Question

In compound $A, 1.00\, g$ nitrogen unites with $0.57\, g$ oxygen. In compound $B, 2.00 \,g$ nitrogen combines with $2.24 \,g$ oxygen. In compound $C, 3.00\, g$ nitrogen combines with $5.11 \,g$ oxygen. These results obey the following law

• A. Law of constant proportion
• B. Law of multiple proportion
• C. Law of reciprocal proportion
• D. Dalton’s law of partial pressure

Answer 1

Answer: (B)

Here, According to the question
Compound $A : 1.00\, g\, N +0.57\, g\, O _{2}$
Compound $B: 2.00\, g\, N +2.24\, g\, O _{2}$
Compound $C : 3.00\, g\, N +5.11\, O _{2}$
So If we fixed the amount of nitrogen $(1\, g)$ for all compound then,
Compound A:
$1.00\, g$ of $N$ combine with $0.57\, g$ of $O _{2}$
Compound B :
$2\, g\, N$ of $N$ combine with $2.24\, g$ of $O _{2}$
$1\,N =1.12\, g\, O _{2}$
Compound C:
$3\, g\, N$ combine with $5.11\, O _{2}$
$1\, g\, N =1.70\, g\, O _{2}$
Thus,
Take in consideration the ratio of oxygen of all three compounds for the fixed amount of Nitrogen then we get
Ratio of oxygen $\approx 1: 2: 3$
This ratio indicates the law of multiple proportion.