Question 1

Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. 3 I2(s)+ 2 Fe(s)→ 2 Fe3+(aq)+ 6 I⁻(aq)

Accepted Answer

A)  -1.1 × 102 kJ 
B)  +4.9 × 101 kJ 
C)  -9.7 × 101 kJ 
D)  +2.3 × 102 kJ 
E)  -3.3 × 102 kJ 
A)  -1.1 × 102 kJ 
B)  +4.9 × 101 kJ 
C)  -9.7 × 101 kJ 
D)  +2.3 × 102 kJ 
E)  -3.3 × 102 kJ

Question 2

Determine the redox reaction represented by the following cell notation. Fe(s)∣ Fe2+(aq)   Cu2+(aq)∣ Cu(s)

Accepted Answer

A)  Cu(s) + Fe2+(aq) → Fe(s) + Cu2+(aq) 
B)  Fe(s) + Cu2+(aq) → Cu(s) + Fe2+(aq) 
C)  2 Fe(s) + Cu2+(aq) → Cu(s) + 2 Fe2+(aq) 
D)  2 Cu(s) + Fe2+(aq) → Fe(s) + 2 Cu2+(aq) 
E)  3 Fe(s) + 2 Cu2+(aq) → 2 Cu(s) + 3 Fe2+(aq) 
A)  Cu(s) + Fe2+(aq) → Fe(s) + Cu2+(aq) 
B)  Fe(s) + Cu2+(aq) → Cu(s) + Fe2+(aq) 
C)  2 Fe(s) + Cu2+(aq) → Cu(s) + 2 Fe2+(aq) 
D)  2 Cu(s) + Fe2+(aq) → Fe(s) + 2 Cu2+(aq) 
E)  3 Fe(s) + 2 Cu2+(aq) → 2 Cu(s) + 3 Fe2+(aq)

Question 3

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten   with an applied emf of 4.50 V?

Accepted Answer

A)  0.0336 
B)  0.0298 
C)  7.4 
D)  29.8 
E)  14.9 
A)  0.0336 
B)  0.0298 
C)  7.4 
D)  29.8 
E)  14.9

Question 4

Identify the battery that is used as a common flashlight battery.

Accepted Answer

A)  dry-cell battery 
B)  lithium ion battery 
C)  lead-acid storage battery 
D)  NiCad battery 
E)  fuel cell 
A)  dry-cell battery 
B)  lithium ion battery 
C)  lead-acid storage battery 
D)  NiCad battery 
E)  fuel cell

Question 5

What is the reducing agent in the redox reaction represented by the following cell notation? Ba(s)∣ Ba2+(aq)   Li+(aq)∣ Li(s)

Accepted Answer

A)  Ba(s) 
B)  Ba2+(aq) 
C)  Li+(aq) 
D)  Li(s) 
E)  Pt 
A)  Ba(s) 
B)  Ba2+(aq) 
C)  Li+(aq) 
D)  Li(s) 
E)  Pt

Question 6

In a dry-cell 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 7

What element is being oxidized in the following redox reaction? Mg2+(aq)+ NH4+(aq)→ Mg(s)+ NO3⁻(aq)

Accepted Answer

A)  Mg 
B)  N 
C)  H 
D)  O 
A)  Mg 
B)  N 
C)  H 
D)  O

Question 8

Given that E°red = -0.40 V for Cd2+/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s)∣ Cd2+(1.0 × 10-5 M)∣∣ Cd2+(0.100 M)∣ Cd(s)

Accepted Answer

A)  E° = 0.00 V and E = +0.24 V 
B)  E° = 0.00 V and E = +0.12 V 
C)  E° = -0.40 V and E = -0.16 V 
D)  E° = -0.40 V and E = -0.28 V 
A)  E° = 0.00 V and E = +0.24 V 
B)  E° = 0.00 V and E = +0.12 V 
C)  E° = -0.40 V and E = -0.16 V 
D)  E° = -0.40 V and E = -0.28 V

Question 9

What is the oxidizing agent in the redox reaction represented by the following cell notation? Mn(s)∣ Mn2+(aq)   K+(aq)∣ K(s)

Accepted Answer

A)  Mn(s) 
B)  Mn2+(aq) 
C)  K+(aq) 
D)  K(s) 
E)  Pt 
A)  Mn(s) 
B)  Mn2+(aq) 
C)  K+(aq) 
D)  K(s) 
E)  Pt

Question 10

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(l)
Sn(s)→ Sn2+(aq)+ 2 e-
How many moles of Sn(s)are oxidized by four moles of Cr2O72-?

