Assertion: The masses of oxygen that combine with a fixed mass of nitrogen in NO, NO₂, N₂O₃, and N₂O₄ are in the ratio 1:2:3:4.
Reason: Nitrogen and oxygen combine to form only two types of oxides.

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Both assertion and reason are correct, and reason is the correct explanation for assertion.

Both assertion and reason are correct, but reason is not the correct explanation for assertion.

Assertion is correct, but reason is incorrect.

Both assertion and reason are incorrect.

answer is C.

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Detailed Solution

The assertion is correct because when we look at the oxides of nitrogen (like NO, NO₂, N₂O₃, and N₂O₄), they exhibit a simple whole-number ratio for the masses of oxygen combining with a fixed amount of nitrogen. For example, if we have a certain amount of nitrogen (say 28 grams), the amounts of oxygen in these compounds can follow a ratio of 1:2:3:4.

The reason is incorrect because nitrogen and oxygen do not just form two types of oxides. They can form several oxides, including NO, NO₂, N₂O, N₂O₃, N₂O₄, and N₂O₅. This variety in compounds is part of why the law of multiple proportions is relevant.

Thus, while the assertion is true (the masses of oxygen are in a simple ratio), the reason incorrectly suggests there are only two oxides of nitrogen, which makes the reason incorrect.

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