Zinc is used to protect iron from corrosion because zinc is

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more electropositive than iron

cheaper than iron

a bluish white metal

a good conductor of heat and electricity

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Answer is Wrong!

This question was previously asked in

UPSC NDA-2 – 2017

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Zinc is used to protect iron from corrosion through a process called galvanization. Zinc protects iron because it is more electropositive (or more reactive) than iron. In the electrochemical series, zinc is placed above iron, meaning it loses electrons more easily and has a higher tendency to be oxidized. When both metals are present in the presence of an electrolyte (like moisture), zinc acts as the anode and corrodes sacrificially, while iron acts as the cathode and is protected from oxidation (rusting). Even if the zinc coating is scratched and iron is exposed, the zinc in contact with the electrolyte will still corrode preferentially, providing galvanic protection to the iron.

– Zinc is more electropositive/reactive than iron.
– Zinc acts as a sacrificial anode, corroding instead of iron.
– Provides protection even if the coating is scratched (galvanic protection).

Other methods of protecting iron from rusting include painting, greasing, plating with less reactive metals (like tin, although this doesn’t provide sacrificial protection if scratched), and alloying (like stainless steel). Galvanization is a very effective and widely used method due to zinc’s sacrificial nature.

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