Write the Nernst equation for the electrode reaction: $$\mathrm{M^{n+}} + n\,e^- \longrightarrow \mathrm{M(s)}$$

CBSE Class 12 · 2002 · Delhi · Redox Reactions and ElectrochemistryVery Short Answer

Write the Nernst equation for the electrode reaction:

M^{n +} + n e^{-} ⟶ M (s)

Answer: E = E° − (0.059/n) log(1/[Mⁿ⁺]) = E° + (0.059/n) log[Mⁿ⁺] at 298 K.

For M

^{n +}

n

^{-} \to

M(s), at 298 K:

E_{M^{n +} /M} = E_{M^{n +} /M}^{\circ} - \frac{0.059}{n} lo g \frac{1}{[ M ^{n +} ]}

equivalently

E = E^{\circ} + \frac{0.059}{n} lo g [M^{n +}]

CBSE Class 12 Board · 2002 · Delhi · Subjective