Calculate the potential of a cell in which the following cell reaction occurs at 298 K.Snxx+ (1.5 M) + Zn(s) vec Sn2+ (0.5 M)+ Zn2+ (2 M)

Calculate the potential of the following cell reaction at 298 K Sn^(4+)(1.50 M)+Zn(s) to Sn^(2+)(0.50 M)+Zn^(2+)(2.0 M) The standard potential, E^(@) of the cell is 0.89 V. Whether the potential of the cell will increase or decrease if the concentration of Sn^(4+) is increased in the cell.

Calculate the potential of the following cell reaction at 298K: Sn^(4+)(1.50M)+Zn(s)rarrSn^(2+)(0.5M)+zn^(2+)(2.0M) The standard potential of the cell is 0.89V, will the potential of the cell will increase or decrease if the concentration of Sn^(2+) is increased in the cell?

Calculate the e.m.f of the following concentration cell at 298K, Zn(s)| Zn^(2+)(0.1) || Zn^(2+) (1.0)|Zn(s)

The emf of the cell in which the following reactions, Zn(s)+Ni^(2+) (0.1M) rarr Zn^(2+) (1.0 M) + Ni(s) occurs, is found to 0.5105 V at 298 K. The standard emf of the cell is :

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) .