In the redox reaction Sn(s) + 2 HCl(aq) → SnCl2(aq) + H2(g), which element is oxidized?

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Multiple Choice

In the redox reaction Sn(s) + 2 HCl(aq) → SnCl2(aq) + H2(g), which element is oxidized?

Explanation:
The test is about changes in oxidation states during a redox reaction: oxidation means a loss of electrons and a rise in oxidation state, while reduction means a gain of electrons and a fall in oxidation state. In this reaction, tin starts as elemental tin with an oxidation state of 0 and ends up as Sn2+ in SnCl2, so its oxidation state increases from 0 to +2. That loss of electrons shows tin is oxidized. Hydrogen in HCl starts at +1 and ends as H2 with oxidation state 0, which means it gains electrons and is reduced. Chlorine stays at -1 on both sides, so it doesn’t undergo a redox change. Thus, tin is the element that is oxidized.

The test is about changes in oxidation states during a redox reaction: oxidation means a loss of electrons and a rise in oxidation state, while reduction means a gain of electrons and a fall in oxidation state.

In this reaction, tin starts as elemental tin with an oxidation state of 0 and ends up as Sn2+ in SnCl2, so its oxidation state increases from 0 to +2. That loss of electrons shows tin is oxidized. Hydrogen in HCl starts at +1 and ends as H2 with oxidation state 0, which means it gains electrons and is reduced. Chlorine stays at -1 on both sides, so it doesn’t undergo a redox change.

Thus, tin is the element that is oxidized.

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