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

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:

In order to increase the volume of a gas by 10%, the pressure of the gas should be

A real gas deviates most from ideal behavior at:

Equal volumes of two gases are kept in separate containers at the same temperature and pressure. Then:

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

Consider a fixed amount of an ideal gas at constant temperature. If the pressure of the gas is tripled, which of the following describes the change in volume?

Boyle’s law may be expressed as:

Equal volumes of two gases which don’t react together are confined in separate vessels. Their pressure is 100 mm and 300 mm of Hg respectively. If the two vessels are joined together, then what will be the pressure of the resulting mixture? (Temperature remains constant)

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: