Consider the following reaction 2H2 g O2 g gt 2H2O l Which one of the following ...........

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Consider the following reaction:

2H₂(g) + O₂ (g) ---> 2H₂O (l)

Which one of the following statements about the reaction given above is correct?

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The oxidation state of hydrogen increases while that of oxygen decreases

The oxidation state of hydrogen decreases while that of oxygen increases

There is no change in the oxidation state of hydrogen as well as that of oxygen

During the reaction, hydrogen is reduced while oxygen is oxidized

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Explanation:

Let’s break down the options for the reaction:

2H2(g) + O2(g) ? 2H2O(l)

- In H2: The oxidation state of H is 0.

- In O2: The oxidation state of O is 0.

- In H2O: H is +1, O is -2.

Option 1: The oxidation state of hydrogen increases while that of oxygen decreases.

- ?? Incorrect. H goes from 0 to +1 (oxidation increases), O from 0 to -2 (oxidation decreases). The statement about H increasing is correct, but for oxygen, it should be decreasing (more negative means decrease, but statement direction is off).

Option 2: The oxidation state of hydrogen decreases while that of oxygen increases.

- ?? Incorrect. H is oxidized (0 to +1), O is reduced (0 to -2).

Option 3: There is no change in the oxidation state of hydrogen as well as that of oxygen.

- ?? Incorrect. Changes occur for both elements.

Option 4: During the reaction, hydrogen is reduced while oxygen is oxidized.

- ?? Incorrect. H is oxidized, O is reduced.

Correct Answer:

- Option 1 is *mostly* correct regarding the direction of change, but in chemistry, "oxidation state increases" means becoming more positive (H: 0 ? +1, so increase) and "decreases" means becoming more negative (O: 0 ? -2, so decrease). Therefore, Option 1 is the BEST match.