Respuesta :
Answer: [tex]\Delta G^0=22823J[/tex]
[tex]E^0=-0.12V[/tex]
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 [tex]K_{eq}[/tex]
The Gibbs free energy is related to equilibrium constant by following relation:
[tex]\Delta G^0=-2.303RTlog K[/tex]
R = gas constant = 8.314 J/Kmol
T = temperature in kelvin =[tex]298K[/tex]
K = equilibrium constant
[tex]\Delta G^0=-2.303RTlog K[/tex]
[tex]\Delta G^0=-2.303\times 8.314\times 298\times log(1.0\times 10^{-4})[/tex]
[tex]\Delta G^0=22823J[/tex]
The standard emf of a cell is related to Gibbs free energy by following relation:
[tex]\Delta G^0=-nFE^0[/tex]
[tex]\Delta G^0[/tex] = gibbs free energy = 22823J
n= no of electrons gained or lost = 2
F= faraday's constant = 96500 C
[tex]E^0[/tex] = standard emf
[tex]22823J=-2\times 96500\times E^0[/tex]
[tex]E^0=-0.12V[/tex]
