If the equilibrium constant for a two-electron redox reaction at 298 k is 1.0×10−4, calculate the corresponding δg∘ and e∘cel under standard conditions.

δg∘ =

e∘cell =

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as

The Gibbs free energy is related to equilibrium constant by following relation:

R = gas constant = 8.314 J/Kmol

T = temperature in kelvin =

K = equilibrium constant

The standard emf of a cell is related to Gibbs free energy by following relation:

= gibbs free energy  = 22823J

n= no of electrons gained or lost  = 2

F= faraday's constant  = 96500 C

= standard emf

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