Question 1

Which of the following is the weakest reducing agent?

Accepted Answer

A)  Al(s) 
B)  F-(aq) 
C)  K(s) 
D)  Al3+(aq) 
E)  Ba2+(aq) 
A)  Al(s) 
B)  F-(aq) 
C)  K(s) 
D)  Al3+(aq) 
E)  Ba2+(aq) B

Question 2

Identify a characteristic that does not describe a standard hydrogen electrode.

Accepted Answer

A)  1 M HCl solution with hydrogen gas 
B)  1 atmosphere 
C)  zinc electrode 
D)  inert platinum electrode 
E)  potential of zero 
A)  1 M HCl solution with hydrogen gas 
B)  1 atmosphere 
C)  zinc electrode 
D)  inert platinum electrode 
E)  potential of zero C

Question 3

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg2+(aq)→ 2 Al3+(aq)+ 3 Mg(s)

Accepted Answer

A)  +4.1 × 102 kJ 
B)  +1.4 × 102 kJ 
C)  -2.3 × 102 kJ 
D)  -7.8 × 102 kJ 
E)  +6.8 × 102 kJ 
A)  +4.1 × 102 kJ 
B)  +1.4 × 102 kJ 
C)  -2.3 × 102 kJ 
D)  -7.8 × 102 kJ 
E)  +6.8 × 102 kJ A

Question 4

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 3 Cl2(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe3+(aq)
Cl2(g)+ 2 e⁻ → 2 Cl⁻(aq)E° = +1.36 V
Fe3+(aq)+ 3 e⁻ → Fe(s)E° = -0.04 V

Accepted Answer

A)  +4.16 V 
B)  -1.40 V 
C)  -1.32 V 
D)  +1.32 V 
E)  +1.40 V 
A)  +4.16 V 
B)  -1.40 V 
C)  -1.32 V 
D)  +1.32 V 
E)  +1.40 V

Question 5

In an alkaline battery,MnO2 is reduced to

Accepted Answer

A)  MnO3. 
B)  Mn2O2. 
C)  MnO(OH). 
D)  MnO4-. 
E)  Mn2O3. 
A)  MnO3. 
B)  Mn2O2. 
C)  MnO(OH). 
D)  MnO4-. 
E)  Mn2O3.

Question 6

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s)∣ Al3+(aq,0.115 M)   Al3+(aq,3.89 M)∣ Al(s)

Accepted Answer

A)  +1.66 V 
B)  +0.060 V 
C)  0.00 V 
D)  +0.090 V 
E)  +0.030 V 
A)  +1.66 V 
B)  +0.060 V 
C)  0.00 V 
D)  +0.090 V 
E)  +0.030 V

Question 7

The gas OF2 can be produced from the electrolysis of an aqueous solution of KF,as shown in the equation below. OF2(g)+ 2 H+(aq)+ 4 e- → H2O(l)+ 2 F-(aq)E° = +2.15 V
Using the given standard reduction potential,calculate the amount of OF2 that is produced,and the electrode at which the OF2 is produced,upon the passage of 0.480 faradays through an aqueous KF solution.

Accepted Answer

A)  6.48 g of OF2 at the anode 
B)  26.0 g of OF2 at the anode 
C)  6.48 g of OF2 at the cathode 
D)  26.0 g of OF2 at the cathode 
A)  6.48 g of OF2 at the anode 
B)  26.0 g of OF2 at the anode 
C)  6.48 g of OF2 at the cathode 
D)  26.0 g of OF2 at the cathode

Question 8

A sacrificial electrode is composed of a metal that

Accepted Answer

A)  does not serve as a protective coating. 
B)  reduces more easily than iron. 
C)  has an oxide that is crumbly when formed. 
D)  oxidizes more easily than iron. 
E)  oxidizes the same as iron. 
A)  does not serve as a protective coating. 
B)  reduces more easily than iron. 
C)  has an oxide that is crumbly when formed. 
D)  oxidizes more easily than iron. 
E)  oxidizes the same as iron.

Question 9

What element is being oxidized in the following redox reaction? C3H8O2(aq)+ K2Cr2O7(aq)→ C3H4O4(aq)+ Cr+3(aq)

Accepted Answer

A)  C 
B)  H 
C)  O 
D)  K 
E)  Cr 
A)  C 
B)  H 
C)  O 
D)  K 
E)  Cr

Question 10

Match between columns Premises: Q = K Q = 1 ΔG° > 0 ΔG° < 0 Q < 1 Q > 1

Accepted Answer

The Answer of ES1U1B1cellS1U1B0 = E°S1U1B1cellS1U1B0 and E°S1U1B1cellS1U1B0 > 0 is...

