A gaseous compound of nitrogen and hydrogen contains 12.5 \% (by mass) of hydrogen. The density of the compound relative to hydrogen is 16. The molecular formula of the compound is:

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Correct answer: D. N_2 H_4

In an unknown compounds containing N and H given \% of H=12.5 \% \% of N=100-12.5=87.5 \% Element Percentage Atomic ratio Simple ratio H 12.5 \% (12.5)/(1)= 12.5 (12.5)/(6.25)= 2 N 87.5 (87.5)/(14)= 6.25 (6.25)/(6.25)= 1 2 × vapour density = Mol. wt =16 × 2=32 . Molecular formula =n × empirical formula mass n= (32)/(16)= 2 Molecular formula of the compound will be =(NH_2)_2 =N_2 H_4

A gaseous compound of nitrogen and hydrogen contains 12.5 \% (by...

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More from Some Basic Concepts of Chemistry

Element	Percentage	Atomic ratio	Simple ratio
H	12.5 \%	$\frac{12.5}{1}=$ 12.5	$\frac{12.5}{6.25}=$ 2
N	87.5	$\frac{87.5}{14}=$ 6.25	$\frac{6.25}{6.25}=$ 1