Chemistry - Electrochemistry Question with Solution | TestHub

For a Zn-Cu cell, zinc acts as the anode (undergoes oxidation) and copper acts as the cathode (undergoes reduction).

The standard emf of the cell is given by:

$E_{\text{cell}}^{\circ }=E_{\text{cathode}}^{\circ }-E_{\text{anode}}^{\circ }$

Substituting the given standard reduction potentials:

$E_{\text{cell}}^{\circ }=E^{\circ }({\text{Cu}}^{2+}/\text{Cu})-E^{\circ }({\text{Zn}}^{2+}/\text{Zn})$

$E_{\text{cell}}^{\circ }=0.34-(-0.76)$

$E_{\text{cell}}^{\circ }=0.34+0.76=1.1$ V

Answer: $1.1$ V