Chemistry – Physical chemistry | e-Consult

a) Standard Cell Potential:

The standard cell potential (E^o_cell) is calculated as:

E^o_cell = E^o_cathode - E^o_anode

In this case, the cathode is the Cu²⁺/Cu(s) half-cell (reduction) and the anode is the Zn²⁺/Zn(s) half-cell (oxidation). Therefore:

E^o_cell = +0.34 V - (-0.76 V) = +1.10 V

b) Effect of [Zn²⁺]:

According to the Nernst equation, the cell potential is affected by the concentration of the ions. Increasing the concentration of Zn²⁺ will increase the cell potential. This is because the reaction at the zinc anode (oxidation) will be driven more towards completion, leading to a greater tendency for electrons to be released and contribute to the overall cell potential. The Nernst equation shows the relationship between cell potential and ion concentration.