Question 1

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17  ×	imes×  105.Calculate  Δ\DeltaΔ G° for the reaction at 25°C.

Accepted Answer

A)  -12.6 kJ
B)  -28.9 kJ
C)  12.6 kJ
D)  28.9 kJ
E)  None of these choices is correct. F) D) and E)
G) C) and D)

Question 2

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 3

In a fuel cell,an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Accepted Answer

A) True 
 B)False

Question 4

A concentration cell is based on the aqueous reaction
Cu2+(1.00 M) $\to$ Cu2+(0.0100 M)
The cell consists of copper electrodes dipping into solutions of Cu2+ ions.The anions present are sulfate ions.Draw a neat diagram to represent this cell,showing and labeling all necessary components including: anode,cathode,electron flow,cation flow and anion flow.

Accepted Answer

The answer of A concentration cell is based on the...

Question 5

The value of E°cell for the reaction
2Cr3+(aq) + 6Hg(l)   →	o→  2Cr(s) + 3Hg22+(aq) 
Is 1.59 V.Calculate  Δ\DeltaΔ G° for the reaction.

Accepted Answer

A)  -921 kJ
B)  -767 kJ
C)  -460 kJ
D)  -307 kJ
E)  None of these choices is correct. F) A) and C)
G) A) and E)

Question 6

A concentration cell is based on the aqueous reaction
Cu2+(1.00 M) $\to$ Cu2+(0.0100 M)
The cell consists of copper electrodes dipping into solutions of Cu2+ ions.The anions present are sulfate ions.Write the shorthand cell notation for this cell.

Accepted Answer

Cu(s)| Cu²⁺

Question 7

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Accepted Answer

A)  zinc
B)  graphite
C)  copper
D)  iron
E)  sodiumF) A) and B)
G) B) and C)

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

Question 9

Oxidation occurs at the cathode of a galvanic cell,but at the anode of an electrolytic cell.

Accepted Answer

A) True 
 B)False

Question 10

Examine the following half-reactions and select the strongest reducing agent among the species listed.
HgO(s) + H2O(l) + 2e- 2O(l) + 2e-   Hg(l) + 2OH-(aq) ;E° = 0.0977 V Zn(OH) 2(s) + 2e-   Zn(s) + 2OH-(aq) ;E° = -1.25 V Ag2O(s) + H2O(l) + 2e-   Ag(s) + 2OH-(aq) ;E° = 0.342 V B(OH) 3(aq) + 7H+(aq) + 8e-   BH4-(aq) + 3H2O(l) ;E° = -0.481 V A) Hg(l)  B) Zn(s)  C) Ag(s)  D) BH4-(aq)  E) Zn(OH) 2(s) " class="answers-bank-image d-inline" rel="preload" >
Hg(l) + 2OH-(aq) ;E° = 0.0977 V
Zn(OH) 2(s) + 2e- 2O(l) + 2e-   Hg(l) + 2OH-(aq) ;E° = 0.0977 V Zn(OH) 2(s) + 2e-   Zn(s) + 2OH-(aq) ;E° = -1.25 V Ag2O(s) + H2O(l) + 2e-   Ag(s) + 2OH-(aq) ;E° = 0.342 V B(OH) 3(aq) + 7H+(aq) + 8e-   BH4-(aq) + 3H2O(l) ;E° = -0.481 V A) Hg(l)  B) Zn(s)  C) Ag(s)  D) BH4-(aq)  E) Zn(OH) 2(s) " class="answers-bank-image d-inline" rel="preload" >
Zn(s) + 2OH-(aq) ;E° = -1.25 V
Ag2O(s) + H2O(l) + 2e- 2O(l) + 2e-   Hg(l) + 2OH-(aq) ;E° = 0.0977 V Zn(OH) 2(s) + 2e-   Zn(s) + 2OH-(aq) ;E° = -1.25 V Ag2O(s) + H2O(l) + 2e-   Ag(s) + 2OH-(aq) ;E° = 0.342 V B(OH) 3(aq) + 7H+(aq) + 8e-   BH4-(aq) + 3H2O(l) ;E° = -0.481 V A) Hg(l)  B) Zn(s)  C) Ag(s)  D) BH4-(aq)  E) Zn(OH) 2(s) " class="answers-bank-image d-inline" rel="preload" >
Ag(s) + 2OH-(aq) ;E° = 0.342 V
B(OH) 3(aq) + 7H+(aq) + 8e- 2O(l) + 2e-   Hg(l) + 2OH-(aq) ;E° = 0.0977 V Zn(OH) 2(s) + 2e-   Zn(s) + 2OH-(aq) ;E° = -1.25 V Ag2O(s) + H2O(l) + 2e-   Ag(s) + 2OH-(aq) ;E° = 0.342 V B(OH) 3(aq) + 7H+(aq) + 8e-   BH4-(aq) + 3H2O(l) ;E° = -0.481 V A) Hg(l)  B) Zn(s)  C) Ag(s)  D) BH4-(aq)  E) Zn(OH) 2(s) " class="answers-bank-image d-inline" rel="preload" >
BH4-(aq) + 3H2O(l) ;E° = -0.481 V

