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 :

Question

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 : (A) NH2 (B) N3H (C) NH3 (D) N2H4

Tardigrade Admin · Accepted Answer

N H Mass % 87.5 12.5 Mol (87.5/14) (12.5/1) =6.25 =12.5 1 2 Empirical formula = NH2 Since Vapour density = 16 ∴ mol. wt. = 32 ∵ Molecular formula = n x Emp. formula =2× NH2 =N2 H4

Q. 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 :

$N H_{2}$

$N_{3} H$

$N H_{3}$

$N_{2} H_{4}$

N H

Mass % 87.5 12.5

Mol $\frac{87.5}{14}$ $\frac{12.5}{1}$

=6.25 =12.5

1 2

Empirical formula = $N H_{2}$

Since Vapour density = 16

$∴$ mol. wt. = 32

$∵$ Molecular formula = n x Emp. formula

$= 2 \times N H_{2}$

$= N_{2} H_{4}$

	N	H
Mass %	87.5	12.5
Mol	$\frac{87.5}{14}$	$\frac{12.5}{1}$
	=6.25	=12.5
	1	2

Q. 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 :

NH2​

N3​H

NH3​

N2​H4​

N H Mass % 87.5 12.5 Mol 1487.5​ 112.5​ =6.25 =12.5 1 2 Empirical formula = NH2​ Since Vapour density = 16 ∴ mol. wt. = 32 ∵ Molecular formula = n x Emp. formula =2×NH2​ =N2​H4​

$N H_{2}$

$N_{3} H$

$N H_{3}$

$N_{2} H_{4}$

N H

Mass % 87.5 12.5

Mol $\frac{87.5}{14}$ $\frac{12.5}{1}$

=6.25 =12.5

1 2

Empirical formula = $N H_{2}$

Since Vapour density = 16

$∴$ mol. wt. = 32

$∵$ Molecular formula = n x Emp. formula

$= 2 \times N H_{2}$

$= N_{2} H_{4}$