The density of methane at $27\,^oC$ and $2.0\,atm$ pressure is ............ $g\,L^{-1}$.

The pressure and temperature of $4 \ dm^3$ of carbon dioxide gas are doubled. Then the volume of carbon dioxide gas would be ............. $dm^3$.

If the temperature of a gas is increased by $1\,^oC$ while keeping the pressure and the amount of gas constant,what is the change in the original volume of the gas?

Find the temperature in degree Celsius if volume and pressure of $2 \ mol$ ideal gas is $20 \ dm^3$ and $4.926 \ atm$ respectively. $(R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1})$

At $240.55 \ K$,for one mole of an ideal gas,a graph of $P$ (on $y$-axis) and $V^{-1}$ (on $x$-axis) gave a straight line passing through the origin. Its slope $(m)$ is $2000 \ J \ mol^{-1}$. What is the kinetic energy (in $J \ mol^{-1}$) of the ideal gas?

Pressure of $1 \ g$ ideal gas $X$ at $300 \ K$ is $2 \ atm$. When $2 \ g$ of another gas $Y$ is introduced in the same vessel at the same temperature,the total pressure becomes $3 \ atm$. The correct relationship between molar masses of $X$ and $Y$ is: