Following are the values of standard potentials of two half cells, which of the following will be the value of standard cell potential `(E_("cell")^(@))`
`Ni^(2+)//Ni: E^(@)=-0.25V`
`Zn^(2+)//Zn: E^(@)=+0.77V`

The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

Calculate the standard electrode potential of the Ni^(2+)//Ni electrode , if the cell potential potential of the cell, Ni//N^(2+)(0.01 M)//Cu is 0.59" V ". "Given" E_(Cu^(2+)//Cu)^(@)=+0.34 " V "

Calculate the voltage of following electrochemical cell under standard conditions. Name anode and cathode in each cell. (i) Zn - Ag (ii) Co - Ni. The standard reduction potentials of various half cells are: Zn^(2+)//Zn =-0.76V, Ag^(+)//Ag= +0.80V Co^(2+)//Co = -0.28V, Ni^(2+)//Ni= -0.25V

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 .

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 .

The standard cell potential for the cell is , Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu [E^@ for Zn^(2+)//Zn=-0.76V, E^@ for Cu^(2+)//Cu=+0.34V]

Calculate the EMF of the electrochemical cell for which the following cell reaction is given below- Zx(S) + ni^(2_+)(aq) rarr Zn^(+2)(aq) + Ni(S) Given E_(zn^2//zn)^@ = - 0.76 V E_(Ni^(2+) // Nl) = - 0.25 V.

Calculate standard cell potential of following galvanic cell Zn//Zn^(2)+(1 M) // Pb^(2)+(1 M)//Pb . If E_(Pb)^(0) = 0.126V and E_(Zn)^(0) = -0.763V