Accepted Answer

A)  4 
B)  8 
C)  12 
D)  24 
A)  4 
B)  8 
C)  12 
D)  24

Question 11

Identify the components of a fuel cell.

Accepted Answer

A)  nickel-metal hydride 
B)  lithium ion 
C)  hydrogen-oxygen 
D)  nickel-cadmium 
E)  zinc-manganese 
A)  nickel-metal hydride 
B)  lithium ion 
C)  hydrogen-oxygen 
D)  nickel-cadmium 
E)  zinc-manganese

Question 12

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s)∣ Sn2+(aq,1.8 M)   Ag+(aq,0.055 M)∣ Ag(s)

Accepted Answer

A)  -0.94 V 
B)  -0.85 V 
C)  +1.02 V 
D)  +0.98 V 
E)  +0.86 V 
A)  -0.94 V 
B)  -0.85 V 
C)  +1.02 V 
D)  +0.98 V 
E)  +0.86 V

Question 13

Based on the following information, I2(s)+ 2 e- → 2 I-(aq)E° = +0.54 V
Cd2+(aq)+ 2 e- → Cd (s)E° = -0.40 V
Which of the following chemical species is the strongest reducing agent?

Accepted Answer

A)  I2(s) 
B)  Cd2+(aq) 
C)  I-(aq) 
D)  Cd(s) 
A)  I2(s) 
B)  Cd2+(aq) 
C)  I-(aq) 
D)  Cd(s)

Question 14

Why are iron nails coated with zinc?

Accepted Answer

Zinc is more easily oxidized t

Question 15

In a nickel-metal hydride battery,NiO(OH)is reduced to

Accepted Answer

A)  Ni(OH)4. 
B)  NiO2. 
C)  Ni. 
D)  Ni(OH)2. 
E)  NiOH. 
A)  Ni(OH)4. 
B)  NiO2. 
C)  Ni. 
D)  Ni(OH)2. 
E)  NiOH.

Question 16

What element is being reduced in the following redox reaction? MnO4⁻(aq)+ H2C2O4(aq)→ Mn2+(aq)+ CO2(g)

Accepted Answer

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

Question 17

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

Accepted Answer

A)  Pb2+(aq) + Au(s) 
B)  Ag+(aq) + Br⁻(aq) 
C)  Na+(aq) + Al(s) 
D)  Fe3+(aq) + Al(s) 
E)  None of the above pairs will react. 
A)  Pb2+(aq) + Au(s) 
B)  Ag+(aq) + Br⁻(aq) 
C)  Na+(aq) + Al(s) 
D)  Fe3+(aq) + Al(s) 
E)  None of the above pairs will react.

Question 18

Identify the battery that is in most automobiles.

Accepted Answer

A)  dry-cell battery 
B)  lithium ion battery 
C)  lead-acid storage battery 
D)  NiCad battery 
E)  fuel cell 
A)  dry-cell battery 
B)  lithium ion battery 
C)  lead-acid storage battery 
D)  NiCad battery 
E)  fuel cell

Question 19

Balance the following redox reaction if it occurs in H2SO4.What are the coefficients in front of C10H22O2 and H2SO4 in the balanced reaction? C10H22O2(aq)+ Na2Cr2O7(aq)→ C10H18O4(aq)+ Cr2(SO4)3(aq)

Accepted Answer

A)  C10H22O2 = 3, H2SO4 = 4 
B)  C10H22O2 = 2, H2SO4 = 8 
C)  C10H22O2 = 1, H2SO4 = 16 
D)  C10H22O2 = 3, H2SO4 = 16 
E)  C10H22O2 = 2, H2SO4 = 4 
A)  C10H22O2 = 3, H2SO4 = 4 
B)  C10H22O2 = 2, H2SO4 = 8 
C)  C10H22O2 = 1, H2SO4 = 16 
D)  C10H22O2 = 3, H2SO4 = 16 
E)  C10H22O2 = 2, H2SO4 = 4

Question 20

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

Accepted Answer

A)  I-(aq) + Zn2+(aq) 
B)  Ba(s) + Mn2+ (aq) 
C)  H2(g) + Cd2+(aq) 
D)  Ag(s) + Ni2+(aq) 
E)  All of the above pairs will react. 
A)  I-(aq) + Zn2+(aq) 
B)  Ba(s) + Mn2+ (aq) 
C)  H2(g) + Cd2+(aq) 
D)  Ag(s) + Ni2+(aq) 
E)  All of the above pairs will react.

