Question 1

Using the standard reduction potentials in Table 17.2 to calculate the equilibrium constant for the reaction
Fe3+ (aq)  + V2+ (aq)  → Fe2+ (aq)  + V3+ (aq) 
At a temperature of 298 K.

Accepted Answer

A)   1.3 × 1040
B)   3.8 × 10-18
C)   2.6 × 1017
D)   4.2 × 108E) B) and C)
F) All of the above

Question 2

The conductivity of an aqueous solution of ammonium sulphate, (NH4) 2SO4 (aq)  is 0.316 S m-1. Calculate the concentration of the solution.

Accepted Answer

A)   0.0110 mol dm-3
B)   0.0148 mol dm-3
C)   0.0091 mol dm-3
D)   0.0898 mol dm-3E) A) and B)
F) B) and C)

Question 3

Calculate the standard cell potential for the reaction
2 MnO4-(aq)  + 5 Sn2+ (aq)  + 16 H+ (aq)  → 2 Mn2+ (aq)  + 5 Sn4+ (aq)  + 8 H2O
At a temperature of 298 K.

Accepted Answer

A)   -1.57 V
B)   +1.37 V
C)   +3.14 V
D)   +2.29 VE) A) and B)
F) A) and D)

Question 4

Use the data for the standard reduction potentials given in Table 17.2 to predict which of the following is the strongest oxidising agent in acidic solution: OCl- (aq) , Cr2O7- (aq) , H2O2 (aq)  or MnO4- (aq)

Accepted Answer

A)   OCl- (aq) 
B)   Cr2O7- (aq) 
C)   H2O2 (aq) 
D)   MnO4- (aq) E) A) and C)
F) B) and C)

Question 5

The position of equilibrium for the cell
Cr2O72- (aq)  + 6 Fe2+(aq)  + 14 H+(aq)  → 2 Cr3+ (aq)  + 6 Fe3+ (aq)  + 7 H2O (l) 
Favours the formation of products. Identify the half-cell processes that occur at the anode and cathode.

Accepted Answer

A)   Cathode: Cr2O72-/Cr3+ Anode: Fe3+/Fe2+
B)   Cathode: Cr3+/Cr2+ Anode: Fe3+/Fe
C)   Cathode: Fe3+/Fe Anode: Cr3+/Cr2+
D)   Cathode: Fe3+/Fe2+ Anode: Cr2O72-/Cr3+E) B) and D)
F) A) and B)

Question 6

Calculate the standard cell potential for the reaction
3 Zn(s)  + Cr2O72− (aq)  + 14 H+ (aq)  → 3 Zn2+ (aq)  + 2Cr3+ (aq)  + 7 H2O (l) 
At a temperature of 298 K.

Accepted Answer

A)   -0.57 V
B)   +1.37 V
C)   +3.61 V
D)   +2.09 VE) C) and D)
F) B) and D) D

Question 7

Determine the change in standard Gibbs energy at 298 K for the reaction
PbO2 (s)  + Pb (s)  + 2 H2SO4 (aq)  → 2 PbSO4 (aq)  + 2 H2O (l) 
Which this basis of the lead-acid battery.

Accepted Answer

A)   -394 kJ mol-1
B)   -197 kJ mol-1
C)   -163 kJ mol-1
D)   -201 kJ mol-1E) B) and D)
F) A) and D)

Question 8

What is the best description of the following reaction?
PbO2 (s)  + H2O (l)  + 2 e- → PbO (s)  + 2 OH- (aq)

Accepted Answer

A)   Oxidation of PbO2
B)   Hydrolysis of PbO2
C)   Reduction of PbO2
D)   disproportionation of PbO2E) A) and C)
F) B) and D)

Question 9

By considering the standard reduction potentials given in Table 7.2, decide which of the following metals could be used as a sacrificial coating to protect nickel metal, Ni (s) .

Accepted Answer

A)   Copper, Cu (s) 
B)   Magnesium, Mg (s) 
C)   Silver, Ag (s) 
D)   Tin, Sn (s) E) A) and C)
F) B) and C)

Question 10

Determine the limiting molar conductivity of an aqueous solution of ammonium chloride, NH4Cl (aq) .

Accepted Answer

A)   15.0 mS m2 mol-1
B)   22.6 mS m2 mol-1
C)   147.6 mS m2 mol-1
D)   14.8 mS m2 mol-1E) A) and B)
F) B) and C)

Question 11

Determine the limiting molar conductivity of an aqueous solution of magnesium chloride, MgCl2 (aq) .

