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Law of definite proportions - class-VIII
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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, 2.9 g of iron oxide gave 2.09 g of iron on reduction. Which law is illustrated from the above data?
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A
Law of constant proportions
💡 Explanation:
In experiment 1,
$2.4\ g$ of iron oxide gives $1.68\ g$ iron on reduction with hydrogen.
$FeO \rightarrow Fe+O _2$
Percent of $Fe$ in $FeO$ is = $\frac{1.68}{2.4} \times 100=70$
Therefore ratio of $m _{Fe}:m _{O}::7:3$
In experiment 2:
$2.9\ g$ of iron oxide gives $2.09\ g$ iron on reduction.
Percent of $Fe$ in $FeO$ is = $\frac{2.09}{2.9} \times 100=72$
Therefore ratio of $m _{Fe}:m _{O} \approx 7:3$
When a given chemical compound contains its component elements in fixed ratio (by mass) and does not depend on its source and method of preparation, it follows law of constant proportion.
option A is correct