Zinc granules are added in excess to 500 mL of 1M `Ni(NO_(3))_(2)` solution of `25^(@)C` untill the equilibrium is reached. If `E_(Zn^(2+)//Zn)^(@)` and `E_(Ni^(2+)//Ni)^(@)` are `-0.75V` and `-0.24V` respectively, find out the `[Ni^(2+)]` at equilibrium.

Zn - granules are added in excess to 500 mL of 1.0 M nicke nitrate solution at 25^(@)C until the equilibrium is reached. If standard reduction potential of Zn^(2+)|Zn and Ni^(2+)|Ni are -0.75V and -0.24V , respectively, find out the concentration of Ni^(2+) in solution at equilibrium.

Zinc granules are added in excess to 500mL OF 1.0m nickel nitrate solution at 25^(@)C until the equilibrium is reached. If the standard reduction potential of Zn^(2+)|Zn and Ni^(2+)|Ni are -0.75V and -0.24V , respectively, find out the concentration of Ni^(2+) in solution at equilibrium.

Zinc granules are added in excess to 500mL OF 1.0m nickel nitrate solution at 25^(@)C until the equilibrium is reached. If the standard reduction potential of Zn^(2+)|Zn and Ni^(2+)|Ni are -0.75V and -0.24V , respectively, find out the concentration of Ni^(2+) in solution at equilibrium.

Given E_(Ag^(+)//Ag)^(@) = +0.8V , E_(Ni^(+2)//Ni)^(@) = -0.25V . Which of the folowing statements is true?

Write Nernst equation and find e.m.f of cell Ni//Ni_((0.01M))^(2+)//Cu_((1M))^(2+)//Cu_() . Given E_(Cu^(2+)//Cu)^(@)= 0.34V, E_(Ni^(2+)//Ni)^(@)= -0.22V

Calculate the emf of the cell at 298K E_(NI^(2+)//NI)^0 is -0.25V and E_(Ag^+//Ag)^0 is +0.80V .

E^(@) values of Ni^(2+)//Ni and Cu^(2+)//Cu are -0.25 V and +0.34 V respectively. Is the reaction: Ni+Cu^(2+)toNi^(2+)+Cu spontaneous or not ? Give reason also.