According to Boyle's law, the pressure and volume of an ideal gas at constant temperature are inversely proportional (PV = constant).

The root mean square speed of gas molecules is directly proportional to the square root of the absolute temperature of the gas.

The average speed of gas molecules is directly proportional to the square root of the absolute temperature.

The RMS speed is given by the formula v_rms = sqrt(3RT/M).

Using v_rms = sqrt(3RT/M), we find v_rms = sqrt(3 * 8.314 * 273 / 0.032) which is approximately 400 m/s.

The RMS speed (v_rms) of an ideal gas is given by the formula v_rms = sqrt((3RT)/M), where R is the universal gas constant, T is the absolute temperature, and M is the molar mass.

The RMS speed (v_rms) of an ideal gas is given by the formula v_rms = sqrt((3RT)/M), where R is the universal gas constant, T is the temperature in Kelvin, and M is the molar mass.

The root mean square speed (v_rms) is given by the formula v_rms = (3RT/M)^0.5, where R is the gas constant, T is the temperature, and M is the molar mass.

The root mean square speed of gas molecules is directly proportional to the square root of the absolute temperature, as given by the equation v_rms = sqrt(3kT/m).

The root mean square speed (v_rms) is given by the formula v_rms = sqrt(3kT/m) where k is the Boltzmann constant, T is the temperature, and m is the mass of a gas molecule.

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

The value of R in L·atm/(K·mol) is 0.0821.

The value of the ideal gas constant R in L·atm/(K·mol) is 0.0821.

The value of R in L·kPa/(K·mol) is 8.314.

The ideal gas law combines Boyle's and Charles's laws, relating pressure, volume, and temperature of an ideal gas.

The Ideal Gas Law describes the relationship between pressure, volume, and temperature of a gas.

The Ideal Gas Law (PV = nRT) relates pressure, volume, and temperature of an ideal gas.

The Ideal Gas Law (PV = nRT) relates pressure, volume, and temperature of an ideal gas.

The Ideal Gas Law (PV = nRT) relates pressure, volume, and temperature of an ideal gas.

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

Avogadro's Law states that the volume of a gas is directly proportional to the number of moles at constant temperature and pressure.

The kinetic theory of gases assumes that gas molecules do not experience intermolecular forces, which is why option 3 is NOT part of the assumptions.

The average kinetic energy of gas molecules is dependent only on the temperature of the gas, not on the mass or type of gas.

RMS speed is inversely proportional to the square root of molar mass. Hydrogen (H2) has the lowest molar mass among the options, thus it has the highest RMS speed.

Hydrogen (H2) has the lowest molar mass, thus it will have the highest average speed according to the kinetic theory.

RMS speed is inversely proportional to the square root of molar mass. Hydrogen has the lowest molar mass, hence it will have the highest RMS speed.

The root mean square speed is inversely proportional to the square root of the molar mass. H2 has the lowest molar mass, hence it has the highest root mean square speed.

At a given temperature, lighter gases like hydrogen (H2) have higher average speeds compared to heavier gases like oxygen (O2) or carbon dioxide (CO2).

Hydrogen (H2) has the lowest molar mass among the given gases, thus it will have the highest root mean square speed at the same temperature, as v_rms is inversely proportional to the square root of molar mass.

Newton's Law is not a gas law; it pertains to motion and forces.