Question 1

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

Question 2

Will H2(g)form when Cu is placed in 1.0 M HCl?

Accepted Answer

Question 3

For the electrochemical cell Ni(s)| Ni2+(1 M)|| H+(1 M)| H2(1 atm)| Pt(s), which one of the following changes will cause a decrease in the cell voltage?

Accepted Answer

A) Increase the pressure of H2 to 2.0 atm . 
B) Decrease the mass of the nickel electrode. 
C) Lower the pH of the cell electrolyte. 
D) Decrease the concentration of Ni2+ ion. 
E) None of the above. 
A) Increase the pressure of H2 to 2.0 atm . 
B) Decrease the mass of the nickel electrode. 
C) Lower the pH of the cell electrolyte. 
D) Decrease the concentration of Ni2+ ion. 
E) None of the above.

Question 4

Which one of the following reagents is capable of transforming Br- (aq)to Br2(l)under standard-state conditions?

Accepted Answer

A) I- (aq) 
B) NO3- (aq) 
C) Ag+ (aq) 
D) Al3+ (aq) 
E) Au3+ (aq) 
A) I- (aq) 
B) NO3- (aq) 
C) Ag+ (aq) 
D) Al3+ (aq) 
E) Au3+ (aq)

Question 5

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

Accepted Answer

2CrO₄^2-(

Question 6

Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq)|| Cl2(g), Cl- (aq)| Pt
Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu4+/Pu3+)?

Accepted Answer

A) 2.37 V 
B) 1.01 V 
C) -1.71 V 
D) -1.01 V 
E) 1.71 V 
A) 2.37 V 
B) 1.01 V 
C) -1.71 V 
D) -1.01 V 
E) 1.71 V

Question 7

Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br- (aq)+ I2(s)    
Br2(l)+ 2I- (aq)

Accepted Answer

A) 5.7 $\times$ 10-19 
B) 18.30 
C) 1.7 $\times$ 1054 
D) 1.9 $\times$ 1018 
E) 5.7 $\times$ 10-55 
A) 5.7 $\times$ 10-19 
B) 18.30 
C) 1.7 $\times$ 1054 
D) 1.9 $\times$ 1018 
E) 5.7 $\times$ 10-55

Question 8

For the reaction, 2Cr2+ + Cl2(g)$\to$ 2Cr3+ + 2Cl-, E°cell is 1.78 V.Calculate E°cell for the related reaction Cr3+ + Cl- $\to$ Cr2+ + 1/2Cl2(g).

Accepted Answer

A) 1.78 V 
B) 0.89 V 
C) -1.78 V 
D) -0.89 V 
E) None of these. 
A) 1.78 V 
B) 0.89 V 
C) -1.78 V 
D) -0.89 V 
E) None of these.

Question 9

The overall reaction 2Co3+(aq)+ 2Cl-(aq)$\to$ 2Co2+(aq)+ Cl2(g)has the standard cell voltage E°cell= 0.46 V.Given E° = 1.36 V for the reaction Cl2(g)+ 2e- $\to$ 2Cl-(aq), calculate the standard reduction potential for the following the half reaction at 25°C: Co3+ + e- $\to$ Co2+

Accepted Answer

A) 1.82 V 
B) -0.90 V 
C) 0.90 V 
D) -1.82 V 
E) -1.36 V 
A) 1.82 V 
B) -0.90 V 
C) 0.90 V 
D) -1.82 V 
E) -1.36 V

Question 10

Consider the reaction Pb(s)+ 2H+(aq)$\to$ Pb2+(aq)+ H2(g). If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II)ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Accepted Answer

A) 2.8 
B) 3.2 
C) 6.0 
D) 3.0 
E) 5.7 
A) 2.8 
B) 3.2 
C) 6.0 
D) 3.0 
E) 5.7

Question 11

Calculate E°cell for a silver-aluminum cell in which the cell reaction is Al(s)+ 3Ag+(aq)$\to$Al3+(aq)+ 3Ag(s)

Accepted Answer

A) -2.46 V 
B) 0.86 V 
C) -0.86 V 
D) 2.46 V 
E) none of these 
A) -2.46 V 
B) 0.86 V 
C) -0.86 V 
D) 2.46 V 
E) none of these

Question 12

Will H2(g)form when Fe is placed in 1.0 M HCl?

