Concept explainers
To review:
The standard free energy for the following reactions:
Introduction:
Gibbs free energy is the potential that can be used for the calculation of maximum reversible work that is performed at constant temperature and pressure. The phosphoryl group transfer potential of a compound can be defined as ameasure of the strength of attachment of a group to amolecule. It usually refers to the differences in the standard free energies of the molecule with and without the group.
Explanation of Solution
According to the standard reduction potentials (E°’) given in table 9.1, E°’ of some
Redox half-reaction | E°’ (in Volt or V) |
|
|
|
-0.32 |
|
+0.235 |
The calculation of standard free energy for the following reactions is described below:
For calculating the standard free energy, the number of electrons transferred needs to be balanced. For a reaction, the standard free energy can be calculated by using the Nernst equation
Where,
n is the number of electrons transferred,
F is Faraday’s constant, which is 96.15 kJ/V.mol (kilojoule per Volt. mole) and
∆E°’ is overall cell potential.
∆E°’ can be calculated by the following formula:
In the given case, E°’ of electron acceptor is +0.82 V and that of electron donor is -0.32 V.
Putting the values of n, F, and ∆E°’ in the Nernst equation:
Thus, the standard free energy of the reaction is
In the given case, E°’ of the electron acceptor is +0.82 V and that of the electron donor is -0.235 V.
For a reaction, the standard free energy can be calculated by using the Nernst equation.
Putting the value of n, F, and ∆ E°’ in the Nernst equation:
Thus, the standard free energy of the reaction is
Thus, it can be concluded that the standard free energy of
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Chapter 9 Solutions
Biochemistry: The Molecular Basis of Life
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