For the net cell reaction of the cell `Zn(s) |Xn^(2+) ||Cd^(2+) |Cd(s) DeltaG^(@)` in Kilojules at `25^(@)C` is `(E_(cell)^(@) = 0.360 V)`:-

For the net cell reaction of the cell Zn(s) |Xn^(2+) ||Cd^(2+) |Cd(s) DeltaG^(@) in Kilojoules at 25^(@)C is (E_(cell)^(@) = 0.360 V) :-

Cell reaction for the cell Zn|Zn^(2+)(1.0M)||Cd^(2+)(1.0M)|Cd is given by

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 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 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 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 standard reduction potential of Cd^(2+)//Cd electrode for the cell : Zn(s)|Zn^(2+)("IM") || Cd^(2+)(IM)|Cd(s) ("Given that " E_(cell)^(@)=0.36 V and E_(Zn^(2+)//Zn)^(@)=-0.76V)

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) .