Accepted Answer

Question 13

Using a table of standard reduction potentials, determine which of these reactions (if any)is/are nonspontaneous in the direction indicated at 25°C.

Accepted Answer

A) 2Fe3+ + 2Cl- $\to$ 2Fe2+ + Cl2(g) 
B) 2Fe3+ + 2Br- $\to$ 2Fe2+ + Br2(l) 
C) 2Fe3+ + 2I- $\to$ 2Fe2+ + I2(s) 
D) A and B 
E) All are spontaneous. 
A) 2Fe3+ + 2Cl- $\to$ 2Fe2+ + Cl2(g) 
B) 2Fe3+ + 2Br- $\to$ 2Fe2+ + Br2(l) 
C) 2Fe3+ + 2I- $\to$ 2Fe2+ + I2(s) 
D) A and B 
E) All are spontaneous.

Question 14

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl2(g)is evolved at the anode.

Accepted Answer

A) True 
 B)False

Question 15

The reduction of 1.00 mole of Cr3+ to Cr requires 9.65 $\times$ 104 C of electrical charge.

Accepted Answer

A) True 
 B)False

Question 16

Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

Accepted Answer

A) Pb 
B) Fe 
C) Zn 
D) Na 
E) Ag 
A) Pb 
B) Fe 
C) Zn 
D) Na 
E) Ag

Question 17

Using a table of standard electrode potentials, decide which of the following statements is completely true.

Accepted Answer

A) Cu2+ can oxidize H2, and Fe can reduce Mn2+. 
B) Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+. 
C) Fe2+ can oxidize H2, and Fe2+ can reduce Au3+. 
D) Br2 can oxidize Ni, and H2 can reduce Mn2+. 
E) H+ can oxidize Fe, and Ni can reduce Br2. 
A) Cu2+ can oxidize H2, and Fe can reduce Mn2+. 
B) Ni2+ can oxidize Cu2+, and Fe2+ can reduce H+. 
C) Fe2+ can oxidize H2, and Fe2+ can reduce Au3+. 
D) Br2 can oxidize Ni, and H2 can reduce Mn2+. 
E) H+ can oxidize Fe, and Ni can reduce Br2.

Question 18

Complete and balance the following redox equation. What is the coefficient of OH- when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + I- $\to$  MnO2 + IO3- (basic solution)

Accepted Answer

A) 1 
B) 2 
C) 4 
D) 10 
E) None of these. 
A) 1 
B) 2 
C) 4 
D) 10 
E) None of these.

Question 19

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours. How many moles of calcium metal should be deposited?

Accepted Answer

A) 5.83 $\times$ 10-5 mol 
B) 0.210 mol 
C) 0.420 mol 
D) 0.840 mol 
E) 1.95 $\times$ 109 mol 
A) 5.83 $\times$ 10-5 mol 
B) 0.210 mol 
C) 0.420 mol 
D) 0.840 mol 
E) 1.95 $\times$ 109 mol

Question 20

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H2(g, 1.0 atm)+ 2Ag+(aq, 1.0 M)$\to$2H+(aq, pH = ?)+ 2Ag(s)
Calculate the pH of the H+(aq)solution.

Accepted Answer

A) 1.4 
B) 2.7 
C) 5.4 
D) 7.1 
E) 14.9 
A) 1.4 
B) 2.7 
C) 5.4 
D) 7.1 
E) 14.9

Exam 19: Electrochemistry

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

Will H2(g)form when Cu is placed in 1.0 M HCl?

For the electrochemical cell Ni(s)| Ni2+(1 M)|| H+(1 M)| H2(1 atm)| Pt(s), which one of the following changes will cause a decrease in the cell voltage?

Which one of the following reagents is capable of transforming Br- (aq)to Br2(l)under standard-state conditions?

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

Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq)|| Cl2(g), Cl- (aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu4+/Pu3+)?

Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br- (aq)+ I2(s) Br2(l)+ 2I- (aq)

For the reaction, 2Cr2+ + Cl2(g) →\to→ 2Cr3+ + 2Cl-, E°cell is 1.78 V.Calculate E°cell for the related reaction Cr3+ + Cl- →\to→ Cr2+ + 1/2Cl2(g).

