1. Tardigrade
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  3. Chemistry
  4. The Gibbs energy change (in J) for the given reaction at [ Cu 2+]=[ Sn 2+]=1 M and 298 K is: Cu ( s )+ Sn 2+( aq .) arrow Cu 2+( aq .)+ Sn ( s ) ( E Sn 2+ Sn 0=-0.16 V , E Cu 2+| Cu 0=0.34 V . Take .F=96500 C mol -1)

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Q. The Gibbs energy change (in J) for the given reaction at $\left[ Cu ^{2+}\right]=\left[ Sn ^{2+}\right]=1 M$ and $298 K$ is:

$Cu ( s )+ Sn ^{2+}( aq .) \rightarrow Cu ^{2+}( aq .)+ Sn ( s )$

$\left( E _{ Sn ^{2+} Sn }^{0}=-0.16 V , E _{ Cu ^{2+}| Cu }^{0}=0.34 V \right.$

Take $\left.F=96500 C mol ^{-1}\right)$

JEE MainJEE Main 2020Thermodynamics

Solution:

$\Delta G=\Delta G^{o}+R T \ln \left[\frac{S n^{+2}}{C u^{+2}}\right]$

$=-2 \times 96500[(-0.16)-0.34]+R T \ln \left(\frac{1}{1}\right)$

$=96500 J$