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For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at $25^\circ C$. The value of standard Gibbs energy, $\Delta G^\circ$, will be (F = 96500 C $mol^{-1}$)
A
−98.0 kJ
B
−89.0 kJ
C
−89.0 J
D
−44.5 kJ
Detailed Solution
Cell reaction: $Cu + 2Ag^+ \rightarrow Cu^{2+} + 2Ag$
Copper loses two electrons, so n = 2.
$\Delta G^\circ = -nFE^\circ_{cell}$
$\Delta G^\circ = -2\times96500\times0.46$
$\Delta G^\circ = -88780$ J
$\Delta G^\circ \approx -89.0$ kJ
Copper loses two electrons, so n = 2.
$\Delta G^\circ = -nFE^\circ_{cell}$
$\Delta G^\circ = -2\times96500\times0.46$
$\Delta G^\circ = -88780$ J
$\Delta G^\circ \approx -89.0$ kJ