The correct answer is option 1: Both the statements are individually true and Statement II is the correct explanation of Statement I.
Statement I states that zinc is used for galvanization to protect iron from rusting. This statement is true. Galvanization is the process of applying a protective zinc coating to iron or steel to prevent rusting. The zinc coating acts as a barrier between the iron and oxygen in the air, preventing the iron from coming into contact with oxygen and water, which are necessary for rust formation.
Statement II states that zinc is more reactive towards oxygen than iron. This statement is also true. Reactivity is a measure of how easily a substance reacts with other substances. Zinc is more reactive than iron because it readily reacts with oxygen to form zinc oxide. This reactivity allows zinc to act as a sacrificial metal in galvanization, meaning it will corrode and protect the iron underneath it from rusting.
Statement II correctly explains why zinc is used for galvanization to protect iron from rusting. Zinc`s higher reactivity towards oxygen allows it to form a protective barrier that prevents the iron from coming into contact with oxygen and water, thus preventing rusting.