A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. a. Which of the two gases exerts the greater partial pressure?

Key Concepts

Partial Pressure

Partial pressure is the pressure that a single gas in a mixture would exert if it occupied the entire volume alone. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. Understanding this concept is crucial for determining how each gas contributes to the overall pressure in a container.

Ideal Gas Law

The Ideal Gas Law, represented as PV = nRT, relates the pressure (P), volume (V), number of moles (n), the ideal gas constant (R), and temperature (T) of a gas. This law helps predict the behavior of gases under various conditions. In this scenario, it can be used to compare the behavior of nitrogen and xenon, particularly their pressures at the same temperature and volume.

Molar Mass and Density

Molar mass is the mass of one mole of a substance, and it influences the density of gases. In this case, nitrogen (N2) has a lower molar mass compared to xenon (Xe), which means that at the same temperature and volume, nitrogen will have a higher number of moles per unit volume, leading to a greater partial pressure. Understanding the relationship between molar mass, density, and gas behavior is essential for this question.