 V

Accepted Answer

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

Question 8

The lead-acid battery is an example of a secondary battery.

Accepted Answer

A) True 
 B)False

Question 9

The voltaic cell made up of cobalt,copper and their M2+ ions,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)   →	o→  Cu(s) + Co2+(aq)

Accepted Answer

A)  -0.28 V
B)  -0.96V
C)  0.28 V
D)  0.96 V
E)  None of these choices is correct.

Question 10

Consider the non-aqueous cell reaction
2Na(l) + FeCl2(s)  2(s)    2NaCl(s) + Fe(s)  For which E°cell = 2.35 V at 200°C. \Delta G° at this temperature is A) 453 kJ B) -453 kJ C) 907 kJ D) -907 kJ E) None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" >
2NaCl(s) + Fe(s) 
For which E°cell = 2.35 V at 200°C. Δ\DeltaΔ G° at this temperature is

Accepted Answer

A)  453 kJ
B)  -453 kJ
C)  907 kJ
D)  -907 kJ
E)  None of these choices is correct.

Question 11

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 g

Question 12

A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V) and a Fe/Fe2+ electrode (E°= -0.44 V) .If Ecell = 0 and the temperature is 25°C,what is the ratio [Fe2+]/[Cd2+]?

Accepted Answer

A)  2  ×	imes×  101
B)  1  ×	imes×  101
C)  1
D)  1  ×	imes×  10-1
E)  5  ×	imes×  10-2

Question 13

Consider the reaction
CuO(s) + H2(g)   →	o→  Cu(s) + H2O(l) 
In this reaction,which substances are the oxidant and reductant,respectively?

Accepted Answer

A)  CuO and H2
B)  H2 and CuO
C)  CuO and Cu
D)  H2O and H2
E)  None of these choices is correct.

Question 14

Cryolite,Na3AlF6 is used in the electrolysis of aluminum oxide because

Accepted Answer

A)  it is a good source of fluoride ions.
B)  it provides a source of fluorine,an oxidizing agent.
C)  it provides a source of sodium,a reducing agent.
D)  it reduces the energy requirement of the process,by lowering the melting point.
E)  it is very soluble in water.

Question 15

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) $\to$ 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

The answer of Manganese dioxide (MnO2)for use in dry cells...

Question 16

Consider the following balanced redox reaction
3CuO(s) + 2NH3(aq)   →	o→ N2(g) + 3H2O(l) + 3Cu(s) 
Which of the following statements is true?

Accepted Answer

A)  CuO(s) is the oxidizing agent and copper is reduced.
B)  CuO(s) is the oxidizing agent and copper is oxidized.
C)  CuO(s) is the reducing agent and copper is oxidized.
D)  CuO(s) is the reducing agent and copper is reduced.
E)  CuO(s) is the oxidizing agent and N2(g) is the reducing agent.

Question 17

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e. ,they have an element in common,but in different oxidation states) ?

Accepted Answer

A)  HCl and Cl-
B)  H+ and OH-
C)  H2O and H+
D)  Fe3+ and Fe2O3
E)  MnO2 and Mn2+

Question 18

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)   →	o→  I2(s) + Zn(s) 
B)  I2(s) + Zn(s)   →	o→  2I-(aq) + Zn2+(aq) 
C)  2I-(aq) + Zn(s)   →	o→  I2(s) + Zn2+(aq) 
D)  I2(s) + Zn2+(aq)   →	o→  2I-(aq) + Zn(s) 
E)  None of these,since graphite must be in the equation.

Question 19

In the shorthand notation for cells,a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Accepted Answer

A) True 
 B)False

Question 20

Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C.K = 1.17  ×	imes×  105
 Ni2+(aq) + Cd(s)   →	o→  Cd2+(aq) + Ni(s)

Accepted Answer

A)  0.075 V
B)  0.10 V
C)  0.12 V
D)  0.15 V
E)  0.30 V

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Cryolite,Na₃AlF₆ is used in the electrolysis of aluminum oxide because

Correct Answer
verified

Correct Answer
verified

Which component of the following cell notation is the anode? P | Q || R | S

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

Correct Answer
verified

Correct Answer
verified

In the shorthand notation for cells,a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Correct Answer
verified

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e. ,they have an element in common,but in different oxidation states) ?

