For the cell, Hg, Hg₂Cl₂/ Cl⁻ (0.1M) / Cl⁻(0.01M) / Cl₂;pt E_cell 0 is 1.10V. Hence, Ecell  is 

Explanation

Stepwise reactions:

2Cl⁻ + 2Hg → Hg₂Cl₂ + 2e⁻ 2e⁻ + Cl₂ → 2Cl⁻

Combined reaction:

2Hg + Cl₂ → Hg₂Cl₂

E° = 1.1 V

Nernst Equation

E_cell = 1.1 - (0.0591 / 2) log([Cl⁻]²_cathode / [Cl⁻]_anode)

Substituting Values

E_cell = 1.1 - (0.0591 / 2) log((0.01)² / (0.1)²) E_cell = 1.1 - (0.0591 / 2) log(0.01) E_cell = 1.1 - (0.0591 / 2) × (-2) E_cell = 1.1 + 0.0591

Final Answer

E_cell = 1.1591 V