
(a)
Interpretation:
The equilibrium constant for the given reaction has to be calculated.
Concept Introduction:
Half–cell reactions: In the
Standard cell potentials: The standard emf (electromotive force,
Redox reactions: A
- Oxidation half-reaction.
- Reduction half-reaction.
(a)

Explanation of Solution
The given reaction is
The equilibrium constant, K is calculated as follows,
(b)
Interpretation:
The equilibrium constant for the given reaction has to be calculated.
Concept Introduction:
Half–cell reactions: In the electrochemical cell, both oxidation and reduction occur simultaneously. The oxidation occurs at the anode, while the reduction occurs at the cathode. The loss of an electron occurs from the anode by oxidation as well as the gain of an electron occurs from the cathode by reduction.
Standard cell potentials: The standard emf (electromotive force,
Redox reactions: A redox reaction is a chemical reaction where both oxidation and reduction occur simultaneously. In a redox reaction, one of the reactant is oxidized, while the other reactant is reduced at the same time. It can be represented as two half-reactions with the number of transferred electrons. They are as follows:
- Oxidation half-reaction.
- Reduction half-reaction.
(b)

Explanation of Solution
The given reaction is
The equilibrium constant, K is calculated as follows,
(c)
Interpretation:
The equilibrium constant for the given reaction has to be calculated.
Concept Introduction:
Half–cell reactions: In the electrochemical cell, both oxidation and reduction occur simultaneously. The oxidation occurs at the anode, while the reduction occurs at the cathode. The loss of an electron occurs from the anode by oxidation as well as the gain of an electron occurs from the cathode by reduction.
Standard cell potentials: The standard emf (electromotive force,
Redox reactions: A redox reaction is a chemical reaction where both oxidation and reduction occur simultaneously. In a redox reaction, one of the reactant is oxidized, while the other reactant is reduced at the same time. It can be represented as two half-reactions with the number of transferred electrons. They are as follows:
- Oxidation half-reaction.
- Reduction half-reaction.
(c)

Explanation of Solution
The given reaction is
The equilibrium constant, K is calculated as follows,
(d)
Interpretation:
The equilibrium constant for the given reaction has to be calculated.
Concept Introduction:
Half–cell reactions: In the electrochemical cell, both oxidation and reduction occur simultaneously. The oxidation occurs at the anode, while the reduction occurs at the cathode. The loss of an electron occurs from the anode by oxidation as well as the gain of an electron occurs from the cathode by reduction.
Standard cell potentials: The standard emf (electromotive force,
Redox reactions: A redox reaction is a chemical reaction where both oxidation and reduction occur simultaneously. In a redox reaction, one of the reactant is oxidized, while the other reactant is reduced at the same time. It can be represented as two half-reactions with the number of transferred electrons. They are as follows:
- Oxidation half-reaction.
- Reduction half-reaction.
(d)

Explanation of Solution
The given reaction is
The equilibrium constant, K is calculated as follows,
(e)
Interpretation:
The equilibrium constant for the given reaction has to be calculated.
Concept Introduction:
Half–cell reactions: In the electrochemical cell, both oxidation and reduction occur simultaneously. The oxidation occurs at the anode, while the reduction occurs at the cathode. The loss of an electron occurs from the anode by oxidation as well as the gain of an electron occurs from the cathode by reduction.
Standard cell potentials: The standard emf (electromotive force,
Redox reactions: A redox reaction is a chemical reaction where both oxidation and reduction occur simultaneously. In a redox reaction, one of the reactant is oxidized, while the other reactant is reduced at the same time. It can be represented as two half-reactions with the number of transferred electrons. They are as follows:
- Oxidation half-reaction.
- Reduction half-reaction.
(e)

Explanation of Solution
The given reaction is
The equilibrium constant, K is calculated as follows,
(f)
Interpretation:
The equilibrium constant for the given reaction has to be calculated.
Concept Introduction:
Half–cell reactions: In the electrochemical cell, both oxidation and reduction occur simultaneously. The oxidation occurs at the anode, while the reduction occurs at the cathode. The loss of an electron occurs from the anode by oxidation as well as the gain of an electron occurs from the cathode by reduction.
Standard cell potentials: The standard emf (electromotive force,
Redox reactions: A redox reaction is a chemical reaction where both oxidation and reduction occur simultaneously. In a redox reaction, one of the reactant is oxidized, while the other reactant is reduced at the same time. It can be represented as two half-reactions with the number of transferred electrons. They are as follows:
- Oxidation half-reaction.
- Reduction half-reaction.
(f)

Explanation of Solution
The given reaction is
The equilibrium constant, K is calculated as follows,
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Chapter 5 Solutions
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