A cell Ni(s) | Ni²⁺(0.002 M) || Cl₂(g)(0.5 atm) | Cl⁻(0.05 M) | Pt(s) operates at 298 K. What is the cell potential? (Gi
E°cell = 1.36 - (-0.25) = 1.61 V . Ecell = 1.61 - (0.059/2) log ([Ni²⁺][Cl⁻]²/PCl_₂) = 1.61 - 0.0295 log (0.002 × 0.0025/0.5) = 1.61 + 0.084 = 1.694 V .
Ref: NCERT Class 12 Chemistry > Chapter 2: Electrochemistry > Topic: Nernst Equation and Gibbs Energy and Equilibrium Constant