The overall reaction 2Co3+(aq)+ 2Cl-(aq) →\to→ 2Co2+(aq)+ Cl2(g)has the standard cell voltage E°cell= 0.46 V.Given E° = 1.36 V for the reaction Cl2(g)+ 2e- →\to→ 2Cl-(aq), calculate the standard reduction potential for the following the half reaction at 25°C: Co3+ + e- →\to→ Co2+

Consider the reaction Pb(s)+ 2H+(aq) →\to→ Pb2+(aq)+ H2(g). If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II)ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Calculate E°cell for a silver-aluminum cell in which the cell reaction is Al(s)+ 3Ag+(aq) →\to→ Al3+(aq)+ 3Ag(s)

Will H2(g)form when Fe is placed in 1.0 M HCl?

Using a table of standard reduction potentials, determine which of these reactions (if any)is/are nonspontaneous in the direction indicated at 25°C.

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl2(g)is evolved at the anode.

The reduction of 1.00 mole of Cr3+ to Cr requires 9.65 ×\times× 104 C of electrical charge.

Which of these metals will reduce water to hydrogen in basic solution under standard conditions?

Using a table of standard electrode potentials, decide which of the following statements is completely true.

Complete and balance the following redox equation. What is the coefficient of OH- when the equation is balanced using the set of smallest whole-number coefficients? MnO4- + I- →\to→ MnO2 + IO3- (basic solution)

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl2 for 4.50 hours. How many moles of calcium metal should be deposited?

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H2(g, 1.0 atm)+ 2Ag+(aq, 1.0 M) →\to→ 2H+(aq, pH = ?)+ 2Ag(s) Calculate the pH of the H+(aq)solution.

Chemistry: The Study of Change

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Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

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Quantum Theory and the Electronic Structure of Atoms

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Chemical Bonding I: Basic Concepts

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Physical Properties of Solutions

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Filters

Will H₂(g)form when Cu is placed in 1.0 M HCl?

For the electrochemical cell Ni(s)| Ni²⁺(1 M)|| H⁺(1 M)| H₂(1 atm)| Pt(s), which one of the following changes will cause a decrease in the cell voltage?

Which one of the following reagents is capable of transforming Br^-(aq)to Br₂(l)under standard-state conditions?

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

Consider an electrochemical cell based on the following cell diagram: Pt | Pu³⁺(aq), Pu⁴⁺(aq)|| Cl₂(g), Cl^-(aq)| Pt Given that the standard cell emf is 0.35 V and that the standard reduction potential of chlorine is 1.36 V, what is the standard reduction potential E°(Pu⁴⁺/Pu³⁺)?

Determine the equilibrium constant, K_eq, at 25°C for the reaction 2Br^-(aq)+ I₂(s) Br₂(l)+ 2I^-(aq)

For the reaction, 2Cr²⁺ + Cl₂(g) $\to$ 2Cr³⁺ + 2Cl^-, E°_cell is 1.78 V.Calculate E°_cell for the related reaction Cr³⁺ + Cl^- $\to$ Cr²⁺ + ¹/₂Cl₂(g).

Consider the reaction Pb(s)+ 2H⁺(aq) $\to$ Pb²⁺(aq)+ H₂(g). If the hydrogen gas pressure is maintained at 1.00 atm and the lead(II)ion concentration is 0.025 M, find the pH at which this reaction is at equilibrium.

Calculate E°_cell for a silver-aluminum cell in which the cell reaction is Al(s)+ 3Ag⁺(aq) $\to$ Al³⁺(aq)+ 3Ag(s)

Will H₂(g)form when Fe is placed in 1.0 M HCl?

When an aqueous solution of NaCl is electrolyzed, Na(l)is produced at the cathode, and Cl₂(g)is evolved at the anode.

The reduction of 1.00 mole of Cr³⁺ to Cr requires 9.65 $\times$ 10⁴ C of electrical charge.

Complete and balance the following redox equation. What is the coefficient of OH^-when the equation is balanced using the set of smallest whole-number coefficients? MnO₄^- + I^- $\to$ MnO₂ + IO₃^- (basic solution)

A current of 2.50 A was passed through an electrolytic cell containing molten CaCl₂ for 4.50 hours. How many moles of calcium metal should be deposited?

The measured voltage of a cell in which the following reaction occurs is 0.96 V: H₂(g, 1.0 atm)+ 2Ag⁺(aq, 1.0 M) $\to$ 2H⁺(aq, pH = ?)+ 2Ag(s) Calculate the pH of the H⁺(aq)solution.