Electrochemistry - Result Question 28
####30. For the cell reaction
[2019]
$2 Fe^{3+}(aq)+2 I^{-}(aq) \to 2 Fe^{2+}(aq)+I_2(aq)$
$0.24 V$ at $298 K$. The standard Gibbs energy ( $\Delta$, $G^{\circ}$ ) of the cell reaction is:
[Given that Faraday constant $F=96500 C mol^{-1}$ ]
(a) $-46.32 kJ mol^{-1}$
(b) $-23.16 kJ mol^{-1}$
(c) $46.32 kJ mol^{-1}$
(d) $23.16 kJ mol^{-1}$
Show Answer
Solution:
- (a) $\Delta G=-n F E^{\circ}$
$=-2 \times 96500 \times 0.24=-46320 J / mol$
$=-46.32 kJ / mol$
