In the kinetic theory of gases, the temperature of a gas is a measure of the average kinetic energy of the molecules.

In elastic collisions, both kinetic energy and momentum are conserved, which is a key assumption in the kinetic theory of gases.

In an ideal gas, the internal energy is primarily due to the kinetic energy of the gas molecules, as potential energy is negligible.

In the kinetic theory, the temperature of a gas is a measure of the average kinetic energy of the molecules.

The average speed of gas molecules is given by the formula v_avg = (8kT/πm)^(1/2), where k is the Boltzmann constant, T is the temperature, and m is the mass of a gas molecule.

The average speed of gas molecules is given by the formula v_avg = sqrt(8kT/πm), where k is the Boltzmann constant, T is the temperature, and m is the mass of a molecule.

Absolute zero is defined as the temperature at which molecular motion ceases, corresponding to 0 Kelvin.

Absolute zero refers to the lowest possible temperature, at which gas molecules theoretically stop moving, making both A and B correct.

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

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

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

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

According to Gay-Lussac's law, the pressure of an ideal gas is directly proportional to its temperature when the volume is held constant.

This relationship is known as Boyle's Law, which states that the pressure of an ideal gas is inversely proportional to its volume at constant temperature.

The root mean square speed (v_rms) of gas molecules is given by the formula v_rms = √(3RT/M), where R is the universal gas constant, T is the temperature, and M is the molar mass.

Helium behaves most like an ideal gas under standard conditions due to its low intermolecular forces and small size.

Helium behaves most like an ideal gas because it is a monoatomic gas with weak intermolecular forces.

Hydrogen (H2) has the lowest molar mass among the given gases, thus it has the highest root mean square speed at the same temperature.

Helium behaves most like an ideal gas due to its low intermolecular forces and small size, making it closer to the ideal gas behavior.

At the same temperature, lighter gases have higher average speeds. Hydrogen (H2) has the lowest molar mass and thus the highest average speed.