Nernst Equation

The Equation: $E = E^{\circ} - \frac{RT}{n F} ln Q$ , where $Q$ is the reaction quotient.
Variable $Q$ : $Q$ is defined by the concentrations (or activities) of products divided by reactants.
Application: It explains why the cell potential changes as reactants are consumed and products are formed. When the concentrations are non-standard (not $1$ M), $E \neq = E^{\circ}$ .
Equilibrium: As $Q$ approaches the equilibrium constant $K$ , $E$ drops toward zero. At equilibrium, $E = 0$ .

This medium difficulty chemistry question is from the chapter electrochemistry, covering the topic of nernst equation. It appeared in the 2025 exam.

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Nernst Equation

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