Question

Using the Kinetic Molecular Theory, explain Charles's Law of gases. Refer to specific points of the

Answer 1

Answer:

Kinetic theory explains why the volume of a container must expand when the temperature of the gas inside increases in order for the pressure to remain constant.

Step-by-step explanation:

Charles' law: for a fixed mass of gas at constant pressure the volume is directly proportional to the temperature.

Analysis of a gas when its temperature increases according to kinetic theory:

The temperature has increased therefore the molecules have more kinetic energy, so they move with a greater velocity.¹

If the container's dimensions do not change the molecules will travel across the container between the walls in less time (because they are moving faster and covering the same distance between the container walls). This will increase the rate of collisions, which would increase the pressure.²

But if the dimensions of the container increased then the molecules would cover a larger distance faster thereby maintaining a constant rate of collisions. This would maintain a constant pressure.

Answer 2

Charles law: a law stating that the volume of an ideal gas at constant pressure is directly proportional to the absolute temperature.

According to kinetic energy, increase in temperature will increase kinetic energy

Based on the dimensions of the cup/container, the increase in kinetic energy will cause more collisions, causing increase in pressure as well. This increase in pressure will cause the container to expand in compensation.

This proves charles law because the temperature increase caused the pressure to change as well.