At $N.T.P.$,the volume of a gas is found to be $273 \ mL$. What will be the volume of this gas at $600 \ mm \ Hg$ and $273 \ ^oC$? ................. $mL$

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

$A$ sealed flask with a capacity of $2 \, dm^{3}$ contains $11 \, g$ of propane gas. The flask is so weak that it will burst if the pressure becomes $2 \, MPa$. The minimum temperature at which the flask will burst is $....... \, ^{\circ}C$. [Nearest integer] (Given: $R = 8.3 \, J \, K^{-1} \, mol^{-1}$. Atomic masses of $C$ and $H$ are $12 \, u$ and $1 \, u$ respectively.) (Assume that propane behaves as an ideal gas.)

"Equal volumes of all gases at the same temperature and pressure contain equal number of particles." This statement is a direct consequence of

Pressure of $1 \, g$ of an ideal gas $A$ at $27^{\circ} C$ is found to be $2 \, bar$. When $2 \, g$ of another ideal gas $B$ is introduced in the same flask at the same temperature,the pressure becomes $3 \, bar$. Find a relationship between their molecular masses.

What is the value of the ratio of density $(d)$ to molar mass $(M)$ for an ideal gas?