Correct Answer
verified

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V) .Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

Correct Answer
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Correct Answer
verified

The lead-acid battery is an example of a secondary battery.

Correct Answer
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Correct Answer
verified

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) $\to$ N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
verified

The voltaic cell made up of cobalt,copper and their M²⁺ ions,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) $\to$ Cu(s) + Co²⁺(aq)

Correct Answer
verified

A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V) and a Fe/Fe²⁺ electrode (E°= -0.44 V) .If E_cell = 0 and the temperature is 25°C,what is the ratio [Fe²⁺]/[Cd²⁺]?

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

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C.K = 1.17 $\times$ 10⁵ Ni²⁺(aq) + Cd(s) $\to$ Cd²⁺(aq) + Ni(s)

Correct Answer
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Correct Answer
verified

Consider the reaction CuO(s) + H₂(g) $\to$ Cu(s) + H₂O(l) In this reaction,which substances are the oxidant and reductant,respectively?

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

Which of the following statements about voltaic and electrolytic cells is correct?

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Cryolite,Na3AlF6 is used in the electrolysis of aluminum oxide because

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Which component of the following cell notation is the anode? P | Q || R | S

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

In the shorthand notation for cells,a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Correct AnswerverifiedShow Answer

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e. ,they have an element in common,but in different oxidation states) ?

Correct AnswerverifiedShow Answer

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/Cu2+ electrode (E° = 0.34 V) .Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

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Calculate Δ\DeltaΔ G° for the oxidation of 3 moles of copper by nitric acid. Cu2+(aq) + 2e- Cu(s) ;E° = 0.34 V NO3-(aq) + 4H+(aq) + 3e- NO(g) + 2H2O(l) ;E° = 0.957 V

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The lead-acid battery is an example of a secondary battery.

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Consider the non-aqueous cell reaction 2Na(l) + FeCl2(s) 2NaCl(s) + Fe(s) For which E°cell = 2.35 V at 200°C. Δ\DeltaΔ G° at this temperature is

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Consider the following balanced redox reaction 3CuO(s) + 2NH3(aq) →\to→ N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true?

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The voltaic cell made up of cobalt,copper and their M2+ ions,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) →\to→ Cu(s) + Co2+(aq)

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A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V) and a Fe/Fe2+ electrode (E°= -0.44 V) .If Ecell = 0 and the temperature is 25°C,what is the ratio [Fe2+]/[Cd2+]?

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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

Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C.K = 1.17 ×\times× 105 Ni2+(aq) + Cd(s) →\to→ Cd2+(aq) + Ni(s)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the reaction CuO(s) + H2(g) →\to→ Cu(s) + H2O(l) In this reaction,which substances are the oxidant and reductant,respectively?

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

Correct AnswerverifiedShow Answer

Which of the following statements about voltaic and electrolytic cells is correct?

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Cryolite,Na₃AlF₆ is used in the electrolysis of aluminum oxide because

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/Cu²⁺ electrode (E° = 0.34 V) .Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

Correct Answer
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Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) $\to$ N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
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The voltaic cell made up of cobalt,copper and their M²⁺ ions,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) $\to$ Cu(s) + Co²⁺(aq)

Correct Answer
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A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V) and a Fe/Fe²⁺ electrode (E°= -0.44 V) .If E_cell = 0 and the temperature is 25°C,what is the ratio [Fe²⁺]/[Cd²⁺]?

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

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C.K = 1.17 $\times$ 10⁵ Ni²⁺(aq) + Cd(s) $\to$ Cd²⁺(aq) + Ni(s)

Correct Answer
verified

Correct Answer
verified

Consider the reaction CuO(s) + H₂(g) $\to$ Cu(s) + H₂O(l) In this reaction,which substances are the oxidant and reductant,respectively?

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