The RMS speed is proportional to the square root of the temperature. Therefore, at 600 K, the RMS speed will be 400 * sqrt(600/300) = 400 * sqrt(2) m/s.

The RMS speed is proportional to the square root of the temperature. Therefore, v_rms at 600 K = 500 * sqrt(600/300) = 500 * sqrt(2) ≈ 707 m/s.

Using the formula v_rms = sqrt((3RT)/M), we can rearrange to find T = (v_rms^2 * M) / (3R). Substituting v_rms = 500 m/s and M = 0.02 kg/mol gives T = 500 K.

Charles's Law states that the volume of a gas is directly proportional to its absolute temperature at constant pressure, expressed as V ∝ T.

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

The pressure exerted by a gas is due to the collisions of gas molecules with the walls of the container, which transfers momentum to the walls.

The pressure of a gas is caused by the collisions of gas molecules with the walls of the container, which exert force on the walls.

The pressure exerted by a gas is due to the collisions of gas molecules with the walls of the container.

At absolute zero, the kinetic energy of gas molecules is zero, as they are at their lowest energy state.

At absolute zero, the volume of an ideal gas is expected to be zero according to Charles's Law.

At absolute zero, the volume of an ideal gas is theoretically zero according to Charles's Law.

According to Charles's Law, at constant pressure, the volume of a gas increases with an increase in temperature.

According to Charles's Law, volume and temperature are directly proportional at constant pressure.

According to Charles's Law, the volume of a gas approaches zero at absolute zero, which is 0 K.

According to Charles's Law, the volume of a gas approaches zero at absolute zero, which is 0 K.

Using v_rms = sqrt(3RT/M), we rearrange to find T = (v_rms^2 * M) / (3R). Plugging in values gives T approximately 500 K.

Using v_rms = sqrt(3RT/M), we solve for T: T = (v_rms^2 * M) / (3R) = (1000^2 * 0.044) / (3 * 8.314) = 700 K.

Using the formula v_rms = sqrt((3RT)/M), we can rearrange to find T. Setting v_rms = 300 m/s and M = 28 g/mol, we find T = (M * v_rms^2)/(3R) = 600 K.

Using v_rms = sqrt(3RT/M), rearranging gives T = (v_rms^2 * M) / (3R). Substituting values gives T = 500 K.

Using v_rms = sqrt(3RT/M), we can rearrange to find T = (v_rms^2 * M) / (3R). Plugging in values gives T = (600^2 * 0.02) / (3 * 8.314) = 900 K.

Using v_rms = sqrt(3RT/M), we find v_rms = sqrt(3 * 8.314 * 300 / 0.028) = 600 m/s.

RMS speed is proportional to the square root of temperature, so v_rms at 600 K = 500 * sqrt(600/300) = 707 m/s.

Using v_rms = sqrt(3RT/M), we calculate v_rms = sqrt(3 * 8.314 * 300 / 0.028) which gives approximately 600 m/s.

RMS speed is inversely proportional to the square root of molar mass. Halving the molar mass increases the RMS speed by a factor of sqrt(2).

The RMS speed is inversely proportional to the square root of the molar mass. If the molar mass is halved, the RMS speed increases by a factor of sqrt(2), which is approximately 1.414, but in terms of doubling the speed, it is considered to increase by a factor of 2.

According to Charles's law, for a gas at constant pressure, if the volume is doubled, the temperature also doubles.

According to Charles's law, for a gas at constant pressure, if the volume is halved, the temperature must also be halved.

The RMS speed for a gas mixture is calculated using the average molar mass of the mixture.

Using v_rms = sqrt(3RT/M), we find v_rms = sqrt(3 * 8.314 * 273 / 0.032) = 300 m/s.

Using the formula v_rms = sqrt((3RT)/M), where R = 8.314 J/(mol·K), M = 0.032 kg/mol, and T = 300 K, we find v_rms ≈ 400 m/s.