Test: Behaviour of Gases - SSC MTS / SSC GD MCQ

Gases have particles with large spaces between them, allowing for compression when pressure is applied.

The kinetic molecular theory describes gases as being composed of tiny molecules that are in constant motion.

Boyle's law states that at constant temperature, the pressure and volume of a gas are inversely proportional.

Gay-Lussac's law states that the pressure of a gas is directly proportional to its absolute temperature at constant volume.

Charles's law states that at constant pressure, the volume of a gas is directly proportional to its temperature.

Avogadro's law states that equal volumes of gases, at the same temperature and pressure, contain the same number of molecules.

The ideal gas law combines Boyle's law, Charles's law, and Gay-Lussac's law into a single equation.

The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature.

Carbon dioxide deviates the most from ideal gas behavior due to its larger molecular size and intermolecular forces.

Graham's law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Boyle's law can be used to determine the molar mass of an unknown gas by comparing the volume changes at constant temperature.

The average kinetic energy of gas molecules is directly proportional to the temperature. As the temperature increases, so does the kinetic energy.

The van der Waals equation of state corrects for the volume occupied by gas molecules, which is neglected in the ideal gas law.

Real gases deviate from ideal behavior when the intermolecular forces and molecular volumes become significant at high temperatures and low pressures.

Boyle's law describes the inverse relationship between the pressure and volume of a gas at constant temperature.

According to Dalton's law of partial pressures, the partial pressure of a gas is directly proportional to its mole fraction in the mixture.

Dalton's law states that the total pressure exerted by a mixture of gases is equal to the sum of the pressures of the individual gases.

Boyle's law states that the volume of a gas is inversely proportional to its pressure at constant temperature.

The critical temperature of a gas is the temperature above which the gas cannot be liquefied, regardless of the pressure applied.

The average kinetic energy of gas molecules is directly proportional to their temperature and inversely proportional to their molar mass. Helium has the lowest molar mass among the options, so it has the highest average kinetic energy at the same temperature.