A gaseous mixture contains oxygen and nitrogen in the ratio 1:4 by weight. The ratio of their number of molecules is

Question

A gaseous mixture contains oxygen and nitrogen in the ratio 1:4 by weight. The ratio of their number of molecules is (A) 1:4 (B) 1:8 (C) 7:32 (D) 3:16

Tardigrade Admin · Accepted Answer

Number of moles of O2=(1/32) and number of mol of N2=(4/28) So ( textNumber textof textmolecules textof textO text2/ textNumber textof textmolecules textN text2) text= ( textNumber textof textmol textof textO text2/ textNumber textof textmol textof textN text2) =(1 / 32/4 / 28)=(1/32)× (28/4) =(7/32)=7:32

Q. A gaseous mixture contains oxygen and nitrogen in the ratio 1:4 by weight. The ratio of their number of molecules is

1:4

1:8

7:32

3:16

Number of moles of $O_{2} = \frac{1}{32}$
and number of mol of $N_{2} = \frac{4}{28}$
So $\frac{Number of molecules of O _{2}}{Number of molecules N _{2}} = \frac{Number of mol of O _{2}}{Number of mol of N _{2}}$
$= \frac{1/32}{4/28} = \frac{1}{32} \times \frac{28}{4}$
$= \frac{7}{32} = 7 : 32$

Q. A gaseous mixture contains oxygen and nitrogen in the ratio 1:4 by weight. The ratio of their number of molecules is

1:4

1:8

7:32

3:16

Number of moles of O2​=321​ and number of mol of N2​=284​ So NumberofmoleculesN2​NumberofmoleculesofO2​​=NumberofmolofN2​NumberofmolofO2​​ =4/281/32​=321​×428​ =327​=7:32

Number of moles of $O_{2} = \frac{1}{32}$
and number of mol of $N_{2} = \frac{4}{28}$
So $\frac{Number of molecules of O _{2}}{Number of molecules N _{2}} = \frac{Number of mol of O _{2}}{Number of mol of N _{2}}$
$= \frac{1/32}{4/28} = \frac{1}{32} \times \frac{28}{4}$
$= \frac{7}{32} = 7 : 32$