Mark the correct Nernst equation for the given cell. `F_((s))|Fe^(2+)(0.001 M) ||H^(+)(1M) | H_(2(g)) ( 1 bar ) | Pt_((s))` is

Options

A. `E_("cell")=E_("cell")^(@)-(0.591)/(2) log""([Fe^(2+)][H^(+)]^(2))/([Fe][H_(2)])`
B. `E_("cell")=E_("cell")^(@)-(0.591)/(2) log""([Fe][H^(+)]^(2))/([Fe^(2+)][H_(2)])`
C. `E_("cell")=E_("cell")^(@)-(0.591)/(2) log""([Fe^(2+)][H_(2)])/([Fe][H^(+)]^(2))`
D. `E_("cell")=E_("cell")^(@)-(0.591)/(2) log""([Fe][H_(2)])/([Fe^(2+)][H^(+)]^(2))`

Answer

C

Explanation

At Anode : `Fe to Fe^(3+) (0.001 M) + 2e^(-)`
`("At cathode": 2H^(+) (1M) + 2e^(-) to H_(2) (1"atm"))/("Net Reaction": Fe+2H^(+) to Fe^(@+) + H_(2))`
Nernst equation for the given cell,
`E_("cell")=E_("cell")^(0) -(0.0591)/(2) log""([Fe^(2+)][H_(2)])/([Fe][H^(+)]^(2))`