Home › UP Board Class 12 › chemistry › Electrochemistry › GALVANISATION protects iron from rusting by coat…
GALVANISATION protects iron from rusting by coating it with:
ATin (Sn), which is less reactive than the iron underneath
BCopper (Cu), which is more noble metal than the iron beneath
CZinc (Zn), the more reactive metal as sacrificial anode
DGold (Au), which never tarnishes in normal atmospheric air
Answer & Solution
Correct answer: C. Zinc (Zn), the more reactive metal as sacrificial anode
GALVANISATION = coating iron with ZINC. Zn is more reactive than Fe (more negative E°), so Zn oxidises preferentially, sacrificing itself to protect the iron underneath. Even if the coat is scratched, Zn still corrodes first (cathodic protection).
Related questions
For an electrochemical cell operating spontaneously, ΔG° is related to E°_cell byWhich of the following statements about electrode potentials is INCORRECT?The overall cell reaction of the lead storage battery on discharge isThe primary cell that cannot be reused after its EMF drops to zero is exemplified byRusting of iron requires which two chemicals in contact with the metal?Fuel cells directly convertThe specific conductivity of a 0.1 M KCl solution is 1.29 × 10⁻² S/cm. The molar conductivMolar conductivity of a strong electrolyte at concentration c is related to its limiting v