Exam 19: Electrochemistry

Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. 3 I2(s)+ 2 Fe(s)→ 2 Fe3+(aq)+ 6 I⁻(aq)

Determine the redox reaction represented by the following cell notation. Fe(s)∣ Fe2+(aq) Cu2+(aq)∣ Cu(s)

How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten with an applied emf of 4.50 V?

Identify the battery that is used as a common flashlight battery.

What is the reducing agent in the redox reaction represented by the following cell notation? Ba(s)∣ Ba2+(aq) Li+(aq)∣ Li(s)

In a dry-cell battery,MnO2 is reduced to

What element is being oxidized in the following redox reaction? Mg2+(aq)+ NH4+(aq)→ Mg(s)+ NO3⁻(aq)

Given that E°red = -0.40 V for Cd2+/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s)∣ Cd2+(1.0 × 10-5 M)∣∣ Cd2+(0.100 M)∣ Cd(s)

What is the oxidizing agent in the redox reaction represented by the following cell notation? Mn(s)∣ Mn2+(aq) K+(aq)∣ K(s)

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(l) Sn(s)→ Sn2+(aq)+ 2 e- How many moles of Sn(s)are oxidized by four moles of Cr2O72-?

Identify the components of a fuel cell.

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s)∣ Sn2+(aq,1.8 M) Ag+(aq,0.055 M)∣ Ag(s)

Based on the following information, I2(s)+ 2 e- → 2 I-(aq)E° = +0.54 V Cd2+(aq)+ 2 e- → Cd (s)E° = -0.40 V Which of the following chemical species is the strongest reducing agent?

Why are iron nails coated with zinc?

In a nickel-metal hydride battery,NiO(OH)is reduced to

What element is being reduced in the following redox reaction? MnO4⁻(aq)+ H2C2O4(aq)→ Mn2+(aq)+ CO2(g)

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

Identify the battery that is in most automobiles.

Balance the following redox reaction if it occurs in H2SO4.What are the coefficients in front of C10H22O2 and H2SO4 in the balanced reaction? C10H22O2(aq)+ Na2Cr2O7(aq)→ C10H18O4(aq)+ Cr2(SO4)3(aq)

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

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Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction. 3 I₂(s)+ 2 Fe(s)→ 2 Fe³⁺(aq)+ 6 I⁻(aq)

Determine the redox reaction represented by the following cell notation. Fe(s)∣ Fe²⁺(aq) Cu²⁺(aq)∣ Cu(s)

What is the reducing agent in the redox reaction represented by the following cell notation? Ba(s)∣ Ba²⁺(aq) Li⁺(aq)∣ Li(s)

In a dry-cell battery,MnO₂ is reduced to

What element is being oxidized in the following redox reaction? Mg²⁺(aq)+ NH₄⁺(aq)→ Mg(s)+ NO₃⁻(aq)

Given that E°_red = -0.40 V for Cd²⁺/Cd at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Cd(s)∣ Cd²⁺(1.0 × 10^-5 M)∣∣ Cd²⁺(0.100 M)∣ Cd(s)

What is the oxidizing agent in the redox reaction represented by the following cell notation? Mn(s)∣ Mn²⁺(aq) K⁺(aq)∣ K(s)

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6 e^- → 2 Cr³⁺(aq)+ 7 H₂O(l) Sn(s)→ Sn²⁺(aq)+ 2 e^- How many moles of Sn(s)are oxidized by four moles of Cr₂O₇^2-?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s)∣ Sn²⁺(aq,1.8 M) Ag⁺(aq,0.055 M)∣ Ag(s)

Based on the following information, I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Cd²⁺(aq)+ 2 e^- → Cd (s)E° = -0.40 V Which of the following chemical species is the strongest reducing agent?

What element is being reduced in the following redox reaction? MnO₄⁻(aq)+ H₂C₂O₄(aq)→ Mn²⁺(aq)+ CO₂(g)

Balance the following redox reaction if it occurs in H₂SO₄.What are the coefficients in front of C₁₀H₂₂O₂and H₂SO₄ in the balanced reaction? C₁₀H₂₂O₂(aq)+ Na₂Cr₂O₇(aq)→ C₁₀H₁₈O₄(aq)+ Cr₂(SO₄)₃(aq)