A gas has double the average velocity of $S{O}_{2}SO\_2$ gas at any temperature. The gas may be:

The density of a gas is 1.964g $d{m}^{-3}dm^\{-3\}$ at 273 K and 76 cm Hg. The gas is :

The root mean square velocity of one mole of a monoatomic gas having molar mass M is $u_{rms}u\_\{rms\}$. The relation between average kinetic energy (E) of the gas and $u_{rms}u\_\{rms\}$ is:

The term that corrects for the attractive forces present in a real gas in the van der Waals equation is:

What is the dominant intermolecular force or bond that must be overcome in converting liquid $C{H}_{3}OHCH\_3OH$ to gas?

Most probable speed, average speed, and rms speed are related as:

The rms speed of hydrogen molecules at room temperature is 2400 ${\text{m s}}^{-1}\backslash text\{m\; s\}^\{-1\}$. At room temperature the rms speed of oxygen molecules would be:

The critical temperature of a gas is that temperature :

Two samples of gases A and B are at the same temperature. The molecules of A are travelling four times faster than the molecules of B. The ratio of their molar masses $M_A\mathrm{/}{M}_{B}M\_A/M\_B$ will be:

The compressibility factor of one mole of a gas is defined as Z = PV/RT. The compressibility factor of an ideal gas is :