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Calculate the standard reduction potential of `Cd^(2+)//Cd` electrode for the cell : `Zn(s)|Zn^(2+)("IM") || Cd^(2+)(IM)|Cd(s)` `("Given that " E_(cell)^(@)=0.36 V and E_(Zn^(2+)//Zn)^(@)=-0.76V)` |
Answer» `E_(cell)^(@)=E_(cathode)^(@)-E_(anode)^(@)` `E_(cell)^(@)=(E_(Cd^(2+)//Cd)^(@))-(E_(Zn^(2+)//Zn)^(@))` `(E_(Cd^(2+)//Cd))=E_(cell)^(@)+(E_(Zn^(2+)//Zn)^(@))=0.36+(-0.76)=-0.40 V` |
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