Accepted Answer

A)   3.0 mS m2 mol-1
B)   18.2 mS m2 mol-1
C)   25.8 mS m2 mol-1
D)   28.8 mS m2 mol-1E) B) and D)
F) All of the above

Question 12

The standard cell potential for the reaction
2Al (s)  + 3Sn2+(aq)  → 2Al3+(aq)  + 3Sn (s) 
Has a value of +1.53 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Accepted Answer

A)   The reaction is spontaneous in the forward direction
B)   The reaction is at equilibrium
C)   The reaction is spontaneous in the backward direction
D)   It is not possible to determine from the standard cell potential alone, whether the reaction will be spontaneousE) A) and D)
F) All of the above

Question 13

Determine the amount of electrical work that can be done by the system in the reaction
Ag+ (aq)  + Fe2+ (aq)  → Fe3+ (aq)  + Ag (s) 
Using the data provided in Table 16.2.

Accepted Answer

A)   -152 kJ mol-1
B)   -32 kJ mol-1
C)   -2.9 kJ mol-1
D)   -28.9 kJ mol-1E) C) and D)
F) None of the above

Question 14

Use the standard reduction potentials for the Ag(s) /AgCl(s)  and Ag+(aq) /Ag(s)  half cells in Table 16.2 to determine the solubility product of silver chloride, AgCl, at 298 K.

Accepted Answer

A)   1.8  1017
B)   5.6  10-10
C)   6.4  109
D)   1.6  10-10E) B) and C)
F) A) and C)

Question 15

The standard cell potential for the reaction
6 [Fe(CN) 6]3- (aq)  + 2 Cr3+ (aq)  + 7 H2O (aq)  → Cr2O72- (aq)  + 14 H+ + 6 [Fe(CN) 6]4- (aq) 
Has a value of -0.97 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Accepted Answer

A)   The reaction is spontaneous in the forward direction
B)   The reaction is at equilibrium
C)   The reaction is spontaneous in the backward direction
D)   It is not possible to determine from the standard cell potential alone, whether the reaction will be spontaneousE) All of the above
F) C) and D)

Question 16

Use the Nernst equation to calculate the cell potential for the cell
Al (s)  | Al3+ (aq, c = 0.20 mol dm-3)  ║ Cu2+ (aq, c = 0.10 mol dm-3)  | Cu (s) 
At a temperature of 298 K.

Accepted Answer

A)   +1.98 V
B)   +2.02 V
C)   +0.02 V
D)   +2.00 VE) A) and D)
F) C) and D)

Question 17

A concentration cell is formed by dipping two copper, Cu (s)  electrodes into copper sulfate, CuSO4 (aq) , solutions of different concentrations, and joining the half cells by a salt bridge. Determine the ratio of the concentrations of the copper sulfate solutions necessary to create a potential difference between the electrodes of 0.10 V.

Accepted Answer

A)   2400
B)   10
C)   6.1  107
D)   1300E) B) and C)
F) A) and D) A

Question 18

The standard Gibbs energy change for the reaction
H+ (aq)  + OH- (aq)  → H2O (l) 
Is -80.1 kJ mol-1 at 298 K. Determine the standard reaction potential for the cell
Pt (s)  | O2 (g)  | H+ (aq)  ║ OH- (aq)  | O2 (g)  | Pt (s) 
At this temperature.

Accepted Answer

A)   +0.83 V
B)   +3.32 V
C)   +0.21 V
D)   +0.19 VE) A) and B)
F) A) and C) A

Question 19

Determine the standard cell potential at 298 K for the reaction
2 OH- (aq)  + Cl2 (g)  → Cl- (aq)  + OCl- (aq)  + H2O (l) 
Using the data for the standard reduction potentials in Table 17.2.

Accepted Answer

A)   +0.47 V
B)   -0.94 V
C)   +2.25 V
D)   0.00 VE) None of the above
F) B) and C)

Question 20

Determine the amount of electrical work that can be done by the system in the reaction
Cu (s)  + Zn2+ (aq)  → Cu2+ (aq)  + Zn (s) 
For which

Accepted Answer

A)   -212 kJ mol-1
B)   -106 kJ mol-1
C)   -54 kJ mol-1
D)   -2.20 kJ mol-1E) A) and C)
F) B) and C)

Exam 16: Electrochemistry

Using the standard reduction potentials in Table 17.2 to calculate the equilibrium constant for the reaction Fe³⁺(aq) + V²⁺ (aq) → Fe²⁺(aq) + V³⁺ (aq) At a temperature of 298 K.

