1. Tardigrade
  2. Question
  3. Chemistry
  4. The standard Gibbs energy for the given cell reaction in kJ mol-1 at 298 K is: Zn(s) + Cu2+ (aq) arrow Zn2+ (aq) + Cu (s), E° = 2 V at 298 K (Faraday's constant, F = 96000 C mol-1)

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Q. The standard Gibbs energy for the given cell reaction in $kJ \,mol^{-1}$ at $298 K$ is : $Zn(s) + Cu^{2}+ (aq) \rightarrow Zn^{2+} (aq) + Cu (s), E° = 2 V$ at $298 K$ (Faraday's constant, $F = 96000\, C\, mol^{-1}$)

JEE MainJEE Main 2019Equilibrium

Solution:

$\Delta \, G^{\circ} \, = \, -nFE^{\circ}_{cell}$
=$-2 \times 96000 \times 2$
= $-384000\, J$
= $-384\, kJ$