The standerd potential at `25^(@)` for the following Half rection is given :
`Zn^(2+)+2e^(-)toZn,E^(@)=-0.762 V`
`Mg^(2+)+2e^(-)toMg,E^(@)=-2.37 V`
When Zinc dust is added to the solution of `MgCl_(2)`.

The standard Potentials at 25^@C for the half reactions are given against them below: Zn^(2+) + 2e^(-) to Zn,E^@ = -0.762V Mg^(2+) + 2e^(-) to Mg, E^@ = -2.37V When Zn dust is added to a solution of MgCl_2

The standard potentials at 25^@C for the following half reactions are given against them Zn^(2+) +2e^(-) rarr Zn, E^0 =-0 . 762 V Mg^(2+) +2e^(-) rarr Mg, =- 2.37 V . When zinc dust is added to a solution of magnesium chloride .

The standard potential E^(@) for the half reactions are as : Zn rarr Zn^(2+) + 2e^(-), E^(@) = 0.76V Cu rarr Cu^(2+) +2e^(-) , E^(@) = -0.34 V The standard cell voltage for the cell reaction is ? Zn +Cu^(2) rarr Zn ^(2+) +Cu

The standard potential E^(@) for the half reactions are as : Zn rarr Zn^(2+) + 2e^(-), E^(@) = 0.76V Cu rarr Cu^(2+) +2e^(-) , E^(@) = -0.34 V The standard cell voltage for the cell reaction is ? Zn +Cu^(2) rarr Zn ^(2+) +Cu

The standard potential (E^(0)) for the half reaction are as Zn to Zn^(2+) + 2e^(-) , E^(0) = + 0.76 V Fe to Fe^(2+) + 2e^(-) , E^(0) = + 0.41 V . The emf for the cell reaction Fe^(2+) + Zn to Zn^(2+) + Fe is