A galvanic cell consists of a metallic zinc plate immersed in 0.1 M `Zn(NO_(3))_(2)` solution. Calculate the emf of the cell at `25^(@)C`. Write the chemical equations for the electrode reactions and represent the cell. (Given : `E_(Zn^(2+)//Zn)^(@) = - 0.76` volt and `E_(Pb^(2+)//Pb)^(@) = - 0.13` volt)

Answer

`Zn rarr Zn^(2+) + 2e^(-)," "Pb^(2+)+2e^(-) rarr Pb`
`Zn|underset(0.1 M)(Zn^(2+))||underset(0.02 M)(Pb^(2+))|Pb`
`E_(cell)^(@)=0.63" volt "E_(cell)=0.609" volt"`