If the absolute temperature of an ideal gas becomes double and the pressure becomes half,the volume of the gas would be:

Density of carbon monoxide is maximum at

At $273 \ K$ temperature and $76 \ cm \ of \ Hg$ pressure,the volume of $1.786 \ g$ of a gas is $1 \ L$. The gas is likely to be .........

Calculate the volume of $6.022 \times 10^{21}$ molecules of $CO_2$ at $300 \ K$ temperature and $2 \ bar$ pressure. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$ (in $mL$)

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?

What is the molar volume of an ideal gas at $27\,^oC$ and $1\, atm$ pressure in $L$?