Question 1

Determine the equilibrium constant for the following reaction at 25°C.
2I- (aq)+ Br2(l)$\rarr$I2(s)+ 2Br-(aq).

Accepted Answer

1.8 * 10<s...

Question 2

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO2(s) + Cl-  →\rarr→  Pb2+ + Cl2(g) (acidic solution)

Accepted Answer

A)  2
B)  4
C)  5
D)  9
E)  11 F) B) and D)
G) B) and C)

Question 3

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Accepted Answer

Question 4

The measured voltage of the cell Pt(s) | H2 (1.0 atm) | H+(aq) || Ag+(1.0 M) | Ag(s) is 1.02 V at 25°C. Calculate the pH of the solution.

Accepted Answer

A)  1.86
B)  1.69
C)  3.72
D)  3.89
E)  7.43F) B) and E)
G) D) and E)

Question 5

Suppose the reaction Pb(s) + 2H+(aq)   →\rarr→ Pb2+(aq) + H2(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

Accepted Answer

A)  2.5 M.
B)  1.6 * 10-2 M.
C)  2.5 * 10-4 M.
D)  1.6 * 10-6 M.
E)  0.40 M. F) None of the above
G) A) and E)

Question 6

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 * 10-9 M
C)  6.2 * 10-3 M
D)  2.6 * 10-51 M
E)  6.2 * 10-5 MF) A) and B)
G) D) and E)

Question 7

Many different ways have been proposed to make batteries. One cell is set up with copper and lead electrodes in contact with CuSO4(aq)and Pb(NO3)2 (aq), respectively. If the Pb2+ and Cu2+ concentrations are each 1.0 M, what is the overall cell potential?
Pb2+ + 2e- $\rarr$ Pb E° = -0.22 V
Cu2+ + 2e- $\rarr$ Cu E° = +0.34 V

Accepted Answer

The answer of Many different ways have been proposed to...

Question 8

Consider the following reaction: 2Fe2+(aq) + Cu2+  →\rarr→ 2Fe3+(aq) + Cu. When the reaction comes to equilibrium, what is the cell voltage?

Accepted Answer

A)  0.43 V
B)  1.11 V
C)  0.78 V
D)  -0.43 V
E)  0 V F) A) and E)
G) All of the above

Question 9

Complete and balance the following redox reaction under basic conditions:
CrO42-(aq)+ SO32-(aq)$\rarr$ Cr(OH)3(s)+ SO42-(aq)

Accepted Answer

2CrO₄^2-(...

Question 10

Which of the following species is the strongest oxidizing agent under standard-state conditions?

Accepted Answer

A)  Ag+(aq) 
B)  H2(g) 
C)  H+(aq) 
D)  Cl2(g) 
E)  Al3+(aq) F) A) and D)
G) B) and C)

Question 11

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M) || Cu2+ (0.0500 M) | Cu

Accepted Answer

A)  0.62 V
B)  0.52 V
C)  0.59 V
D)  0.66 V
E)  0.56 VF) A) and D)
G) A) and E)

Question 12

Calculate E°cell for the following reaction: 2Fe2+(aq) + Cd2+(aq)  →\rarr→ 2Fe3+(aq) + Cd(s)

Accepted Answer

A)  -0.37 V
B)  0.37 V
C)  -1.17 V
D)  1.17 V
E)  None of these. F) None of the above
G) A) and B)

Question 13

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Accepted Answer

Question 14

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

Question 15

Consider the reaction 2Fe3+(aq) + Fe(s)  →\rarr→  3Fe2+(aq) . Find the equilibrium constant for this reaction at 25°C.

Accepted Answer

A)  1 * 1011
B)  8 * 1040
C)  3 * 1020
D)  7 * 10-12
E)  1 * 10-41 F) B) and D)
G) C) and E)

Question 16

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn2+ || NO3- (acid soln) , NO(g) | Pt

Accepted Answer

A)  Sn
B)  Sn2+
C)  NO3-
D)  NO
E)  PtF) B) and C)
G) All of the above

Question 17

What concentration of Ni2+ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Accepted Answer

Question 18

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Accepted Answer

A)  0.20 g
B)  0.40 g
C)  12 g
D)  24 g
E)  47 gF) C) and D)
G) A) and E)

Question 19

Which element is associated with the term "galvanized"?

