Question 1

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Cd and Ag+ in the balanced reaction?
Cd(s)+ Ag+(aq)→ Ag(s)+ Cd2+(aq)

Accepted Answer

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

Question 2

Nickel can be plated from aqueous solution according to the following half reaction.How long would it take (in minutes)to plate 29.6 g of nickel at 4.7 A?
Ni2+(aq)+ 2 e⁻ → Ni(s)

Accepted Answer

A) 1.7 × 102 minutes 
B) 5.9 × 102 minutes 
C) 3.5 × 102 minutes 
D) 4.8 × 102 minutes 
E) 6.2 × 102 minutes

Question 3

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

Question 4

Which of the following is the strongest reducing agent?

Accepted Answer

A) Na(s) 
B) Li+(aq) 
C) Ca(s) 
D) Ca2+(aq) 
E) Li(s)

Question 5

What is undergoing reduction in the redox reaction represented by the following cell notation?
Fe(s)∣ Fe3+(aq)∣∣ Cl2(g)∣ Cl⁻(aq)∣ Pt

Accepted Answer

A) Fe(s) 
B) Fe3+(aq) 
C) Cl2(g) 
D) Cl⁻(aq) 
E) Pt

Question 6

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K)for the following balanced redox reaction at 25°C.
Pb2+(aq)+ Cu(s)→ Pb(s)+ Cu2+(aq)

Accepted Answer

A) 7.9 × 10-8 
B) 8.9 × 107 
C) 7.9 × 1015 
D) 1.3 × 10-16 
E) 1.1 × 10-8

Question 7

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

Accepted Answer

The answer of Why,if we multiply a reaction by 2,don't...

Question 8

What is the shorthand notation that represents the following galvanic cell reaction?
Pb(s)+ Cu(NO3)2(aq)→ Pb(NO3)2(aq)+ Cu(s)

Accepted Answer

A) Pb(s)∣ Pb2+(aq)∣∣ Cu2+(aq)∣ Cu(s) 
B) Cu(s)∣ Cu2+(aq)∣∣ Pb2+(aq)∣ Pb(s) 
C) Pb(s)∣ NO3-(aq)∣∣ NO3-(aq)∣ Cu(s) 
D) Cu(s)∣ Cu(NO3)2(aq)∣∣ Pb(NO3)2(aq)∣ Pb(s)

Question 9

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al2O3 · xH2O The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

Accepted Answer

A) 0.0168 
B) 0.0596 
C) 39.7 
D) 19.9 
E) 59.6

Question 10

Which of the following reactions would have the smallest value of K at 298 K?

Accepted Answer

A) A + B → C;E°cell = +1.22 V 
B) A + 2 B → C;E°cell = 0.98 V 
C) A + B → 2 C;E°cell = -0.030 V 
D) A + B → 3 C;E°cell = 0.15 V 
E) More information is needed to determine.

Question 11

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

Accepted Answer

A) 10.9 g 
B) 16.4 g 
C) 32.8 g 
D) 36.3 g

Question 12

The electrolysis of molten AlCl3 for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

Accepted Answer

A) 147 
B) 0.606 
C) 4.55 × 10-3 
D) 16.4 
E) 49.1

Question 13

How many electrons are transferred in the following reaction? (The reaction is unbalanced. )
Fe2+(aq)+ K(s)→ Fe(s)+ K+(aq)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 6

Question 14

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode?
Zn(s)∣ Zn2+(aq)∣∣ Ni2+(aq)∣ Ni(s)

Accepted Answer

A) Zn(s)→ Zn2+(aq)+ 2 e- 
B) Zn2+(aq)+ 2 e- → Zn(s) 
C) Ni(s)→ Ni2+(aq)+ 2 e- 
D) Ni2+(aq)+ 2 e- → Ni(s)

Question 15

Using the following standard reduction potentials,
Fe3+(aq)+ e- → Fe2+(aq)E° = +0.77 V
Ni2+(aq)+ 2 e- → Ni(s)E° = -0.26 V
Calculate the standard cell potential for the galvanic cell reaction given below,and determine whether or not this reaction is spontaneous under standard conditions.
Ni2+(aq)+ 2 Fe2+(aq)→ 2 Fe3+(aq)+ Ni(s)

Accepted Answer

A) E° = -0.98 V,nonspontaneous 
B) E° = -0.98 V,spontaneous 
C) E° = +0.98 V,nonspontaneous 
D) E° = +0.98 V,spontaneous

Question 16

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

Question 17

For a galvanic cell that uses the following two half-reactions,
Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(l)
Pb(s)→ Pb2+(aq)+ 2 e-
How many moles of Pb(s)are oxidized by three moles of Cr2O72-?

