drive the relation between NEARST equation and equilibrium constant Kc.
Answers
nearst equation is
Ecell = E0 – [RT/nF] ln Q
Where,
Where,Ecell = cell potential
E0 = cell potential
R = gas constant
T = temperature
n = number of electrons transferred in the redox reaction
F = Faraday constant
Q = reaction quotient
derivation -
When the reactants and the products of the cell reach equilibrium, the value of ΔG becomes 0. At this point, the reaction quotient and the equilibrium constant (Kc) are the same.
Since ΔG = -nFE, the cell potential at equilibrium is also 0.
Substituting the values of Q and E into the Nernst equation, the following equation is obtained.
0 = E°cell – (RT/nF) ln Kc
E0cell = (0.0592V/n) log Kc
E0cell = (0.0592V/n) log KcRearranging this equation, the following equation can be obtained.
E0cell = (0.0592V/n) log KcRearranging this equation, the following equation can be obtained.log Kc = (nE0cell)/0.0592V
E0cell = (0.0592V/n) log KcRearranging this equation, the following equation can be obtained.log Kc = (nE0cell)/0.0592VThus, the relationship between the standard cell potential and the equilibrium constant is obtained.
hope it helps