Accepted Answer

A)  Ga
B)  Zn
C)  Cd
D)  Hg
E)  PbF) A) and B)
G) A) and C)

Question 20

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M)$\rarr$Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

Accepted Answer

A) True 
 B)False

Exam 19: Redox Reactions and Electrochemistry

Which element is associated with the term "galvanized"?

Correct Answer
verified

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

Correct Answer
verified

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min?

Correct Answer
verified

Correct Answer
verified

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M) $\rarr$ Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 25°C. 2I^-(aq)+ Br₂(l) $\rarr$ I₂(s)+ 2Br^-(aq).

Correct Answer
verified
1.8 * 10
View Answer

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO₂(s) + Cl^- $\rarr$ Pb²⁺ + Cl₂(g) (acidic solution)

Correct Answer
verified

The measured voltage of the cell Pt(s) | H₂ (1.0 atm) | H⁺(aq) || Ag⁺(1.0 M) | Ag(s) is 1.02 V at 25°C. Calculate the pH of the solution.

Correct Answer
verified

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn²⁺ || NO₃^-(acid soln) , NO(g) | Pt

Correct Answer
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Suppose the reaction Pb(s) + 2H⁺(aq) $\rarr$ Pb²⁺(aq) + H₂(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

Correct Answer
verified

Consider the following reaction: 2Fe²⁺(aq) + Cu²⁺ $\rarr$ 2Fe³⁺(aq) + Cu. When the reaction comes to equilibrium, what is the cell voltage?

Correct Answer
verified

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Correct Answer
verified

Which of the following species is the strongest oxidizing agent under standard-state conditions?

Correct Answer
verified

Find the emf of the cell described by the cell diagram Ni | Ni²⁺ (0.750 M) || Cu²⁺ (0.0500 M) | Cu

Correct Answer
verified

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
verified

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

Correct Answer
verified

Complete and balance the following redox reaction under basic conditions: CrO₄^2-(aq)+ SO₃^2-(aq) $\rarr$ Cr(OH)₃(s)+ SO₄^2-(aq)

Correct Answer
verified
2CrO₄^2-(...
View Answer

Calculate E°_cell for the following reaction: 2Fe²⁺(aq) + Cd²⁺(aq) $\rarr$ 2Fe³⁺(aq) + Cd(s)

Correct Answer
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Consider the reaction 2Fe³⁺(aq) + Fe(s) $\rarr$ 3Fe²⁺(aq) . Find the equilibrium constant for this reaction at 25°C.

Correct Answer
verified

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Correct Answer
verified

Exam 19: Redox Reactions and Electrochemistry

Which element is associated with the term "galvanized"?

Correct AnswerverifiedShow Answer

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO3(aq)using a current of 6.0 A?

Correct AnswerverifiedShow Answer

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

The electrochemical cell that utilizes the reaction Zn + Cu2+ (1 M) →\rarr→ Zn2+ (1 M)+ Cu will have a lower cell emf when the concentrations of Zn2+ and Cu2+ ions are decreased to 0.1 M.

Correct AnswerverifiedShow Answer

Determine the equilibrium constant for the following reaction at 25°C. 2I- (aq)+ Br2(l) →\rarr→ I2(s)+ 2Br-(aq).

Correct Answerverified1.8 * 10View AnswerShow Answer

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO2(s) + Cl- →\rarr→ Pb2+ + Cl2(g) (acidic solution)

Correct AnswerverifiedShow Answer

The measured voltage of the cell Pt(s) | H2 (1.0 atm) | H+(aq) || Ag+(1.0 M) | Ag(s) is 1.02 V at 25°C. Calculate the pH of the solution.

Correct AnswerverifiedShow Answer

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn2+ || NO3- (acid soln) , NO(g) | Pt

Correct AnswerverifiedShow Answer

Suppose the reaction Pb(s) + 2H+(aq) →\rarr→ Pb2+(aq) + H2(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

Correct AnswerverifiedShow Answer

Consider the following reaction: 2Fe2+(aq) + Cu2+ →\rarr→ 2Fe3+(aq) + Cu. When the reaction comes to equilibrium, what is the cell voltage?

Correct AnswerverifiedShow Answer

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl2. If Ecell is found to be 0.24 V, what is the pH of the acetic acid solution?

