Home
Class 12
CHEMISTRY
[" - A "[21]" Calculate the cell emf and...

[" - A "[21]" Calculate the cell emf and "Delta G" for the cell reaction at "25^(@)C],[" ne cell: "],[qquad [Zn(s)|Zn^(2+)(0.0004m)|Cd^(2+)(0.2M)'Cd(s)],[E^(@)" values at "25^(@)C:Zn^(2+)|Zn=-0.763V],[F=96500C,R=8.314JK^(-1)mol^(-1)]]

Promotional Banner

Similar Questions

Explore conceptually related problems

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 emf and triangle_(r)G^(@) for the cell reactin at 25^(@)C Zn(s)|Zn^(2+)(0.1M)||Cd^(2+)(0.01M)|Cd(s) (given E_(Zn^(2+)//Zn)^(@)=-0.763V,E_(Cd^(2+)//Cd)^(@)=-0.403V 1F=96500Cmol^(-1),R=8.314JK^(-1)mol^(-1)]

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. 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 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) .