NEET Chemistry States Of Matter Gas Laws MCQs

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)

A real gas deviates most from ideal behavior at:

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:

A vessel contains 1 mole of O2 gas at a temperature T. Another identical vessel contains 1 mole of He gas at a temperature 2T. If the average translational kinetic energy of O2 is $K_1$ and that of He is $K_2$, then:

The compressibility factor (Z) for a gas is given by $Z = PV/nRT$. At high pressures, attractive forces between gas molecules become significant. For a gas exhibiting strong intermolecular attractions, at moderately high pressure, Z will be:

Equal masses of three gases A, B, and C are kept in separate containers of equal volume at the same temperature. The pressure in the containers are in the ratio of 1:16:9. The ratio of their molar masses is:

Which of the following gas laws states that at constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure?

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

Which gas law explains why a hot air balloon rises?

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