Relation between equilibrium constant and standard potential of the cell under standard conditions is represented by ____.

$E°_{cell}=\frac{2.303\, RT}{nF}\log K_c$

The correct answer is Option (2) → $E°_{cell}=\frac{2.303\, RT}{nF}\log K_c$

The relation between the standard cell potential (E°cell) and the equilibrium constant (Kc) under standard conditions is derived from the Nernst equation:

The fundamental equations are:

ΔG° = −nF E°cell

ΔG° = −RT ln K

Where n = number of electrons transferred

F = Faraday constant

R = gas constant

T = temperature in Kelvin

Equating the two equations:

$\Delta G^\circ = -RT \ln K = -n F E^\circ_\text{cell}$

$E^\circ_\text{cell} = \frac{RT}{nF} \ln K$

Converting ln to log₁₀:

$E^\circ_\text{cell} = \frac{2.303 RT}{nF} \log K$