Zn | Zn^(2+) (0.6 M) ||H^+(1.2 M) | H^2(g,1 atm) | Pt = -0.763 V ​

Question

Calculate the potential of the following cell at 25 °C :

Zn | Zn²⁺ (0.6 M) ||H⁺(1.2 M) | H₂(g,1 atm) | Pt

\(E^0_{Zn^{2+}/Zn}\) = -0.763 V

Answer 1

Given,

\(E^0_{Zn^{2+}/Zn}\) = -0.763 V;

Concentrations :

[Zn²⁺] = 0.6 M; [H⁺] = 1.2 M

[H₂]_g = 1 atm

Cell potential = E_Cell = ?

= 0.763 – 0.0296 × (- 0.3801) 

= 0.763 + 0.01125 

= 0.77425 V

∴ Cell potential = E⁰_Cell = 0.77425 V