Zinc is used to protect iron from corrsion because zinc is

Options

A. more electropositive than iron
B. cheaper than iron
C. a bluish white metal
D. a good conductor of heat and electricity

Explanation

**Step-by-Step Solution:**

1. **Understanding Corrosion**: Corrosion is a chemical process where metals react with environmental factors (like oxygen and moisture) leading to deterioration. For iron, this often results in rusting, which is primarily iron oxide.

2. **Role of Zinc**: Zinc is used to protect iron from corrosion. This protection is primarily due to zinc's electrochemical properties.

3. **Electropositivity**: Zinc is more electropositive than iron. Electropositivity refers to the tendency of an element to lose electrons. The more electropositive an element is, the more readily it can lose electrons.

4. **Galvanization Process**: The method of protecting iron by coating it with zinc is known as galvanization. In this process, a layer of zinc is applied to the surface of iron, which acts as a sacrificial anode.

5. **Sacrificial Anode Principle**: Since zinc is more electropositive, it will oxidize (lose electrons) before iron does. This means that even if the zinc layer is scratched, zinc will corrode instead of iron, thus protecting the iron from rusting.

6. **Conclusion**: Therefore, zinc is used to protect iron from corrosion because it is more electropositive than iron, allowing it to lose electrons more readily and thus prevent rust formation on iron.

**Final Answer**: Zinc is used to protect iron from corrosion because zinc is more electropositive than iron.

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