The standard emf of the cell.
`Cd(s) | CdCl_(2) (aq) rightarrow 2Ag(s) + Cd^(2+) (aq) + 2Cl^(-)(aq)` is 0.6915 V at `0^(@)` and 0.6753 V at `25^(@)C`. The `DeltaH^(@)` of the reaction at `25^(@)C` is:

The standard emf of the cell, Cd(s) |CdCI_(2) (aq) (0.1M)||AgCI(s)|Ag(s) in which the cell reaction is Cd(s) +2AgCI(s) rarr 2Ag(s) +Cd^(2+) (aq) is 0.6915 V at 0^(@)C and 0.6753V at 25^(@)C . The DeltaH of the reaction at 25^(@)C is,-

The standard emf of the cell, Cd(s) |CdCI_(2) (aq) (0.1M)||AgCI(s)|Ag(s) in which the cell reaction is Cd(s) +2AgCI(s) rarr 2Ag(s) +Cd^(2+) (aq) is 0.6915 V at 0^(@)C and 0.6753V at 25^(@)C . The DeltaH of the reaction at 25^(@)C is,-

The EMF of the following cell : Cd(s)|CdCl_(2)(0.10M)|AgCl(s)|Ag(s) is 0.6915V at 0^(@)C and 0.6753V at 25^(@)C . The DeltaH of reaction in kJ at 25^(@)C is

The EMF of the following cell : Cd(s)|CdCl_(2)(0.10M)||AgCl(s)|Ag(s) is 0.6915V at 0^(@)C and 0.6753V at 25^(@)C . The DeltaH of reaction in kJ at 25^(@)C is

The emf of the following cell: Cd(s)| CdCl_(2) (0.10M)|AgCl(s)Ag(S) Is 0.6915V at 0.6753V at 25^(@) C . The DeltaH of reaction in KJ at 25^(@)C is

The standard potential for the reaction, Cl_(2)(g) + 2Br^(-)(aq) rightarrow Br_(2)(l) + 2Cl^(-)(aq) is 0.283 volts. What is the equilibrium consant for this reaction at 25^(@) C?

The standard E.M.F. for the cell reaction: Zn(s) + Cu^(2+) (aq) - Zn^(2+) (aq) + (Cu) is 1.10 volts at 25^(@) C. The EMF. For the cell reaction when 0.01 M Cu^(2+) and 0.1 M Zn^(2+) solutions are used at 25^(@) C is: