Question

Nernst Equation at equilibrium only equation no details need ​

Answer 1

$\displaystyle\large\underline{\sf\purple{ Nernst\: Equation:- }}$

$\sf \: E_{cell}=E°_{cell}+\dfrac{-2.303RT}{nF}\log \dfrac{[Prduct]}{[Reactant]}$

At Equlilbrum ,$\sf \: E_{cell}=0$

The Nernst Equation is modified as :-

$\sf0=E°_{cell}+\dfrac{-2.303RT}{nF}log \dfrac{[Prduct] _{equilibrium}}{[Reactant] _{equilibrium}}$

$\sf \dashrightarrow \: E°_{cell} = \dfrac{2.303RT}{nF}\log(k_{c})$

• Kc= equilibrium constant at 298K

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