Which has a higher average speed, H2 at 150 K or He at 375^∘...

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Key Concepts

Root-Mean-Square Speed

The root-mean-square (rms) speed is a statistical measure derived from the kinetic theory that quantifies the average speed of gas molecules using the equation v_rms = ?(3kT/m), where k is the Boltzmann constant, T is the absolute temperature, and m is the molecular mass. This formula encapsulates the relationship between temperature, mass, and the resulting speed of gas particles.

Molecular Mass Effect

The mass of a molecule influences how fast it moves at a given temperature. According to kinetic theory, for molecules at the same temperature, lighter molecules will have higher average speeds compared to heavier ones. This aspect is essential when comparing gases like hydrogen and helium.

Kinetic Theory of Gases

This concept explains that gas molecules move randomly and that their behavior, including speed, is governed by the kinetic energy related directly to temperature. The theory provides the basis for understanding how temperature affects the motion of individual gas particles.

Temperature Influence on Molecular Speed

Temperature is a measure of the average kinetic energy of the particles in a substance. Higher temperatures imply higher average speeds of molecules as they possess more kinetic energy, making temperature a crucial factor in comparing speeds of different gases.

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