Correct AnswerverifiedShow Answer

Which of the following species is the strongest oxidizing agent under standard-state conditions?

Correct AnswerverifiedShow Answer

Find the emf of the cell described by the cell diagram Ni | Ni2+ (0.750 M) || Cu2+ (0.0500 M) | Cu

Correct AnswerverifiedShow Answer

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 AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Complete and balance the following redox reaction under basic conditions: CrO42-(aq)+ SO32-(aq) →\rarr→ Cr(OH)3(s)+ SO42-(aq)

Correct Answerverified2CrO42-(...View AnswerShow Answer

Calculate E°cell for the following reaction: 2Fe2+(aq) + Cd2+(aq) →\rarr→ 2Fe3+(aq) + Cd(s)

Correct AnswerverifiedShow Answer

Consider the reaction 2Fe3+(aq) + Fe(s) →\rarr→ 3Fe2+(aq) . Find the equilibrium constant for this reaction at 25°C.

Correct AnswerverifiedShow Answer

What concentration of Ni2+ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO4 solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Correct AnswerverifiedShow Answer

Correct Answer
verified

How many moles of silver metal are produced in 1.2 hours by the electrolysis of AgNO₃(aq)using a current of 6.0 A?

Correct Answer
verified

How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO₄ for 90.0 min?

Correct Answer
verified

Correct Answer
verified

The electrochemical cell that utilizes the reaction Zn + Cu²⁺(1 M) $\rarr$ Zn²⁺(1 M)+ Cu will have a lower cell emf when the concentrations of Zn²⁺ and Cu²⁺ ions are decreased to 0.1 M.

Correct Answer
verified

Determine the equilibrium constant for the following reaction at 25°C. 2I^-(aq)+ Br₂(l) $\rarr$ I₂(s)+ 2Br^-(aq).

Correct Answer
verified
1.8 * 10
View Answer

Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation? PbO₂(s) + Cl^- $\rarr$ Pb²⁺ + Cl₂(g) (acidic solution)

Correct Answer
verified

The measured voltage of the cell Pt(s) | H₂ (1.0 atm) | H⁺(aq) || Ag⁺(1.0 M) | Ag(s) is 1.02 V at 25°C. Calculate the pH of the solution.

Correct Answer
verified

According to the following cell diagram, which chemical species undergoes reduction? Sn | Sn²⁺ || NO₃^-(acid soln) , NO(g) | Pt

Correct Answer
verified

Suppose the reaction Pb(s) + 2H⁺(aq) $\rarr$ Pb²⁺(aq) + H₂(g) is carried out at pH = 4.00 and at a hydrogen gas pressure of 1.00 atm. The concentration of lead(II) ions that causes this reaction to be at equilibrium is

Correct Answer
verified

Consider the following reaction: 2Fe²⁺(aq) + Cu²⁺ $\rarr$ 2Fe³⁺(aq) + Cu. When the reaction comes to equilibrium, what is the cell voltage?

Correct Answer
verified

A standard hydrogen electrode is immersed in an acetic acid solution. This electrode is connected by an external circuit to an iron nail dipping into 0.10 M FeCl₂. If E_cell is found to be 0.24 V, what is the pH of the acetic acid solution?

Correct Answer
verified

Correct Answer
verified

Find the emf of the cell described by the cell diagram Ni | Ni²⁺ (0.750 M) || Cu²⁺ (0.0500 M) | Cu

Correct Answer
verified

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
verified

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

Correct Answer
verified

Complete and balance the following redox reaction under basic conditions: CrO₄^2-(aq)+ SO₃^2-(aq) $\rarr$ Cr(OH)₃(s)+ SO₄^2-(aq)

Correct Answer
verified
2CrO₄^2-(...
View Answer

Calculate E°_cell for the following reaction: 2Fe²⁺(aq) + Cd²⁺(aq) $\rarr$ 2Fe³⁺(aq) + Cd(s)

Correct Answer
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Consider the reaction 2Fe³⁺(aq) + Fe(s) $\rarr$ 3Fe²⁺(aq) . Find the equilibrium constant for this reaction at 25°C.

Correct Answer
verified

What concentration of Ni²⁺ ion remains in solution after electrolysis of 100. mL of 0.250 M NiSO₄ solution when using a current of 2.40 amperes for 30.0 minutes? Assume Ni metal is plated out.

Correct Answer
verified