The standard Gibbs energy change ($\Delta G^\circ$) is related to the standard cell potential (E$^\circ$) by:
\[ \Delta G^\circ = -nFE^\circ \]
where:
n is the number of moles of electrons transferred in the balanced redox reaction.
F is Faraday's constant (96487 C mol$^{-1}$).
E$^\circ$ is the standard cell potential.
In the given reaction, Zn(s) is oxidized to Zn$^{2+}$(aq) and Fe$^{2+}$(aq) is reduced to Fe(s).
Thus, n=2. E$^\circ$ = 0.32 V
\(\Delta G^\circ = -(2 mol)(96487 C mol^{-1})(0.32 V) \)
\(\Delta G^\circ = -61751.04 J mol^{-1} \approx -61.75 kJ mol^{-1}\)
List I | List II | ||
A | Down’s syndrome | I | 11th chormosome |
B | α-Thalassemia | II | ‘X’ chromosome |
C | β-Thalassemia | III | 21st chromosome |
D | Klinefelter’s syndrome | IV | 16th chromosome |