Statement I : Zinc is used for galvanization to protect iron of from rusting. Statement I : Zinc is more reactive towards oxygen than iron.

Statement I is true as galvanization is a standard method for protecting iron and steel from rusting by applying a thin coating of zinc [2]. Statement II is also true because zinc is higher in the reactivity series than iron, meaning it is more reactive and has a greater affinity for oxygen. This higher reactivity is the fundamental reason why zinc acts as a sacrificial anode [1]. Even if the zinc coating is scratched or broken, the zinc corrodes preferentially (oxidizes) to protect the underlying iron cathodically [3]. Because zinc reacts more readily with oxygen and moisture than iron does, it effectively 'sacrifices' itself to prevent the oxidation of the iron. Thus, Statement II provides the correct scientific explanation for why zinc is used in the galvanization process described in Statement I.

Sources

1. [1] Science , class X (NCERT 2025 ed.) > Chapter 3: Metals and Non-metals > 3.5.1 Prevention of Corrosion > p. 54
2. [2] Science-Class VII . NCERT(Revised ed 2025) > Chapter 4: The World of Metals and Non-metals > Activity 4.5: Let us experiment > p. 50
3. [3] https://en.wikipedia.org/wiki/Galvanic_corrosion