In a compound A, $1.00 g$ of nitrogen combines with $0.57 g$ of oxygen. In a compound B, $2.00 g$ of nitrogen combines with $2.24 g$ of oxygen. In a compound C, $3.00 g$ of nitrogen combines with $5.11 g$ of oxygen. These data shows which of the following laws?

Law of constant proportions

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Law of multiple proportions

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Law of reciprocal proportions

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Dalton’s law of partial pressure

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Solution

The correct option is B Law of multiple proportions
According to the question,
$C o m p o u n d A \Rightarrow 1 g o f N_{2} + 0.57 g o f O_{2}$
$C o m p o u n d B \Rightarrow 2 g o f N_{2} + 2.24 g o f O_{2}$
$∴ 1 g$ of $N_{2}$ will require $\frac{1 \times 2.24}{2} = 1.12 g$ of $O_{2}$
$C o m p o u n d C \Rightarrow 3 g o f N_{2} + 5.11 g o f O_{2}$
$∴ 1 g$ of $N_{2}$ will require $\frac{1 \times 5.11}{3} = 1.70 g$ of $O_{2}$
The ratio of $O_{2} i n A, B a n d C = 0.57 ∶ 1.12 ∶ 1.7 \approx 1 : 2 : 3$
Therefore, the given results obey the law of multiple proportions.

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Similar questions

Q. In a compound A,

1.00 g

of nitrogen combines with

0.57 g

of oxygen. In a compound B,

2.00 g

of nitrogen combines with

2.24 g

of oxygen. In a compound C,

3.00 g

of nitrogen combines with

5.11 g

of oxygen. These data shows which of the following laws?

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