Accepted Answer

A) 3 
B) 6 
C) 9 
D) 18

Question 18

Determine the cell notation for the redox reaction given below.
Sn(s)+ 2 Ag⁺(aq)→ Sn2+(aq)+ 2 Ag(s)

Accepted Answer

A) Ag+(aq)∣ Ag(s)∣∣ Sn(s)∣ Sn2+(aq) 
B) Ag(s)∣ Ag+(aq)∣∣ Sn2+(aq)∣ Sn(s) 
C) Sn(s)∣ Sn2+(aq)∣∣ Ag+(aq)∣ Ag(s) 
D) Sn2+(aq)∣ Sn(s)∣∣ Ag(s)∣ Ag+(aq) 
E) Sn(s)∣ Ag(s)∣∣ Sn2+(aq)∣ Ag+(aq)

Question 19

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Al and F2 in the balanced reaction?
Al(s)+ F2(g)→ Al3+(aq)+ F-(aq)

Accepted Answer

A) Al = 2,F2 = 3 
B) Al = 2,F2 = 6 
C) Al = 1,F2 = 1 
D) Al = 2,F2 = 1 
E) Al = 3,F2 = 2

Question 20

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

Accepted Answer

A) Pb2+(aq)+ Cu(s) 
B) Ag+(aq)+ Br⁻(aq) 
C) Li+(aq)+ Cr(s) 
D) Fe3+(aq)+ Cd(s) 
E) None of the above pairs will react.

Exam 18: Electrochemistry

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Cdand Ag⁺ in the balanced reaction? Cd(s) + Ag⁺(aq) → Ag(s) + Cd²⁺(aq)

Nickel can be plated from aqueous solution according to the following half reaction.How long would it take (in minutes) to plate 29.6 g of nickel at 4.7 A? Ni²⁺(aq) + 2 e⁻ → Ni(s)

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.

Which of the following is the strongest reducing agent?

What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe³⁺(aq) ∣∣ Cl₂(g) ∣ Cl⁻(aq) ∣ Pt

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq)

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO₃) ₂(aq) → Pb(NO₃) ₂(aq) + Cu(s)

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al₂O₃ · xH₂O The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

Which of the following reactions would have the smallest value of K at 298 K?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Fe²⁺(aq) + K(s) → Fe(s) + K⁺(aq)

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s) ∣ Zn²⁺(aq) ∣∣ Ni²⁺(aq) ∣ Ni(s)

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)

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) Pb(s) → Pb²⁺(aq) + 2 e^- How many moles of Pb(s) are oxidized by three moles of Cr₂O₇^2-?

Determine the cell notation for the redox reaction given below. Sn(s) + 2 Ag⁺(aq) → Sn²⁺(aq) + 2 Ag(s)

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Aland F₂ in the balanced reaction? Al(s) + F₂(g) → Al³⁺(aq) + F^-(aq)

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

Exam 18: Electrochemistry

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of Cd and Ag+ in the balanced reaction? Cd(s) + Ag+(aq) → Ag(s) + Cd2+(aq)

Nickel can be plated from aqueous solution according to the following half reaction.How long would it take (in minutes) to plate 29.6 g of nickel at 4.7 A? Ni2+(aq) + 2 e⁻ → Ni(s)

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.

Which of the following is the strongest reducing agent?

What is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq) ∣∣ Cl2(g) ∣ Cl⁻(aq) ∣ Pt

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

Why,if we multiply a reaction by 2,don't we multiply its E°red by 2?

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO3) 2(aq) → Pb(NO3) 2(aq) + Cu(s)

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al2O3 · xH2O The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

Which of the following reactions would have the smallest value of K at 298 K?

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes?

The electrolysis of molten AlCl3 for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Fe2+(aq) + K(s) → Fe(s) + K+(aq)

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s) ∣ Zn2+(aq) ∣∣ Ni2+(aq) ∣ Ni(s)

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)

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr3+(aq) + 7 H2O(l) Pb(s) → Pb2+(aq) + 2 e- How many moles of Pb(s) are oxidized by three moles of Cr2O72-?

Determine the cell notation for the redox reaction given below. Sn(s) + 2 Ag⁺(aq) → Sn2+(aq) + 2 Ag(s)

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Al and F2 in the balanced reaction? Al(s) + F2(g) → Al3+(aq) + F-(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 Cdand Ag⁺ in the balanced reaction? Cd(s) + Ag⁺(aq) → Ag(s) + Cd²⁺(aq)

Nickel can be plated from aqueous solution according to the following half reaction.How long would it take (in minutes) to plate 29.6 g of nickel at 4.7 A? Ni²⁺(aq) + 2 e⁻ → Ni(s)

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 is undergoing reduction in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe³⁺(aq) ∣∣ Cl₂(g) ∣ Cl⁻(aq) ∣ Pt

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq)

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

What is the shorthand notation that represents the following galvanic cell reaction? Pb(s) + Cu(NO₃) ₂(aq) → Pb(NO₃) ₂(aq) + Cu(s)

The most useful ore of aluminum is bauxite,in which Al is present as hydrated oxides,Al₂O₃ · xH₂O The number of kilowatt-hours of electricity required to produce 4.00 kg of aluminum from electrolysis of compounds from bauxite is ________ when the applied emf is 5.00 V.

How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl₂ for 60.0 minutes?

The electrolysis of molten AlCl₃ for 3.25 hr with an electrical current of 15.0 A produces ________ g of aluminum metal.

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Fe²⁺(aq) + K(s) → Fe(s) + K⁺(aq)

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? Zn(s) ∣ Zn²⁺(aq) ∣∣ Ni²⁺(aq) ∣ Ni(s)

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)

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) Pb(s) → Pb²⁺(aq) + 2 e^- How many moles of Pb(s) are oxidized by three moles of Cr₂O₇^2-?

Determine the cell notation for the redox reaction given below. Sn(s) + 2 Ag⁺(aq) → Sn²⁺(aq) + 2 Ag(s)

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Aland F₂ in the balanced reaction? Al(s) + F₂(g) → Al³⁺(aq) + F^-(aq)