Question

Explain why metals are always deposited at the cathode, rather than the anode, during electrolysis.​

Answer 1

Answer:

During electrolytic reduction, the metals are deposited at the cathode (the negatively charged electrode).

Electrolytic reduction is a type of electrolysis in which electric current is passed through an ionic substance (molten or dissolved ), producing a chemical reaction at the electrodes and decomposing the materials.

It is used for highly electropositive metals like Potassium, which cannot get reduced in aqueous solutions.

For example electrolysis of sodium chloride is taken

NaCl → Na +(l) + Cl–(l)

At cathode: reduction of 2Na+(l) + e– → Na(l)

At anode: oxidation of 2Cl–(l) → Cl2(g) + 2e–

Net Reaction is written as: 2Na +(l) + 2Cl–(l) → 2Na(l) + Cl2(g)

Answer 2

During electrolytic reduction, the metals are deposited at the cathode (the negatively charged electrode). ... It is used for highly electropositive metals like Potassium, which cannot get reduced in aqueous solutions.