A mixture of 1 mol of He and 0.5 mol of SO2 is held in a container at a constant temperature of 27°C. The partial pressure of He is 2 atm. If the mixture behaves ideally, what is the density of the mixture (g/L) closest to? (Given: R = 0.082 L atm/mol K, Molar mass of He = 4 g/mol, Molar mass of SO2 = 64 g/mol)

The product of pressure and volume $\left( {PV} \right)$ has a unit of:

The density of an unknown gas at STP is 1.43 g/L. What is the molar mass of the gas?

A device used for measurement of gaseous pressure based on Boyle’s law is known as:

Cooking is fast in a pressure cooker, because

At constant pressure, the volume of a gas increases when its temperature:

Four one litre flasks are separately filled with the gases, ${{\rm{O}}_2},{{\rm{F}}_2},{\rm{C}}{{\rm{H}}_4}$ and ${\rm{C}}{{\rm{O}}_2}$ under the same conditions. The ratio of number of molecules in these gases:

If pressure of a gas contained in a closed vessel is increased by $0.4\%$ when heated by $1^\circ C$ its initial temperature must be:

Solid ${\rm{C}}{{\rm{H}}_4}$ is:

An open vessel containing air is heated from 300 K to 400 K. The fraction of air originally present which goes out of it is:

Two closed vessels of equal volume containing air at pressure ${p_1}$ and temperature ${T_1}$ are connected to each other through a narrow tube. If the temperature in one of the vessels is now maintained at ${T_1}$ and that in the other at ${T_2}$, what will be the pressure in the vessels?