Question 11

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

Accepted Answer

A)  Sn4+(aq) + Mg(s) 
B)  Cr3+(aq) + Ni(s) 
C)  Zn(s) + Na+(aq) 
D)  Cd(s) + Ba2+(aq) 
E)  None of the above pairs will react. 
A)  Sn4+(aq) + Mg(s) 
B)  Cr3+(aq) + Ni(s) 
C)  Zn(s) + Na+(aq) 
D)  Cd(s) + Ba2+(aq) 
E)  None of the above pairs will react.

Question 12

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Fe and Ag+ in the balanced reaction? Fe(s)+ Ag+(aq)→ Ag(s)+ Fe2+(aq)

Accepted Answer

A)  Fe = 1, Ag⁺ = 2 
B)  Fe = 1, Ag⁺ = 3 
C)  Fe = 2, Ag⁺ = 1 
D)  Fe = 2, Ag⁺ = 3 
E)  Fe = 3, Ag⁺ = 3 
A)  Fe = 1, Ag⁺ = 2 
B)  Fe = 1, Ag⁺ = 3 
C)  Fe = 2, Ag⁺ = 1 
D)  Fe = 2, Ag⁺ = 3 
E)  Fe = 3, Ag⁺ = 3

Question 13

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)  Br2(l) 
B)  Au3+(aq) 
C)  Li(s) 
D)  Cl⁻(aq) 
E)  Cu(s) 
A)  Br2(l) 
B)  Au3+(aq) 
C)  Li(s) 
D)  Cl⁻(aq) 
E)  Cu(s)

Question 14

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni2+(aq)∣∣ Cl2(g)∣ Cl-(aq)∣ C(s)

Accepted Answer

A)  Ni(s) + 2 Cl-(aq) → Ni2+(aq) + Cl2(g) 
B)  Ni(s) + Cl2(g) → Ni2+(aq) + 2 Cl-(aq) 
C)  Ni2+(aq) + 2 Cl-(aq) → Ni(s) + Cl2(g) 
D)  Ni2+(aq) + 2 Cl-(aq) → NiCl2(s) 
A)  Ni(s) + 2 Cl-(aq) → Ni2+(aq) + Cl2(g) 
B)  Ni(s) + Cl2(g) → Ni2+(aq) + 2 Cl-(aq) 
C)  Ni2+(aq) + 2 Cl-(aq) → Ni(s) + Cl2(g) 
D)  Ni2+(aq) + 2 Cl-(aq) → NiCl2(s)

Question 15

Balance the following reaction in KOH.What are the coefficients in front of C9H20O2 and KMnO4 in the balanced reaction? C9H20O2(aq)+ KMnO4(aq)→ C9H14O4K2(aq)+ MnO2(aq)

Accepted Answer

A)  C9H20O2 = 3, KMnO4 = 8 
B)  C9H20O2 = 3, KMnO4 = 4 
C)  C9H20O2 = 8, KMnO4 = 4 
D)  C9H20O2 = 2, KMnO4 = 8 
E)  C9H20O2 = 3, KMnO4 = 2 
A)  C9H20O2 = 3, KMnO4 = 8 
B)  C9H20O2 = 3, KMnO4 = 4 
C)  C9H20O2 = 8, KMnO4 = 4 
D)  C9H20O2 = 2, KMnO4 = 8 
E)  C9H20O2 = 3, KMnO4 = 2

Question 16

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s)∣ Fe3+(aq)   Br2(g)∣ Br⁻(aq)∣ Pt

Accepted Answer

A)  Fe(s) 
B)  Fe3+(aq) 
C)  Br2(g) 
D)  Br⁻(aq) 
E)  Pt 
A)  Fe(s) 
B)  Fe3+(aq) 
C)  Br2(g) 
D)  Br⁻(aq) 
E)  Pt

Question 17

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction? Fe2+(aq)+ MnO4⁻(aq)→ Fe3+(aq)+ Mn2+(aq)

Accepted Answer

A)  H⁺ = 2, Fe3+ = 3 
B)  H⁺ = 8, Fe3+ = 5 
C)  H⁺ = 3, Fe3+ = 2 
D)  H⁺ = 5, Fe3+ = 1 
E)  H⁺ = 8, Fe3+ = 1 
A)  H⁺ = 2, Fe3+ = 3 
B)  H⁺ = 8, Fe3+ = 5 
C)  H⁺ = 3, Fe3+ = 2 
D)  H⁺ = 5, Fe3+ = 1 
E)  H⁺ = 8, Fe3+ = 1