Accepted Answer

A)  Hg(l) 
B)  Zn(s) 
C)  Ag(s) 
D)  BH4-(aq) 
E)  Zn(OH) 2(s) F) C) and D)
G) A) and B)

Question 11

A solution is prepared by dissolving 32.0 g of NiSO4 in water.What current would be needed to deposit all of the nickel in 5.0 hours?

Accepted Answer

A)  1.1 A
B)  2.2 A
C)  3.3 A
D)  4.4 A
E)  5.5 AF) B) and D)
G) A) and D)

Question 12

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 $\Delta$G° for the cell reaction.

Accepted Answer

a.2A + D <img  loading="lazy" src="/assets/images/blured-textbook.svg" class="d-inline m-1" alt="blured image" width="139" height="30"> ...

Question 13

A concentration cell consists of two Al/Al3+electrodes.The electrolyte in compartment A is 0.050 M Al(NO3) 3 and in compartment B is 1.25 M Al(NO3) 3.What is the voltage of the cell at 25°C?

Accepted Answer

A)  0.083 V
B)  0.062 V
C)  0.041V
D)  0.028 V
E)  None of these choices is correct.F) D) and E)
G) All of the above

Question 14

A concentration cell is based on the aqueous reaction
Cu2+(1.00 M) $\to$ Cu2+(0.0100 M)
Calculate the potential of this cell if it operates at 25.0°C.

Accepted Answer

The answer of A concentration cell is based on the...

Question 15

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) B) and E)

Question 16

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  	imes  105 B) 1.4  	imes  1010 C) 8.6  	imes  10-6 D) 7.1  	imes  10-11 E) 2.3  	imes  1023 " class="answers-bank-image d-inline" rel="preload" >
Sn(s) + Fe2+(aq)

Accepted Answer

A)  1.2  ×	imes×  105
B)  1.4  ×	imes×  1010
C)  8.6  ×	imes×  10-6
D)  7.1  ×	imes×  10-11
E)  2.3  ×	imes×  1023 F) C) and D)
G) A) and B)

Question 17

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.
I2(s) + 2e- cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I2(s) + 2e-   2I-(aq) ;E°= 0.53 V Cr3+(aq) + 3e-   Cr(s) ;E°= -0.74 V Overall reaction: 2Cr(s) + 3I2(s)   	o  2Cr3+(aq) + (aq) + 6I-(aq)  A) E°cell = -1.27 V,spontaneous B) E°cell = -1.27 V,nonspontaneous C) E°cell = 1.27 V,spontaneous D) E°cell = 1.27 V,nonspontaneous E) E°cell = 1.54 V,spontaneous " class="answers-bank-image d-inline" rel="preload" >
2I-(aq) ;E°= 0.53 V
Cr3+(aq) + 3e- cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I2(s) + 2e-   2I-(aq) ;E°= 0.53 V Cr3+(aq) + 3e-   Cr(s) ;E°= -0.74 V Overall reaction: 2Cr(s) + 3I2(s)   	o  2Cr3+(aq) + (aq) + 6I-(aq)  A) E°cell = -1.27 V,spontaneous B) E°cell = -1.27 V,nonspontaneous C) E°cell = 1.27 V,spontaneous D) E°cell = 1.27 V,nonspontaneous E) E°cell = 1.54 V,spontaneous " class="answers-bank-image d-inline" rel="preload" >
Cr(s) ;E°= -0.74 V
Overall reaction:
2Cr(s) + 3I2(s)   →	o→  2Cr3+(aq) + (aq) + 6I-(aq)