Correct Answer
verified

The conductivity of an aqueous solution of ammonium sulphate, (NH₄) ₂SO₄ (aq) is 0.316 S m^-1. Calculate the concentration of the solution.

Correct Answer
verified

Calculate the standard cell potential for the reaction 2 MnO₄^-(aq) + 5 Sn²⁺ (aq) + 16 H⁺ (aq) → 2 Mn²⁺ (aq) + 5 Sn⁴⁺ (aq) + 8 H₂O At a temperature of 298 K.

Correct Answer
verified

Use the data for the standard reduction potentials given in Table 17.2 to predict which of the following is the strongest oxidising agent in acidic solution: OCl^- (aq) , Cr₂O₇^- (aq) , H₂O₂ (aq) or MnO₄^- (aq)

Correct Answer
verified

The position of equilibrium for the cell Cr₂O₇^2- (aq) + 6 Fe²⁺(aq) + 14 H⁺(aq) → 2 Cr³⁺ (aq) + 6 Fe³⁺ (aq) + 7 H₂O (l) Favours the formation of products. Identify the half-cell processes that occur at the anode and cathode.

Correct Answer
verified

Calculate the standard cell potential for the reaction 3 Zn(s) + Cr₂O₇²⁻ (aq) + 14 H⁺ (aq) → 3 Zn²⁺(aq) + 2Cr³⁺ (aq) + 7 H₂O (l) At a temperature of 298 K.

Correct Answer
verified
D

Determine the change in standard Gibbs energy at 298 K for the reaction PbO₂ (s) + Pb (s) + 2 H₂SO₄ (aq) → 2 PbSO₄ (aq) + 2 H₂O (l) Which this basis of the lead-acid battery.

Correct Answer
verified

What is the best description of the following reaction? PbO₂ (s) + H₂O (l) + 2 e^- → PbO (s) + 2 OH^- (aq)

Correct Answer
verified

By considering the standard reduction potentials given in Table 7.2, decide which of the following metals could be used as a sacrificial coating to protect nickel metal, Ni (s) .

Correct Answer
verified

Determine the limiting molar conductivity of an aqueous solution of ammonium chloride, NH₄Cl (aq) .

Correct Answer
verified

Determine the limiting molar conductivity of an aqueous solution of magnesium chloride, MgCl₂ (aq) .

Correct Answer
verified

The standard cell potential for the reaction 2Al (s) + 3Sn²⁺(aq) → 2Al³⁺(aq) + 3Sn (s) Has a value of +1.53 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Correct Answer
verified

Determine the amount of electrical work that can be done by the system in the reaction Ag⁺ (aq) + Fe²⁺ (aq) → Fe³⁺ (aq) + Ag (s) Using the data provided in Table 16.2.

Correct Answer
verified

Use the standard reduction potentials for the Ag(s) /AgCl(s) and Ag⁺(aq) /Ag(s) half cells in Table 16.2 to determine the solubility product of silver chloride, AgCl, at 298 K.

Correct Answer
verified

The standard cell potential for the reaction 6 [Fe(CN) ₆]^3- (aq) + 2 Cr³⁺ (aq) + 7 H₂O (aq) → Cr₂O₇^2- (aq) + 14 H⁺ + 6 [Fe(CN) ₆]^4- (aq) Has a value of -0.97 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Correct Answer
verified

Use the Nernst equation to calculate the cell potential for the cell Al (s) | Al³⁺ (aq, c = 0.20 mol dm^-3) ║ Cu²⁺ (aq, c = 0.10 mol dm^-3) | Cu (s) At a temperature of 298 K.

Correct Answer
verified

Correct Answer
verified
A

The standard Gibbs energy change for the reaction H⁺ (aq) + OH^- (aq) → H₂O (l) Is -80.1 kJ mol^-1 at 298 K. Determine the standard reaction potential for the cell Pt (s) | O₂ (g) | H⁺ (aq) ║ OH^- (aq) | O₂ (g) | Pt (s) At this temperature.

Correct Answer
verified
A

Determine the standard cell potential at 298 K for the reaction 2 OH^- (aq) + Cl₂ (g) → Cl^- (aq) + OCl^- (aq) + H₂O (l) Using the data for the standard reduction potentials in Table 17.2.

Correct Answer
verified

Determine the amount of electrical work that can be done by the system in the reaction Cu (s) + Zn²⁺ (aq) → Cu²⁺ (aq) + Zn (s) For which

Correct Answer
verified

Exam 16: Electrochemistry

Using the standard reduction potentials in Table 17.2 to calculate the equilibrium constant for the reaction Fe3+ (aq) + V2+ (aq) → Fe2+ (aq) + V3+ (aq) At a temperature of 298 K.

