Irene was investigating the behavior of gases at certain conditions. Which would most likely cause an increase in the rate of collisions between gas molecules in a container?

1. The gasses can be made to move faster: This can be done by increasing their temperature. An increase in the temperature of the gases directly relates to a corresponding increase in their kinetic energy. This means that the molecules of the gases can move with a greater velocity, which will increase collision rates.

2. The volume of the container can be reduced: Consider this; If the container is made smaller, the molecules of the gases will have less space to move about. This means that they will be bumping into the walls of the container more frequently. This reduction in volume leads to an increase in the pressure of the gas. This is exactly what happens in a piston-cylinder assembly

andromache andromache · Answer 2 · 2022-03-03T15:05:54+01:00

The increase in the rate of collisions between gas molecules in a container should result in Increase in temperature and Increase in pressure

Reasons for increasing the rate of collisions:

1. In the case when the gasses should be quick faster, due to this, the temperature should be increased. In this, the gases molecules should be moved have high velocity

2, Here the container volume should be decreased. Due to this, the volume should be decreased that results in the increment of the gas pressure.

Therefore, The increase in the rate of collisions between gas molecules in a container should result in Increase in temperature and Increase in pressure

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