Calculate the cell e.m.f. and `DeltaG` for the cell reaction at 298K for the cell.
`Zn(s) | Zn^(2+) (0.0004M) ||Cd^(2+) (0.2M)|Cd(s)`
Given, `E_(Zn^(2+)//Zn)^(@) =- 0.763 V, E_(Cd^(+2)//Cd)^(@) = - 0.403 V` at `298K`.
`F = 96500 C mol^(-1)`.

Calculate the cell e.m.f. and Delta G for the cell reaction at 298 K for the cell. Zn(s)|Zn^(2+)(0.0004 M)|| Cd^(2+)(0.2 M)| Cd(s) Given E_(Zn^(2+)//Zn)^(@)=-0.763 V,E_(cd^(2+)//cd)^(@)=-0.403 V " at "298 K, F=96500 C " mol"^(-1) .

Calculate the cell emf and Delta_(r ) G^(@) for the cell reation at 25^(@)C . Zn(s) | Zn^(@+) ( 0.1 M )|| Cd^(2+) ( 0.01M) | Cd(s) Given, E_(Zn^(2+) //Zn)^(@) = - 0.763V , E_(Cd^(2+) //Cd) ^(@) = - 0.403 V 1F = 96500 C "mol"^(-1) R = 8.314 JK^(-1) "mol"^(-1) ], Find E_("cell")^(@) = E_("cathode")^(@) - E_("anode")^(@) then Delta _(r ) G^(@) by using formula, Delta _(r ) G^(@) = - n FE_("cell")^(@)

Calculate the cell e.m.f. and DeltaG for the cell reaction at 25^(@)C for the cell: Zn_((s))|Zn^(2+)(0.004M)||Cd^(2+)(0.2M)|Cd_((s)) E^(@) values at 25^(@)C,Zn^(2+)//Zn=-0.763V Cd^(+2)//Cd=-0.403V F=96,500,R=8.314JK^(-1)mo"le"^(-1) .

Calculate e.m.f. of the cell, Zn//Zn^(2+)(aq) (0.01 M) ||Cd^(2+) (0.1 M)|Cd at 298 K. (Given E_(Zn^(2+)//Zn)^(@)=-0.76 V , E_(Cd^(2+)//Cd=-0.40 V )

Calculate the cell e.m.f. triangleG for the cell reaction at 25^oC. Zn(s)|Zn^(2+)(0.0004M)||Cd^(2+)|0.2M)|Cd(s) E^o values at 25^o , Zn^(2+)//Zn=-0.763 v and Cd^(2+)//Cd=-0.403 V

Calculate the cell e.m.f for reaction. Zn_((s))//Zn_((0.0004M))^(2+)//Cd_((0.2M))^(2+)//Cd_((s)) . Given E_(Zn^(2+)//Zn)^(@)= -0.763V, E_(Cd^(2+)//Cd)^(@)= -0.403V