at the same temperature the ratio of mean kinetic energies of molecules of hydrogen and nitrogen is
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The kinetic theory states that "The average kinetic gas of a molecules is proportional to the absolute temperature of a gas". Not all molecules will have the same kinetic energy and hence the same speed. An increase in temperature increases the average speed of the molecules and the range of speed.
The average kinetic energy of Nitrogen and Hydrogen molecules will be the same at any particular temperature if we keep in mind that the formula for kinetic energy is 0.5mv^² it stands to reason that the lighter molecules (hydrogen) will have a higher speed than Nitrogen molecules.
It is important to note that although the average kinetic energy of all gases is the same at any particular temperature, the average velocity of the molecules is not. The heavier molecules tends to travel slower relative to the lighter ones.
The average kinetic energy of Nitrogen and Hydrogen molecules will be the same at any particular temperature if we keep in mind that the formula for kinetic energy is 0.5mv^² it stands to reason that the lighter molecules (hydrogen) will have a higher speed than Nitrogen molecules.
It is important to note that although the average kinetic energy of all gases is the same at any particular temperature, the average velocity of the molecules is not. The heavier molecules tends to travel slower relative to the lighter ones.
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