Question 18

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C.(The equation is balanced.) 2 K(s)+ I2(s)→ 2 K⁺(aq)+ 2 I⁻(aq)
K+(aq)+ e⁻ → K(s)E° = -2.93 V
I2(s)+ 2 e⁻ → 2 I⁻(aq)E° = +0.54 V

Accepted Answer

A)  +6.40 V 
B)  +1.85 V 
C)  -5.32 V 
D)  +3.47 V 
E)  +5.32 V 
A)  +6.40 V 
B)  +1.85 V 
C)  -5.32 V 
D)  +3.47 V 
E)  +5.32 V

Question 19

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ e- → Ag(s)+ Cl-(aq)E° = +0.222 V
The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

Accepted Answer

A)  0.212 
B)  0.118 
C)  0.00222 
D)  22.2 
E)  0.232 
A)  0.212 
B)  0.118 
C)  0.00222 
D)  22.2 
E)  0.232

Question 20

What element is being reduced in the following redox reaction? H2O2(l)+ ClO2(aq)→ ClO2⁻(aq)+ O2(g)

Accepted Answer

A)  H 
B)  O 
C)  Cl 
D)  N 
E)  C 
A)  H 
B)  O 
C)  Cl 
D)  N 
E)  C

Exam 19: Electrochemistry

Which of the following is the weakest reducing agent?

Identify a characteristic that does not describe a standard hydrogen electrode.

Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg2+(aq)→ 2 Al3+(aq)+ 3 Mg(s)

In an alkaline battery,MnO2 is reduced to

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s)∣ Al3+(aq,0.115 M) Al3+(aq,3.89 M)∣ Al(s)

A sacrificial electrode is composed of a metal that

What element is being oxidized in the following redox reaction? C3H8O2(aq)+ K2Cr2O7(aq)→ C3H4O4(aq)+ Cr+3(aq)

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C.

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Fe and Ag+ in the balanced reaction? Fe(s)+ Ag+(aq)→ Ag(s)+ Fe2+(aq)

Which of the following is the strongest oxidizing agent?

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni2+(aq)∣∣ Cl2(g)∣ Cl-(aq)∣ C(s)

Balance the following reaction in KOH.What are the coefficients in front of C9H20O2 and KMnO4 in the balanced reaction? C9H20O2(aq)+ KMnO4(aq)→ C9H14O4K2(aq)+ MnO2(aq)

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s)∣ Fe3+(aq) Br2(g)∣ Br⁻(aq)∣ Pt

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction? Fe2+(aq)+ MnO4⁻(aq)→ Fe3+(aq)+ Mn2+(aq)

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ e- → Ag(s)+ Cl-(aq)E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

What element is being reduced in the following redox reaction? H2O2(l)+ ClO2(aq)→ ClO2⁻(aq)+ O2(g)

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Use the tabulated half-cell potentials to calculate ΔG° for the following redox reaction. 2 Al(s)+ 3 Mg²⁺(aq)→ 2 Al³⁺(aq)+ 3 Mg(s)

In an alkaline battery,MnO₂ is reduced to

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s)∣ Al³⁺(aq,0.115 M) Al³⁺(aq,3.89 M)∣ Al(s)

What element is being oxidized in the following redox reaction? C₃H₈O₂(aq)+ K₂Cr₂O₇(aq)→ C₃H₄O₄(aq)+ Cr⁺³(aq)

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Fe and Ag⁺ in the balanced reaction? Fe(s)+ Ag⁺(aq)→ Ag(s)+ Fe²⁺(aq)

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)∣ Ni²⁺(aq)∣∣ Cl₂(g)∣ Cl^-(aq)∣ C(s)

Balance the following reaction in KOH.What are the coefficients in front of C₉H₂₀O₂ and KMnO₄ in the balanced reaction? C₉H₂₀O₂(aq)+ KMnO₄(aq)→ C₉H₁₄O₄K₂(aq)+ MnO₂(aq)

What is undergoing oxidation in the redox reaction represented by the following cell notation? Fe(s)∣ Fe³⁺(aq) Br₂(g)∣ Br⁻(aq)∣ Pt

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H⁺and Fe³⁺ in the balanced reaction? Fe²⁺(aq)+ MnO₄⁻(aq)→ Fe³⁺(aq)+ Mn²⁺(aq)

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is AgCl(s)+ e^- → Ag(s)+ Cl^-(aq)E° = +0.222 V The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M,respectively.The cell emf is ________ V.

What element is being reduced in the following redox reaction? H₂O₂(l)+ ClO₂(aq)→ ClO₂⁻(aq)+ O₂(g)