In an experiment, $2.4 g$ of iron oxide on reduction with hydrogen gave $1.68 g$ of iron. In another experiment, $2.69 g$ of iron oxide gave $1.88 g$ of iron on reduction. Which law is illustrated from the above data?

Law of constant proportions

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Law of multiple proportions

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Law of reciprocal proportions

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Law of conservation of mass

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Solution

The correct option is A Law of constant proportions
In the first experiment,
$2.4 g$ of iron oxide gave $1.68 g$ of iron.
Mass of iron oxide $= 2.4 g$
Mass of iron $= 1.68 g$

$∴$ Mass of oxygen $= 2.4 - 1.68 = 0.72$
The ratio of masses of iron and oxygen $= \frac{1.68}{0.72} = 7 : 3$

In the second experiment,
Mass of iron oxide $= 2.69 g$
Mass of iron $= 1.88 g$
Mass of oxygen $= 2.69 - 1.88 = 0.81$
The ratio of masses of iron and oxygen $= \frac{1.88}{0.81} = 7 : 3$
The same ratio confirms that these experiments clarify Law of constant proportion.
Hence, option $A$ is correct.

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In an experiment, 2.4 g of iron oxide on reduction with hydrogen gave 1.68 g of iron. In another experiment, 2.69 g of iron oxide gave 1.88 g of iron on reduction. Which law is illustrated from the above data?

In an experiment, $2.4 g$ of iron oxide on reduction with hydrogen gave $1.68 g$ of iron. In another experiment, $2.69 g$ of iron oxide gave $1.88 g$ of iron on reduction. Which law is illustrated from the above data?