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.

Calculate the standard potential of the cell ,If the standard electrode potentials of Zn^(2+)//Zn and Ag^(+) //Ag are -0.763 V and + 0.799 V respectively .

Standard reduction electrode potential of Zn^(2+)//Zn is -0.76V . This means:

The standard reduction potential for Zn^(2+)//Zn, Ni^(2+)//Ni and Fe^(2+)//Fe are -0.76, -0.23 and -0.44V respectively. The reaction X + Y^(2) rarr X^(2+) + Y will be spontaneous when:

The standard reduction potential of Pb and Zn electrodes are -0.12 6 and -0.763 volts respectively . The e.m.f of the cell Zn|Zn^(2+)(0.1M)||Pb^(2+)(1M)|Pb is

E^(c-) of Mg^(2+)|Mg,Zn^(2+)|Zn , and Fe^(2+)|Fe are -2.37V,-0.76V , and -0.44V , respectively. Which of the following is correct ?

E^(c-) of Mg^(2+)|Mg,Zn^(2+)|Zn , and Fe^(2+)|Fe are -2.37V,-0.76V , and -0.44V , respectively. Which of the following is correct ?

The standard reduction potential for Zn^(2+)//Zn is -0.76V. Write the reactions occurring at the electrodes when coupled with NHE or SHE.

The emf of the cell Zn|Zn^(2+) (1 M)||Cu^(2+)|Cu(1M) is 1.1 volt. If the standard reduction potential of Zn^(2+)|Zn is -0.78 volt, what is the standard reduction potential of Cu^(2+)|Cu

The oxidation ptentials of Zn, Cu, Ag, H_2 and Ni are 0.76, - 34, - 0.80 . 0. 00, 0. 25 volt, respectively. Which of the following reactions will provide maximum voltage ?

(a) A cell is prepared by dipping a zinc rod in 1M zinc sulphate solution and a silver electrode in 1M silver nitrate solution. The standard electrode potential given : E^(@)Zn_(2+1//Zn) = -0.76V, E^(@)A_(g+//)A_(g) = +0.80V What is the effect of increase in concentration of Zn^(2+) " on the " E_(cell) ? (b) Write the products of electrolysis of aqueous solution of NaCI with platinum electrodes. (c) Calculate e.m.f. of the following cell at 298 K: "Ni(s)"//"Ni"^(2+)(0.01M)////"Cu"^(2+)(0.1M)//"Cu(s)" ["Given"E_(Ni2+//Ni)^(@) = -0.025 V E_(Cu2+//Cu)^(@) = +0.34V] Write the overall cell reaction.