Two flasks A and B have equal volumes. Flask A contains H2 at 2 atm and 300K. Flask B contains an equal mass of CH4 at 600 K. Assuming ideal behavior, the ratio of the number of molecules in flask A to flask B is:

Dipole-dipole attractive forces are strongest between the molecules of:

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 density of a gas $A$ is twice that of a gas $B$ at the same temperature. The molecular weight of gas $B$ is thrice that of $A$. The ratio of the pressures acting on $A$ and $B$ will be

Vapour pressure increases with increase in

A certain mass of gas occupies a volume of 300 cc at 27\,^\circ C and 620 mm pressure. The volume of this gas at47\,^\circ C and 640 mm pressure will be

At a constant temperature, if the volume of a fixed mass of gas is halved, what happens to its pressure according to Boyle's Law?

A certain mass of gas occupies a volume of 300 cc at 27\,^\circ C and 620 mm pressure. The volume of this gas at47\,^\circ C and 640 mm pressure will be

A gas behaves most like an ideal gas under conditions of:

Equal volumes of all gases, at the same temperature and pressure, contain the same number of molecules. This is a statement of:

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: