Question 1

The more ________ the value of E°red, the greater the driving force for reduction.

Accepted Answer

A) positive 
B) negative 
C) exothermic 
D) endothermic 
E) extensive 
A) positive 
B) negative 
C) exothermic 
D) endothermic 
E) extensive

Question 2

Which substance is serving as the oxidizing agent in the following reaction? 14H+ + Cr2O72- + 3Ni → 3Ni2+ + 2Cr3+ + 7H2O

Accepted Answer

A) Ni 
B) H+ 
C) Cr2O72- 
D) H2O 
E) Ni2+ 
A) Ni 
B) H+ 
C) Cr2O72- 
D) H2O 
E) Ni2+

Question 3

The standard cell potential (E°cell)of the reaction below is +0.126 V. The value of ΔG° for the reaction is ________ kJ/mol. Pb (s) + 2H+(aq) → Pb2+ (aq) + H2 (g)

Accepted Answer

A) -24.3 
B) +24.3 
C) -12.6 
D) +12.6 
E) -50.8 
A) -24.3 
B) +24.3 
C) -12.6 
D) +12.6 
E) -50.8

Question 4

Which element is oxidized in the reaction below? I- + MnO4- + H+ → I2 + MnO2 + cO

Accepted Answer

A) I 
B) Mn 
C) O 
D) H 
A) I 
B) Mn 
C) O 
D) H

Question 5

What is the cathode in the hydrogen fuel cell?

Accepted Answer

A) O2 
B) KOH 
C) Li 
D) H2 
E) Pt 
A) O2 
B) KOH 
C) Li 
D) H2 
E) Pt

Question 6

Which of the following reactions is a redox reaction? (a) K2CrO4 + BaCl2 → BaCrO4  + 2KCl
(b) Pb22+ + 2Br- → PbBr
(c) Cu + S → CuS

Accepted Answer

A) (a)only 
B) (b)only 
C) (c)only 
D) (a)and (c) 
E) (b)and (c) 
A) (a)only 
B) (b)only 
C) (c)only 
D) (a)and (c) 
E) (b)and (c)

Question 7

The most difficult species to reduce and the poorest oxidizing agent is ________.

Accepted Answer

The answer of The most difficult species to reduce and...

Question 8

________ is the reducing agent in the reaction below. Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O

Accepted Answer

A) Cr2O72- 
B) S2O32- 
C) H+ 
D) Cr3+ 
E) S4O62- 
A) Cr2O72- 
B) S2O32- 
C) H+ 
D) Cr3+ 
E) S4O62-

Question 9

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)
With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.53 V. The concentration of H+ in the cathode compartment is ________ M.

Accepted Answer

A) 1.3 × 10-4 
B) 1.7 × 10-8 
C) 1.1 × 10-2 
D) 7.7 × 103  
E) 1.3 × 10-11 
A) 1.3 × 10-4 
B) 1.7 × 10-8 
C) 1.1 × 10-2 
D) 7.7 × 103  
E) 1.3 × 10-11

Question 10

The standard cell potential (E° cell)for the reaction below is +0.63 V. The cell potential for this reaction is ________ V when [ Zn2+] = 3.0 M and [Pb2+] = 2.0 × 10-4 M. Pb2+ (aq) + Zn (s) → Zn2+ (aq) + Pb (s)

Accepted Answer

A) 0.51 
B) 0.86 
C) 0.40 
D) 0.75 
E) 0.63 
A) 0.51 
B) 0.86 
C) 0.40 
D) 0.75 
E) 0.63

Question 11

The half-reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO4- (aq) + 24H+ (aq) + 5Fe (s) → 3Mn2+ (aq) + 5Fe3+ (aq) + 12H2O (l)

Accepted Answer

A) MnO4- (aq) + 8H+ (aq) + 5   → Mn2+ (aq) + 4H2O (l) 
B) 2MnO4- (aq) + 12H+ (aq) + 6e- → 2Mn2+ (aq) + 3H2O (l) 
C) Fe (s) → Fe3+ (aq) + 3e- 
D) Fe (s) → Fe2+ (aq) + 2e- 
E) Fe2+ (aq) → Fe3+ (aq) + e- 
A) MnO4- (aq) + 8H+ (aq) + 5   → Mn2+ (aq) + 4H2O (l) 
B) 2MnO4- (aq) + 12H+ (aq) + 6e- → 2Mn2+ (aq) + 3H2O (l) 
C) Fe (s) → Fe3+ (aq) + 3e- 
D) Fe (s) → Fe2+ (aq) + 2e- 
E) Fe2+ (aq) → Fe3+ (aq) + e-

Question 12

Table 20.1
Half Reaction E°(V)
FS1U1B12S1U1B0 (g) + 2eS1U1P1-S1S1P0 → 2FS1U1P1-S1S1P0 (aq)+2.87
ClS1U1B12S1U1B0 (g) + 2eS1U1P1-S1S1P0 → 2ClS1U1P1-S1S1P0 (aq)+1.359
BrS1U1B12S1U1B0 (l) + 2eS1U1P1-S1S1P0 → 2BrS1U1P1-S1S1P0 (aq)+1.065
OS1U1B12S1U1B0 (g) + 4HS1U1P1+S1S1P0 (aq) + 4eS1U1P1-S1S1P0 → 2HS1U1B12S1U1B0O (l) +1.23
AgS1U1P1+S1S1P0 + eS1U1P1-S1S1P0 → Ag (s)+0.799
FeS1U1P13S1S1P0S1U1P1+S1S1P0 (aq) + eS1U1P1-S1S1P0 → FeS1U1P12+S1S1P0 (aq)+0.771
IS1U1B12S1U1B0 (s) + 2eS1U1P1-S1S1P0 → 2IS1U1P1-S1S1P0 (aq)+0.536
CuS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Cu (s)+0.34
2HS1U1P1+S1S1P0 + 2eS1U1P1-S1S1P0 → HS1U1B12S1U1B0 (g) 0
PbS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Pb (s)-0.126
NiS1U1P12+S1S1P0 + 2eS1U1P1-S1S1P0 → Ni (s)-0.28
LiS1U1P1+S1S1P0 + eS1U1P1-S1S1P0 → Li (s)-3.05
-Which one of the following is the best oxidizing agent?

Accepted Answer

A) H2 
B) Na 
C) O2 
D) Li 
E) Ca 
A) H2 
B) Na 
C) O2 
D) Li 
E) Ca

Question 13

Which one of the following reactions is a redox reaction?

Accepted Answer

A) NaOH + HCl → NaCl + H2O 
B) Pb2+ + 2Cl- → PbCl2 
C) AgNO3 + HCl → HNO3 + AgCl 
D) None of the above is a redox reaction. 
A) NaOH + HCl → NaCl + H2O 
B) Pb2+ + 2Cl- → PbCl2 
C) AgNO3 + HCl → HNO3 + AgCl 
D) None of the above is a redox reaction.

Question 14

The balanced half-reaction in which dichromate ion is reduced to chromium (III)ion is a ________ process.

Accepted Answer

A) four-electron 
B) twelve-electron 
C) three-electron 
D) six-electron 
E) two-electron 
A) four-electron 
B) twelve-electron 
C) three-electron 
D) six-electron 
E) two-electron

Question 15

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+  + 2e- → Zn (s)E° = -0.763 V
The concentrations of zinc ion in the two compartments are 4.50 M and 1.11 × 10-2 M, respectively. The cell emf is ________ V.

Accepted Answer

A) -1.88 × 10-3 
B) -309 
C) 0.0772 
D) 0.154 
E) -0.761 
A) -1.88 × 10-3 
B) -309 
C) 0.0772 
D) 0.154 
E) -0.761

Question 16

What is the correct coefficient for the electrons in the following half-reaction: Ni6+ + ___e- → Ni

Accepted Answer

A) 6 
B) 1 
C) 2 
D) 3 
E) 5 
A) 6 
B) 1 
C) 2 
D) 3 
E) 5

Question 17

The balanced half-reaction in which chlorine gas is reduced to the aqueous chloride ion is a ________ process.

Accepted Answer

A) one-electron 
B) two-electron 
C) four-electron 
D) three-electron 
E) six-electron 
A) one-electron 
B) two-electron 
C) four-electron 
D) three-electron 
E) six-electron

Question 18

What is the cathode in an alkaline battery?

Accepted Answer

A) MnO2 
B) KOH 
C) Zn powder 
D) Mn2O3 
E) Pt 
A) MnO2 
B) KOH 
C) Zn powder 
D) Mn2O3 
E) Pt

Question 19

What is the coefficient of the dichromate ion when the following equation is balanced? Fe2+ + Cr2O72- → Fe3+ + Cr3+ (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 5 
E) 6 
A) 1 
B) 2 
C) 3 
D) 5 
E) 6

Question 20

The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by ________.

Accepted Answer

A) ΔG =   
B) ΔG =   
C) ΔG = -nFE 
D) ΔG = -nRTF 
E) ΔG =   
A) ΔG =   
B) ΔG =   
C) ΔG = -nFE 
D) ΔG = -nRTF 
E) ΔG =

Exam 20: Electrochemistry

The more ________ the value of E°red, the greater the driving force for reduction.

