Question

consider your observations of heavy and light gas particles when you manipulated the temperature of the container.

use the drop-down menus to complete the sentences correctly.

increasing the temperature of the container results in a(n) drop-down in the pressure. replacing the heavy gas particles with light gas particles at the same temperature results in drop-down

Explanation:

Analyze temperature and pressure relationship

Using the Pressure-Volume-Temperature Relationships and Gas Laws knowledge points

$$ P \propto T \quad (\text{at constant } V, n) $$

An increase in temperature increases the average kinetic energy of the gas particles, leading to more frequent and energetic collisions with the container walls, which results in an increase in pressure.

Analyze particle mass and pressure relationship

Using the Kinetic Molecular Theory knowledge point

$$ KE_{\text{avg}} = \frac{3}{2}k_B T = \frac{1}{2}m v_{\text{rms}}^2 $$

At a constant temperature, the average kinetic energy of heavy and light gas particles is identical. Replacing heavy particles with light particles at the same temperature and number density results in no change in the total pressure, because the lighter particles move faster but carry less momentum per collision, perfectly balancing out to yield the same pressure.

Answer:

Consider your observations of heavy and light gas particles when you manipulated the temperature of the container.

Use the drop-down menus to complete the sentences correctly.

Increasing the temperature of the container results in a(n) <blank>increase</blank> in the pressure. Replacing the heavy gas particles with light gas particles at the same temperature results in <blank>no change in pressure</blank>.