Question:
The standard emf of a cell involving one electron charge is found to be $0.591\, V$ at $25^{\circ} C$. The equilibrium constant of the reaction is $\left(1\, F =96500\, C\, mol ^{-1}, R=8.314\, J\, K ^{-1} mol ^{-1}\right)$
The standard emf of a cell involving one electron charge is found to be $0.591\, V$ at $25^{\circ} C$. The equilibrium constant of the reaction is $\left(1\, F =96500\, C\, mol ^{-1}, R=8.314\, J\, K ^{-1} mol ^{-1}\right)$
Updated On: Jul 28, 2022
- $ 1.0\times 10^{1}$
- $ 1.0\times 10^{30}$
- $ 1.0\times 10^{10}$
- $ 1.0\times 10^{5}$
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The Correct Option is C
Solution and Explanation
At $298\, K$
$E^{\circ} =\frac{0.0591}{n} \log K_{c}$
$0.591 =\frac{0.0591}{1} \log K_{c}$
$\log K_{c} =\frac{0.5910}{0.0591}$
$\log K_{c} =10$
$K_{c} =10^{10}$
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Concepts Used:
Nernst Equation
This equation relates the equilibrium cell potential (also called the Nernst potential) to its concentration gradient across a membrane. If there is a concentration gradient for the ion across the membrane, an electric potential will form, and if selective ion channels exist the ion can cross the membrane.
