The average speed of gas molecules is approximately 0.8 times the RMS speed, so average speed = 0.8 * 400 m/s = 320 m/s.

The speed at 1/2 of the RMS speed is simply 500 m/s / 2 = 250 m/s.

The average speed of gas molecules is related to the RMS speed by the relation v_avg = (v_rms * sqrt(8/3)). Therefore, the average speed is approximately 400 m/s.

The RMS speed is an average measure; individual molecular speeds will vary around this value.

Using v_rms = sqrt(3RT/M), we rearrange to find T = (v_rms^2 * M) / (3R). Plugging in values gives T approximately 300 K.

According to Gay-Lussac's Law, if the temperature of a gas is increased while keeping the volume constant, the pressure will also increase proportionally, thus it doubles.

The RMS speed is proportional to the square root of the temperature. If the temperature is doubled, the RMS speed increases by a factor of sqrt(2).

The RMS speed is proportional to the square root of the temperature. If the temperature is doubled, the RMS speed increases by a factor of sqrt(2).

RMS speed is directly proportional to the square root of temperature. Halving the temperature results in a decrease in RMS speed by sqrt(2).

RMS speed increases by sqrt(4) = 2, since v_rms is proportional to sqrt(T).

RMS speed is proportional to the square root of temperature. Increasing from 300 K to 600 K increases the speed by sqrt(2).

According to Gay-Lussac's Law, if the temperature of a gas is increased while keeping the volume constant, the pressure increases.

According to Gay-Lussac's law, at constant volume, the pressure of an ideal gas is directly proportional to its absolute temperature. Therefore, if the temperature is doubled, the pressure also doubles.

The average kinetic energy of gas molecules is directly proportional to the absolute temperature. Therefore, if the temperature is doubled, the average kinetic energy also doubles.

According to Gay-Lussac's law, if the volume is constant, the pressure of an ideal gas is directly proportional to its absolute temperature. Therefore, doubling the temperature doubles the pressure.

According to Boyle's Law, if the volume is doubled, the pressure is halved.

According to Boyle's Law, if the volume of a gas is halved at constant temperature, the pressure will double.

According to Gay-Lussac's Law, if the volume is constant, increasing the temperature increases the pressure.

According to Gay-Lussac's Law, if the temperature of a gas increases in a closed container, the pressure increases.

This principle is known as Dalton's Law of Partial Pressures.

The partial pressure of a gas in a mixture is the pressure that gas would exert if it occupied the entire volume alone.

Dalton's Law of Partial Pressures states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each gas.

According to Boyle's Law, if the volume is halved while keeping the temperature constant, the pressure doubles.

The distribution of molecular speeds in a gas is described by the Maxwell-Boltzmann distribution.

The mean free path is affected by temperature, pressure, and molecular diameter, but not by the color of the gas.

The RMS speed of a mixture of gases is the weighted average of the RMS speeds of the individual components, taking into account their molar masses.

The RMS speed of a mixture of gases is calculated using the average molar mass of the mixture in the formula v_rms = sqrt((3RT)/M_avg).

According to Gay-Lussac's Law, if the volume decreases at constant pressure, the temperature must increase.

The average kinetic energy of a molecule in an ideal gas is directly proportional to the absolute temperature of the gas, given by the formula KE_avg = (3/2)kT.

The average kinetic energy of a molecule in an ideal gas is directly proportional to the absolute temperature (T) of the gas.