
Calculate

Interpretation:
The standard cell potential, emf of the galvanic cell, and free energy change for the given cell reactions at
are to be determined.
Concept introduction:
Gibbs free energy is the change in the enthalpy
According to the standard reduction potential values, the electrode that has lower negative reduction potential will act as a cathode and will undergo reduction. However, if the negative reduction potential of the electrode is high, it will act as an anode and will undergo oxidation.
The standard reduction potential of a galvanic cell may be calculated in terms of standard reduction potential of cathode and anode, as the relation mentioned below:
According to the Nernst equation, the relation between emf, standard cell potential, and reaction quotient at
will be as follows:
Here,
The relation between cell potential and free energy change is as follows:
Here,
is the Gibb’s free energy change,
is the Faraday constant
Answer to Problem 30QP
Solution:
(a)
(b)
Explanation of Solution
a)
The overall reaction of galvanic cell is as follows:
The half-cell reactions of
Oxidation half reaction (Anode):
Reduction half reaction (Cathode):
As the standard reduction potential of
half-cell reaction is less (more negative); therefore, it will act as an anode and will undergo oxidation.
Therefore,
The cell representation of a galvanic cell is as follows:
The standard cell potential that is
(at
) for the above galvanic cell is calculated as follows:
The reaction quotient for the reaction is given by the following expression:
Concentration of
and
is
and
Substitute all the values in the above equation,
In the given galvanic cell, the total loss and total gain of electrons is two.
Now, according to the Nernst equation, the relation between emf, standard cell potential, and reaction quotient at
will be as follows:
Substitute all the values in the above equation,
The relation between cell potential and free energy change is as follows:
Substitute all the values in the above equation,
b)
The overall reaction of galvanic cell is as follows:
The half-cell reactions of
Oxidation half reaction (Anode):
Reduction half reaction (Cathode):
As the standard reduction potential of
half-cell reaction is greater (less negative), it will act as a cathode and will undergo reduction. However, the standard reduction potential of
half-cell reaction is less (more negative); therefore, it will act as an anode and will undergo oxidation.
Therefore,
The cell representation of a galvanic cell is as follows:
The standard cell potential that is
(at
) for the above galvanic cell is calculated as follows:
The reaction quotient for the reaction is as follows:
Concentration of
and
is
and
Substitute all the values in the above expression,
In the given galvanic cell, the total loss of electron and total gain of electron is six.
Now, according to the Nernst equation, the relation between emf, standard cell potential, and reaction quotient at
will be as follows:
On substituting all the values in the above equation,
The relation between cell potential and free energy change is as follows:
Substitute the values of
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Chapter 19 Solutions
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