Question
SLPaper 2
Molten zinc chloride undergoes electrolysis in an electrolytic cell at 450 °C.
1.[2]
Deduce the half-equations for the reaction at each electrode.
Verified
Solution
Cathode (negative electrode):
Zn2+ + 2e− → Zn (l) ✔
Anode (positive electrode):
2Cl− → Cl2 (g) + 2e−
OR
Cl− → ½ Cl2 (g) + e− ✔
2.[2]
Deduce the overall cell reaction including state symbols. Use section 7 of the data booklet.
Verified
Solution
ZnCl2 (l) → Zn (l) + Cl2 (g)
balanced equation ✔
correct state symbols ✔
Accept ionic equation.