Correct AnswerverifiedShow Answer

The conductivity of an aqueous solution of ammonium sulphate, (NH4) 2SO4 (aq) is 0.316 S m-1. Calculate the concentration of the solution.

Correct AnswerverifiedShow Answer

Calculate the standard cell potential for the reaction 2 MnO4-(aq) + 5 Sn2+ (aq) + 16 H+ (aq) → 2 Mn2+ (aq) + 5 Sn4+ (aq) + 8 H2O At a temperature of 298 K.

Correct AnswerverifiedShow Answer

Use the data for the standard reduction potentials given in Table 17.2 to predict which of the following is the strongest oxidising agent in acidic solution: OCl- (aq) , Cr2O7- (aq) , H2O2 (aq) or MnO4- (aq)

Correct AnswerverifiedShow Answer

The position of equilibrium for the cell Cr2O72- (aq) + 6 Fe2+(aq) + 14 H+(aq) → 2 Cr3+ (aq) + 6 Fe3+ (aq) + 7 H2O (l) Favours the formation of products. Identify the half-cell processes that occur at the anode and cathode.

Correct AnswerverifiedShow Answer

Calculate the standard cell potential for the reaction 3 Zn(s) + Cr2O72− (aq) + 14 H+ (aq) → 3 Zn2+ (aq) + 2Cr3+ (aq) + 7 H2O (l) At a temperature of 298 K.

Correct AnswerverifiedD

Determine the change in standard Gibbs energy at 298 K for the reaction PbO2 (s) + Pb (s) + 2 H2SO4 (aq) → 2 PbSO4 (aq) + 2 H2O (l) Which this basis of the lead-acid battery.

Correct AnswerverifiedShow Answer

What is the best description of the following reaction? PbO2 (s) + H2O (l) + 2 e- → PbO (s) + 2 OH- (aq)

Correct AnswerverifiedShow Answer

By considering the standard reduction potentials given in Table 7.2, decide which of the following metals could be used as a sacrificial coating to protect nickel metal, Ni (s) .

Correct AnswerverifiedShow Answer

Determine the limiting molar conductivity of an aqueous solution of ammonium chloride, NH4Cl (aq) .

Correct AnswerverifiedShow Answer

Determine the limiting molar conductivity of an aqueous solution of magnesium chloride, MgCl2 (aq) .

Correct AnswerverifiedShow Answer

The standard cell potential for the reaction 2Al (s) + 3Sn2+(aq) → 2Al3+(aq) + 3Sn (s) Has a value of +1.53 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Correct AnswerverifiedShow Answer

Determine the amount of electrical work that can be done by the system in the reaction Ag+ (aq) + Fe2+ (aq) → Fe3+ (aq) + Ag (s) Using the data provided in Table 16.2.

Correct AnswerverifiedShow Answer

Use the standard reduction potentials for the Ag(s) /AgCl(s) and Ag+(aq) /Ag(s) half cells in Table 16.2 to determine the solubility product of silver chloride, AgCl, at 298 K.

Correct AnswerverifiedShow Answer

The standard cell potential for the reaction 6 [Fe(CN) 6]3- (aq) + 2 Cr3+ (aq) + 7 H2O (aq) → Cr2O72- (aq) + 14 H+ + 6 [Fe(CN) 6]4- (aq) Has a value of -0.97 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Correct AnswerverifiedShow Answer

Use the Nernst equation to calculate the cell potential for the cell Al (s) | Al3+ (aq, c = 0.20 mol dm-3) ║ Cu2+ (aq, c = 0.10 mol dm-3) | Cu (s) At a temperature of 298 K.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedA

The standard Gibbs energy change for the reaction H+ (aq) + OH- (aq) → H2O (l) Is -80.1 kJ mol-1 at 298 K. Determine the standard reaction potential for the cell Pt (s) | O2 (g) | H+ (aq) ║ OH- (aq) | O2 (g) | Pt (s) At this temperature.

Correct AnswerverifiedA

Determine the standard cell potential at 298 K for the reaction 2 OH- (aq) + Cl2 (g) → Cl- (aq) + OCl- (aq) + H2O (l) Using the data for the standard reduction potentials in Table 17.2.

Correct AnswerverifiedShow Answer

Determine the amount of electrical work that can be done by the system in the reaction Cu (s) + Zn2+ (aq) → Cu2+ (aq) + Zn (s) For which

Correct AnswerverifiedShow Answer

Using the standard reduction potentials in Table 17.2 to calculate the equilibrium constant for the reaction Fe³⁺(aq) + V²⁺ (aq) → Fe²⁺(aq) + V³⁺ (aq) At a temperature of 298 K.

