In compound A,1.00 , g nitrogen unites with 0 | vedclass

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(B) According to the question:Compound $A \Rightarrow 1.00 \, g$ of $N$ combines with $0.57 \, g$ of $O$.Compound $B \Rightarrow 2.00 \, g$ of $N$ com

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Law of multiple proportion

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(B) According to the question:Compound $A \Rightarrow 1.00 \, g$ of $N$ combines with $0.57 \, g$ of $O$.Compound $B \Rightarrow 2.00 \, g$ of $N$ combines with $2.24 \, g$ of $O$. Thus,$1.00 \, g$ of $N$ combines with $\frac{2.24}{2} = 1.12 \, g$ of $O$.Compound $C \Rightarrow 3.00 \, g$ of $N$ combines with $5.11 \, g$ of $O$. Thus,$1.00 \, g$ of $N$ combines with $\frac{5.11}{3} \approx 1.70 \, g$ of $O$.The ratio of masses of oxygen that combine with a fixed mass $(1.00 \, g)$ of nitrogen in compounds $A, B,$ and $C$ is $0.57 : 1.12 : 1.70$,which simplifies to approximately $1 : 2 : 3$.Since the ratio is a simple whole number,these results obey the Law of Multiple Proportions.

Mass of dinitrogen	Mass of dioxygen
$14 \ g$	$16 \ g$
$14 \ g$	$32 \ g$
$28 \ g$	$32 \ g$
$28 \ g$	$80 \ g$

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:

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The following data are obtained when dinitrogen and dioxygen react together to form different compounds:

Mass of dinitrogen Mass of dioxygen

$14 \ g$ $16 \ g$

$14 \ g$ $32 \ g$

$28 \ g$ $32 \ g$

$28 \ g$ $80 \ g$

Which law of chemical combination is obeyed by the above experimental data?

"Mass can neither be created nor destroyed" is the statement of

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