Increasing the number of gas molecules at constant temperature and volume leads to more collisions with the walls of the container, resulting in increased pressure.

Increasing the number of gas molecules at constant volume and temperature increases the pressure, according to the ideal gas law.

The RMS speed is independent of the number of gas molecules; it depends only on temperature and molar mass.

According to the ideal gas law, increasing the number of moles (n) of a gas while keeping volume (V) and temperature (T) constant will increase the pressure (P).

According to Avogadro's Law, increasing the number of moles of gas increases the pressure if temperature and volume are constant.

According to Avogadro's Law, increasing the number of moles of gas increases the pressure if the volume is constant.

According to the ideal gas law, increasing the number of moles of gas at constant volume and temperature will increase the pressure.

According to Avogadro's Law, increasing the number of moles of gas at constant volume and temperature will increase the pressure.

According to Avogadro's Law, increasing the number of moles of gas increases the pressure if volume and temperature are constant.

At constant temperature, increasing pressure does not affect the RMS speed, as it is dependent on temperature and molar mass.

At constant volume, increasing pressure increases the temperature of the gas, which in turn increases the RMS speed.

Increasing the temperature of a gas at constant volume increases the pressure, as per Gay-Lussac's law.

Increasing the temperature increases the average kinetic energy of gas molecules, which in turn increases their average speed.

Increasing the temperature increases the average kinetic energy of the molecules, resulting in a wider distribution of molecular speeds.

Increasing the temperature increases the RMS speed, as v_rms is proportional to the square root of temperature.

Increasing the temperature of a gas increases the average kinetic energy of the molecules, which in turn increases their speed.

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

The kinetic theory assumes that gas molecules move in straight lines until they collide with each other or the walls of the container.

Boyle's Law states that the pressure of a gas is inversely proportional to its volume at constant temperature, which can be expressed as PV = constant.

According to Boyle's Law, pressure and volume of a gas are inversely proportional at constant temperature.

Boyle's Law states that the pressure of a gas is inversely proportional to its volume at constant temperature, which can be expressed as PV = constant.

The kinetic energy of gas molecules is directly proportional to the square of the RMS speed, as KE = (1/2)mv_rms^2.

RMS speed is inversely proportional to the square root of molecular weight.

The average kinetic energy of gas molecules is directly proportional to the absolute temperature (KE ∝ T).

For an ideal gas, the RMS speed is always greater than the average speed due to the squaring of velocities in the RMS calculation.

For an ideal gas, the RMS speed is always greater than the average speed due to the nature of the distribution of molecular speeds.

The mean free path (λ) is inversely proportional to the diameter (d) of the gas molecules, meaning λ ∝ 1/d.

The mean free path is inversely proportional to the density of gas molecules. As density increases, the mean free path decreases due to more frequent collisions.

The mean free path is inversely proportional to the diameter of gas molecules; as the diameter increases, the mean free path decreases.

According to Boyle's Law, which is derived from the kinetic theory, pressure is inversely proportional to volume at constant temperature.