Which substance is serving as the oxidizing agent in the following reaction? 14H+ + Cr2O72- + 3Ni → 3Ni2+ + 2Cr3+ + 7H2O

The standard cell potential (E°cell)of the reaction below is +0.126 V. The value of ΔG° for the reaction is ________ kJ/mol. Pb (s) + 2H+(aq) → Pb2+ (aq) + H2 (g)

Which element is oxidized in the reaction below? I- + MnO4- + H+ → I2 + MnO2 + cO

What is the cathode in the hydrogen fuel cell?

Which of the following reactions is a redox reaction? (a) K2CrO4 + BaCl2 → BaCrO4 + 2KCl (b) Pb22+ + 2Br- → PbBr (c) Cu + S → CuS

The most difficult species to reduce and the poorest oxidizing agent is ________.

________ is the reducing agent in the reaction below. Cr2O72- + 6S2O32- + 14H+ → 2Cr3+ + 3S4O62- + 7H2O

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g) With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.53 V. The concentration of H+ in the cathode compartment is ________ M.

The standard cell potential (E° cell)for the reaction below is +0.63 V. The cell potential for this reaction is ________ V when [ Zn2+] = 3.0 M and [Pb2+] = 2.0 × 10-4 M. Pb2+ (aq) + Zn (s) → Zn2+ (aq) + Pb (s)

The half-reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO4- (aq) + 24H+ (aq) + 5Fe (s) → 3Mn2+ (aq) + 5Fe3+ (aq) + 12H2O (l)

Which one of the following reactions is a redox reaction?

The balanced half-reaction in which dichromate ion is reduced to chromium (III)ion is a ________ process.

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn (s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 4.50 M and 1.11 × 10-2 M, respectively. The cell emf is ________ V.

What is the correct coefficient for the electrons in the following half-reaction: Ni6+ + ___e- → Ni

The balanced half-reaction in which chlorine gas is reduced to the aqueous chloride ion is a ________ process.

What is the cathode in an alkaline battery?

What is the coefficient of the dichromate ion when the following equation is balanced? Fe2+ + Cr2O72- → Fe3+ + Cr3+ (acidic solution)

The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by ________.

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The more ________ the value of E°_red, the greater the driving force for reduction.

Which substance is serving as the oxidizing agent in the following reaction? 14H⁺ + Cr₂O₇^2- + 3Ni → 3Ni²⁺ + 2Cr³⁺ + 7H₂O

The standard cell potential (E°_cell)of the reaction below is +0.126 V. The value of ΔG° for the reaction is ________ kJ/mol. Pb (s) + 2H⁺(aq) → Pb²⁺ (aq) + H₂ (g)

Which element is oxidized in the reaction below? I^- + MnO₄^- + H⁺ → I₂ + MnO₂ + cO

Which of the following reactions is a redox reaction? (a) K₂CrO₄ + BaCl₂ → BaCrO₄ + 2KCl (b) Pb₂²⁺ + 2Br^- → PbBr (c) Cu + S → CuS

________ is the reducing agent in the reaction below. Cr₂O₇^2- + 6S₂O₃^2- + 14H⁺ → 2Cr³⁺ + 3S₄O₆^2- + 7H₂O

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn (s) + 2H⁺ (aq) → Zn²⁺ (aq) + H₂ (g) With P_H₂ = 1.0 atm and [Zn²⁺] = 1.0 M, the cell potential is 0.53 V. The concentration of H⁺ in the cathode compartment is ________ M.

The standard cell potential (E° cell)for the reaction below is +0.63 V. The cell potential for this reaction is ________ V when [ Zn²⁺] = 3.0 M and [Pb²⁺] = 2.0 × 10^-4 M. Pb²⁺ (aq) + Zn (s) → Zn²⁺ (aq) + Pb (s)

The half-reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO₄^- (aq) + 24H⁺ (aq) + 5Fe (s) → 3Mn²⁺ (aq) + 5Fe³⁺ (aq) + 12H₂O (l)

A voltaic cell is constructed with two Zn²⁺-Zn electrodes, where the half-reaction is Zn²⁺ + 2e^- → Zn (s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 4.50 M and 1.11 × 10^-2 M, respectively. The cell emf is ________ V.

What is the correct coefficient for the electrons in the following half-reaction: Ni⁶⁺ + ___e^- → Ni

What is the coefficient of the dichromate ion when the following equation is balanced? Fe²⁺ + Cr₂O₇^2- → Fe³⁺ + Cr³⁺ (acidic solution)