Why is the effect of temperature more important for the liquefaction of gases? Define critical temperature and critical pressure.

$30 \mathrm{mol}$ of chlorine gas occupies a volume of $500 \mathrm{ml}$ at $315 \mathrm{K}$ and $4\times {10}^5 \mathrm{Pa}$ pressure. Calculate the compressibility factor of the gas.

($\mathrm{R}=0.083\mathrm{L} \mathrm{bar} {\mathrm{K}}^{-1}{\mathrm{mol}}^{-1}$).

Which one, in each of the following pairs is more viscous? Explain why?

Coconut oil, castor oil

Which one, in each of the following pairs is more viscous? Explain why?

Glycerine, Kerosene

Which one, in each of the following pairs is more viscous? Explain why?

Soft drink, aerated water

A large flask fitted with a stop-cock is evacuated and weighed; its mass is found to be$134.567 \mathrm{g}$. It is then filled to a pressure of $735 \mathrm{mm}$ at ${31}^{\mathrm{o}}\mathrm{C}$ with a gas of unknown molecular mass and then reweighed; its mass is $137.456 \mathrm{g}$.

The flask is then filled with water and weighed again; its mass is now $1067.9 \mathrm{g}$. Assuming that the gas is ideal, calculate the molar mass of the gas.

Density of a gas is found to be $5.46 \mathrm{g} /{\mathrm{dm}}^3$ at $300 \mathrm{K}$ and $2 \mathrm{bar}$ pressure. What will be its density at STP?