Nernst Equation

Question

Nernst equation relates electrode potential to:

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1. **The Equation**: $E = E^\circ - \frac{RT}{nF} \ln Q$, where $Q$ is the reaction quotient.
2. **Variable $Q$**: $Q$ is defined by the concentrations (or activities) of products divided by reactants. 
3. **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), $E 
eq E^\circ$.
4. **Equilibrium**: As $Q$ approaches the equilibrium constant $K$, $E$ drops toward zero. At equilibrium, $E = 0$.

Nernst Equation

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