At $27^{\circ} C$,$1 \ L$ of $H_2$ with a pressure of $1 \ bar$ is mixed with $2 \ L$ of $O_2$ with a pressure of $2 \ bar$ in a $10 \ L$ flask. What is the pressure exerted by the gaseous mixture in $bar$? (Assume $H_2$ and $O_2$ as ideal gases)

Which gas has a density of $1.24 \ g/L$ at $0^{\circ} C$ and $1 \ atm$ pressure?

The density of vapours of a particular volatile diatomic species $A_2$ was found to be $10 \ mg/mL$ at $1 \ atm$ and $273 \ K$. Its atomic weight is given by: [Assume ideal gas behaviour].

Containers $A$ and $B$ contain the same gas. The pressure,volume,and temperature of the gas in $A$ are twice the corresponding values of the gas in $B$. The ratio of the number of molecules of gas in $A$ to that in $B$ is ...

At the same temperature,gas $A$ is taken in a $0.5 \, dm^3$ flask and gas $B$ is taken in a $1 \, dm^3$ flask. If the density of $A$ is $3.0 \, g \, dm^{-3}$ and that of $B$ is $1.5 \, g \, dm^{-3}$,and the molar mass of $A$ is $1/2$ of $B$,what is the ratio of the pressures exerted by the gases?

From the following plots,find the correct option.