Relation between equilibrium constant and standard potential of the cell under standard conditions is represented by ____.
Answer & explanation
Correct answer: option 2
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:
$E^\circ_\text{cell} = \frac{2.303 RT}{nF} \log K$