Question

A mixture of $C{H}_4,N_2$ and $O_2$ is enclosed in a vessel of one litre capacity at $0^{o}C$. The ratio of pressure of gases is $1:4:2$. Total pressure of the gaseous mixture is $2660mm$. The molecules of oxygen present in the vessel is

• A. $\frac{0.02\times {10}^{23}}{22.4}$
• B. $4.02\times {10}^{23}$
• C. $22.4\times {10}^{22}$
• D. $1000$

Answer 1

The correct option is A $\frac{0.02\times {10}^{23}}{22.4}$

Partial pressure of $O_2=\frac{2}{7}\times 2660=760mm.$

Thus $1L$ of $O_2$ is present at $0^{0}C$ and $760mm$ pressure$.$

So$,$ no$.$ of $O_2$ molecules $=\frac{0.02\times {10}^{23}}{22.4}$

Hence,

option $\left(A\right)$ is correct answer.