Calculate emf of the following cell reaction at 2968 K :
`Ni(s)//Ni^(2+)(0.01 M) || Cu^(2+)(0.1 M)//Cu(s)`
[Given `E_(Ni^(2+)//Ni)^(@)=-0.25" V ",E_(Cu^(2+)//Cu)^(@)=+0.34 " V "`]
Write the overall cell reaction.

(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.

Calculate equilibrium constant for the reaction : Mg(s) |Mg^(2+)(0.001 M) || Cu^(2+)(0.0001 M)|Cu(s) Given E_((Mg^(2+)//Mg))^(@)=-2.37" V " , E_((Cu^(2+)//Cu))^(@)=0.34" V "

Find the e.m.f. of the cell, Mg(s)//Mg^(2+)(0.01 M) || Cu^(2+)(aq)(0.0001 M)//Cu(s) "Given" E_(Mg^(2+)//Mg)^(@)=-2.37 " volts" , E_(Cu^(2+)//Cu)^(@)=+0.34" volts" .

Calculate the e.m.f of the cell Mg(s)//Mg^(2+)(0.1 M)||Cu^(2+)(1.0xx10^(-3) M)//Cu(s) Given E_(Cu^(2+)//Cu)^(@)=+0.34 V and E_(Mg^(2+)//Mg)^(@)=-2.37 V

What is the cell potential for following cell Zn(s)//Zn^(2+)(0.04M||Cu^(2+)(0.02M)//Cu(s) Given E_(Zn//Zn^(2+))^@ = -0.76V & E_(Cu//Cu^(2+))^@ = 0.34V

Calculate the e.m.f. of the cell in which the following reaction takes place : Ni(s) +2Ag^(+)(0.002 M)to Ni^(2+)(0.160 M)+2Ag(s) Given E_(cell)^(@) =1.05 v

Calculate EMF of following cell at 298 K Zn|ZnSO_(4) (0.1 M) ||CuSO_(4) (1.0 M)|Cu (s) if E_(cell) = 2.0 V