Answer :
The Nernst equation :
[tex]E_{cell}=E^o_{cell}-\frac{2.303RT}{nF}\log \frac{[Anode]}{[Cathode]}[/tex]
where,
[tex]E^0[/tex] = standard cell potential
n = number of electrons in oxidation-reduction reaction
F = Faraday constant = 96500 C
R= gas constant = 8.314 J/Kmol
T = temperature
[Anode] = anodic ion concentration
[Cathode] = cathodic ion concentration
[tex]E_{cell}=E^o_{cell}-\frac{2.303RT}{nF}\log \frac{[Anode]}{[Cathode]}[/tex]
