Question

Explain the electrochemical process of rusting of iron with the help of given points 1) cathode and anode in the
process
2) Reaction at anode 3) Reaction at cathode​

Answer 1

Answer:

1) Rust (Fe2O3•xH2O) is formed by the subsequent oxidation of Fe2+ by atmospheric oxygen. In the corrosion process, iron metal acts as the anode in a galvanic cell and is oxidized to Fe2+; oxygen is reduced to water at the cathode. ...

2) at cathode: O2(g)+4H(aq)+4e−→2H2O(l)E°=1.23V.

3) at anode: Fe(s)→Fe2(aq)+2e− E°=−0.45V.

Answer 2

Answer : (a) Chemical formula of rust: Fe2O3.xH2O

(b) (i) Fe is oxidised to Fe2+ in the anode region. Fe(s) + 2e

(ii) O2 is reduced to form water in the cathode region. O2 (g) + 4H+(aq) + 4e2H20