Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. a. Do the atoms in the helium sample have the same average kinetic energy as the atoms in the argon sample?

Key Concepts

Kinetic Molecular Theory

The Kinetic Molecular Theory explains the behavior of gases in terms of particles in constant motion. It states that the average kinetic energy of gas particles is directly proportional to the temperature of the gas in Kelvin. Therefore, at the same temperature, different gases will have the same average kinetic energy, regardless of their molecular weight.

Temperature and Kinetic Energy

Temperature is a measure of the average kinetic energy of the particles in a substance. For gases, this means that if two samples are at the same temperature, their particles will have the same average kinetic energy. This principle is crucial for comparing different gases, such as helium and argon, under identical conditions.

Gas Properties and Behavior

Gases exhibit unique properties, including low density and high compressibility, due to the large distances between particles. The behavior of gases can be described by various gas laws, which relate pressure, volume, and temperature. Understanding these properties helps in analyzing how different gases, like helium and argon, behave under the same conditions.