Calculate the electrode potential at a copper electrode dipped in a 0.1 M solution of copper sulphate at `25^(@)C`. The standard electrode potential of `Cu^(2+)//Cu` system is 0.34 volt at 298 K.

Calculate the electrode potential at a copper electrode dipped in 0.1 M solution of copper sulphate at 25^@C . Given, the standard emf of Cu^(2+) system is +0.34V at 298K.

Calculate the electrode potential of a copper electrode dipped in 0.1M solution of copper sulphate at 25^@C . (Given E^@ for Cu is +0.34V at 298K)

Calculate the electrode potential at copper electrode dipped in a 0.1 M solution of copper sulphate at 298K, assuming CuSO_4 to be completely ionised. The standard electrode potential of Cu^(2+)|Cu is 0.34V at 298K.

Calculate the electrode potential of a copper wire dipped in "0.1M CuSO"_(4) solution at 025^(@)C . The standard electrode potential of copper is 0.34 Volt.

Calculate the electrode potential of a copper wire dipped in 0.1M CuSO_4 solution at 298 K. The standrd electrode potential of copper is +0.34 volt.

What is the single electrode potential of a half-cell for zinc electrode dipping in 0.01 M ZnSO_(4) solution at 25^(@)C ? The standard electrode potential of Zn//Zn^(2+) system is 0.763 volt at 25^(@)C .

The standard electrode potential of Cu^(2+)|Cu half cell is +0.34V . What does it mean?

(a) Calculate the potential of Zn^(2+)//Zn electrode in which zinc ion activity is 0.001 M. mol^(-1),=96500 C mol^(-1), E_(Zn^(2+)//Zn)^(@)=-0.76" V ") (b) Calculate the electrode potential of copper electrode dipped in a 0.1 M solution of copper sulphate at 298 K, assuming CuSO_(4) to be completely ionised. The standard reduction potential of copper , E_(Cu^(2+)//Cu)^(@)=0.34" V " at 298 K.