Correct Answer
verified

The conductivity of an aqueous solution of ammonium sulphate, (NH₄) ₂SO₄ (aq) is 0.316 S m^-1. Calculate the concentration of the solution.

Correct Answer
verified

Calculate the standard cell potential for the reaction 2 MnO₄^-(aq) + 5 Sn²⁺ (aq) + 16 H⁺ (aq) → 2 Mn²⁺ (aq) + 5 Sn⁴⁺ (aq) + 8 H₂O At a temperature of 298 K.

Correct Answer
verified

Use the data for the standard reduction potentials given in Table 17.2 to predict which of the following is the strongest oxidising agent in acidic solution: OCl^- (aq) , Cr₂O₇^- (aq) , H₂O₂ (aq) or MnO₄^- (aq)

Correct Answer
verified

The position of equilibrium for the cell Cr₂O₇^2- (aq) + 6 Fe²⁺(aq) + 14 H⁺(aq) → 2 Cr³⁺ (aq) + 6 Fe³⁺ (aq) + 7 H₂O (l) Favours the formation of products. Identify the half-cell processes that occur at the anode and cathode.

Correct Answer
verified

Calculate the standard cell potential for the reaction 3 Zn(s) + Cr₂O₇²⁻ (aq) + 14 H⁺ (aq) → 3 Zn²⁺(aq) + 2Cr³⁺ (aq) + 7 H₂O (l) At a temperature of 298 K.

Correct Answer
verified
D

Determine the change in standard Gibbs energy at 298 K for the reaction PbO₂ (s) + Pb (s) + 2 H₂SO₄ (aq) → 2 PbSO₄ (aq) + 2 H₂O (l) Which this basis of the lead-acid battery.

Correct Answer
verified

What is the best description of the following reaction? PbO₂ (s) + H₂O (l) + 2 e^- → PbO (s) + 2 OH^- (aq)

Correct Answer
verified

Correct Answer
verified

Determine the limiting molar conductivity of an aqueous solution of ammonium chloride, NH₄Cl (aq) .

Correct Answer
verified

Determine the limiting molar conductivity of an aqueous solution of magnesium chloride, MgCl₂ (aq) .

Correct Answer
verified

The standard cell potential for the reaction 2Al (s) + 3Sn²⁺(aq) → 2Al³⁺(aq) + 3Sn (s) Has a value of +1.53 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Correct Answer
verified

Determine the amount of electrical work that can be done by the system in the reaction Ag⁺ (aq) + Fe²⁺ (aq) → Fe³⁺ (aq) + Ag (s) Using the data provided in Table 16.2.

Correct Answer
verified

Use the standard reduction potentials for the Ag(s) /AgCl(s) and Ag⁺(aq) /Ag(s) half cells in Table 16.2 to determine the solubility product of silver chloride, AgCl, at 298 K.

Correct Answer
verified

The standard cell potential for the reaction 6 [Fe(CN) ₆]^3- (aq) + 2 Cr³⁺ (aq) + 7 H₂O (aq) → Cr₂O₇^2- (aq) + 14 H⁺ + 6 [Fe(CN) ₆]^4- (aq) Has a value of -0.97 V at 298 K. Predict whether the reaction, as written, will be spontaneous in the forward direction at this temperature.

Correct Answer
verified

Use the Nernst equation to calculate the cell potential for the cell Al (s) | Al³⁺ (aq, c = 0.20 mol dm^-3) ║ Cu²⁺ (aq, c = 0.10 mol dm^-3) | Cu (s) At a temperature of 298 K.

Correct Answer
verified

Correct Answer
verified
A

The standard Gibbs energy change for the reaction H⁺ (aq) + OH^- (aq) → H₂O (l) Is -80.1 kJ mol^-1 at 298 K. Determine the standard reaction potential for the cell Pt (s) | O₂ (g) | H⁺ (aq) ║ OH^- (aq) | O₂ (g) | Pt (s) At this temperature.

Correct Answer
verified
A

Determine the standard cell potential at 298 K for the reaction 2 OH^- (aq) + Cl₂ (g) → Cl^- (aq) + OCl^- (aq) + H₂O (l) Using the data for the standard reduction potentials in Table 17.2.

Correct Answer
verified

Determine the amount of electrical work that can be done by the system in the reaction Cu (s) + Zn²⁺ (aq) → Cu²⁺ (aq) + Zn (s) For which

Correct Answer
verified