Accepted Answer

A)  E°cell = -1.27 V,spontaneous
B)  E°cell = -1.27 V,nonspontaneous
C)  E°cell = 1.27 V,spontaneous
D)  E°cell = 1.27 V,nonspontaneous
E)  E°cell = 1.54 V,spontaneous F) C) and D)
G) A) and B)

Question 18

The following half-reactions occur in the mercury battery used in calculators.If E°cell = 1.357 V,calculate the equilibrium constant for the cell reaction at 25°C.(Assume the stoichiometric coefficients in the cell reaction are all equal to 1. ) 
HgO(s) + H2O(l) + 2e- cell = 1.357 V,calculate the equilibrium constant for the cell reaction at 25°C.(Assume the stoichiometric coefficients in the cell reaction are all equal to 1. )  HgO(s) + H2O(l) + 2e-   Hg(l) + 2OH-(aq)  ZnO(s) + H2O(l) + 2e-   Zn(s) + 2OH-(aq)  A) 9.4  	imes  1022 B) 7.5  	imes  1045 C) 6.4  	imes  1063 D) 7.8  	imes  1091 E) > 9.9  	imes  1099 " class="answers-bank-image d-inline" rel="preload" >
Hg(l) + 2OH-(aq) 
ZnO(s) + H2O(l) + 2e- cell = 1.357 V,calculate the equilibrium constant for the cell reaction at 25°C.(Assume the stoichiometric coefficients in the cell reaction are all equal to 1. )  HgO(s) + H2O(l) + 2e-   Hg(l) + 2OH-(aq)  ZnO(s) + H2O(l) + 2e-   Zn(s) + 2OH-(aq)  A) 9.4  	imes  1022 B) 7.5  	imes  1045 C) 6.4  	imes  1063 D) 7.8  	imes  1091 E) > 9.9  	imes  1099 " class="answers-bank-image d-inline" rel="preload" >
Zn(s) + 2OH-(aq)

Accepted Answer

A)  9.4  ×	imes×  1022
B)  7.5  ×	imes×  1045
C)  6.4  ×	imes×  1063
D)  7.8  ×	imes×  1091
E)  > 9.9  ×	imes×  1099 F) D) and E)
G) C) and D)

Question 19

A concentration cell consists of two Zn/Zn2+ electrodes.The electrolyte in compartment A is 0.10 M Zn(NO3) 2 and in compartment B is 0.60 M Zn(NO3) 2.What is the voltage of the cell at 25°C?

Accepted Answer

A)  0.010 V
B)  0.020 V
C)  0.023 V
D)  0.046 V
E)  None of these choices is correct.F) All of the above
G) A) and B)

Question 20

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

Accepted Answer

A) True 
 B)False

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M) $\to$ Cu²⁺(0.0100 M) The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions.The anions present are sulfate ions.Write the shorthand cell notation for this cell.

Correct Answer
verified
Cu(s)| Cu^{2+View Answer}

In a fuel cell,an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Correct Answer
verified

Correct Answer
verified

Oxidation occurs at the cathode of a galvanic cell,but at the anode of an electrolytic cell.

Correct Answer
verified

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

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

A concentration cell consists of two Zn/Zn²⁺ electrodes.The electrolyte in compartment A is 0.10 M Zn(NO₃) ₂ and in compartment B is 0.60 M Zn(NO₃) ₂.What is the voltage of the cell at 25°C?

Correct Answer
verified

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M) $\to$ Cu²⁺(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 $\times$ 10⁵.Calculate $\Delta$ G° for the reaction at 25°C.

