An element forms two oxides containing, respectively, 50% and 40% by weight of the element. These oxides illustrate the:

Law of constant composition

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Law of multiple proportion

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Law of reciprocal proportion

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None of these

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Solution

The correct option is B Law of multiple proportion
In one oxide,
$50$ g of element combines with $50$ g of oxygen.

Therefore, $1$ g of an element will combine with $1$ g of oxygen.

In the other oxide,
$40$ g of element combines with $60$ g of oxygen.

Therefore, $1$ g of element will combine with $\frac{64}{40}$ or $1.5$ g of oxygen.

Thus, the weights of oxygen that combine with $1$ g of the element in the two oxides are in the ratio of $1 : 1.5$ or $2 : 3$ ; which is a simple ratio.

This illustrates the law of multiple proportions.

Hence, option $B$ is correct.

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