Calculate emf of the following cell at 25℃. Fe|Fe²⁺(0.001M)|H⁺(0.01M)|H₂(g)(1bar)Pt(s) E°(Fe²⁺|Fe)=-0.44V E°(H⁺/H₂)=0.00V

For the given cell representation, the cell reaction will be
Fe(s)+2H⁺(aq)→Fe²⁺(aq)+H₂(g)
The standard emf of the cell will be
E°cell=E°H⁺/H₂-E°Fe²⁺/Fe
E°cell=0-(-0.44)=0.44V
The Nernst equation for the cell reaction at 25℃ will be
Ecell=E°cell-0.0591/nlog[Fe²⁺][H⁺]²
=0.44-0.0591/2log0.001(0.01)²
=0.44-0.0591/2log10⁻⁵
=0.44-0.0591/2(-5)
=0.44+0.14775
Ecell=0.58775V ≈0.59V