Correct Answer
verified

Correct Answer
verified

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A concentration cell consists of two Al/Al³⁺electrodes.The electrolyte in compartment A is 0.050 M Al(NO₃) ₃ and in compartment B is 1.25 M Al(NO₃) ₃.What is the voltage of the cell at 25°C?

Correct Answer
verified

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

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

Correct Answer
verified

The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l) $\to$ 2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V.Calculate $\Delta$ G° for the reaction.

Correct Answer
verified

A solution is prepared by dissolving 32.0 g of NiSO₄ in water.What current would be needed to deposit all of the nickel in 5.0 hours?

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell is based on the aqueous reaction Cu2+(1.00 M) →\to→ Cu2+(0.0100 M) The cell consists of copper electrodes dipping into solutions of Cu2+ ions.The anions present are sulfate ions.Write the shorthand cell notation for this cell.

Correct AnswerverifiedCu(s)| Cu2+View AnswerShow Answer

In a fuel cell,an external source of electrical power is used to drive a non-spontaneous reaction in which a fuel is produced.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Oxidation occurs at the cathode of a galvanic cell,but at the anode of an electrolytic cell.

Correct AnswerverifiedShow Answer

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

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

A concentration cell consists of two Zn/Zn2+ electrodes.The electrolyte in compartment A is 0.10 M Zn(NO3) 2 and in compartment B is 0.60 M Zn(NO3) 2.What is the voltage of the cell at 25°C?

Correct AnswerverifiedShow Answer

A concentration cell is based on the aqueous reaction Cu2+(1.00 M) →\to→ Cu2+(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Correct AnswerverifiedShow Answer

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

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 ×\times× 105.Calculate Δ\DeltaΔ G° for the reaction at 25°C.

Correct AnswerverifiedShow Answer

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I2(s) + 2e- 2I-(aq) ;E°= 0.53 V Cr3+(aq) + 3e- Cr(s) ;E°= -0.74 V Overall reaction: 2Cr(s) + 3I2(s) →\to→ 2Cr3+(aq) + (aq) + 6I-(aq)

Correct AnswerverifiedShow Answer

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A concentration cell consists of two Al/Al3+electrodes.The electrolyte in compartment A is 0.050 M Al(NO3) 3 and in compartment B is 1.25 M Al(NO3) 3.What is the voltage of the cell at 25°C?

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 Δ\DeltaΔ G° for the cell reaction.

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

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

Correct AnswerverifiedShow Answer

The value of E°cell for the reaction 2Cr3+(aq) + 6Hg(l) →\to→ 2Cr(s) + 3Hg22+(aq) Is 1.59 V.Calculate Δ\DeltaΔ G° for the reaction.

Correct AnswerverifiedShow Answer

A solution is prepared by dissolving 32.0 g of NiSO4 in water.What current would be needed to deposit all of the nickel in 5.0 hours?

Correct AnswerverifiedShow Answer

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M) $\to$ Cu²⁺(0.0100 M) The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions.The anions present are sulfate ions.Write the shorthand cell notation for this cell.

Correct Answer
verified
Cu(s)| Cu^{2+View Answer}

Correct Answer
verified

Correct Answer
verified

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

A concentration cell consists of two Zn/Zn²⁺ electrodes.The electrolyte in compartment A is 0.10 M Zn(NO₃) ₂ and in compartment B is 0.60 M Zn(NO₃) ₂.What is the voltage of the cell at 25°C?

Correct Answer
verified

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M) $\to$ Cu²⁺(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 $\times$ 10⁵.Calculate $\Delta$ G° for the reaction at 25°C.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A concentration cell consists of two Al/Al³⁺electrodes.The electrolyte in compartment A is 0.050 M Al(NO₃) ₃ and in compartment B is 1.25 M Al(NO₃) ₃.What is the voltage of the cell at 25°C?

Correct Answer
verified

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

Correct Answer
verified

The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l) $\to$ 2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V.Calculate $\Delta$ G° for the reaction.

Correct Answer
verified

A solution is prepared by dissolving 32.0 g of NiSO₄ in water.What current would be needed to deposit all of the nickel in 5.0 hours?

Correct Answer
verified