Calculate ΔG°rxn and E°cell for a redox reaction with n = 2 that has an equilibrium...
Question:
Calculate ΔG°rxn and E°cell for a redox reaction with n = 2 that has an equilibrium constant of K = {eq}5.6\times10^{-2} {/eq}.
Relation between Electrode Potential and Change in Gibbs Free Energy
{eq}\Delta G^{o}=\ -nFE^{o}\ \\ Also, \Delta G^{o}=\ -RTlnk_{eq}\\ So, on\ comparing,\\ -nFE^{o}=-RTlnK_{eq}\\ {/eq}
F= Faraday constant
R= Gas constant
n= number of electrons involved
{eq}\Delta G^{o} {/eq}= Change in Standard Gibbs Free Energy
{eq}E^{o} {/eq}= Standard Reduction potential
So, with the help of this relation, we can calculate {eq}\Delta G^{o} {/eq} when {eq}E^{o} {/eq} is given and vice versa.
Answer and Explanation: 1
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View this answerCalculation of {eq}\boldsymbol{\mathbf{\Delta G^{o}}} {/eq}
As we know,
{eq}\Delta G^{o}=\ -RTlnK_{eq} {/eq}
where {eq}\Delta G^{o} {/eq}= Gibbs...
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