Answer: The gas pressure increases.
Step-by-step explanation:
When collisions increase between gas particles, the gas pressure increases. This is because the gas particles are hitting the walls of the container more often, which exerts more force on the walls. The pressure of a gas is defined as the force per unit area exerted by the gas particles on the walls of the container.
Here is a simple analogy: imagine a balloon filled with air. If you squeeze the balloon, you are increasing the number of collisions between the gas particles and the walls of the balloon. This increases the force on the walls of the balloon, which increases the pressure of the air inside the balloon.
Another example is a bicycle pump. When you pump air into a bicycle tire, you are increasing the number of gas particles in the tire. This increases the number of collisions between the gas particles and the walls of the tire, which increases the pressure of the air inside the tire.
The relationship between gas pressure and collisions is described by Boyle's law, which states that the pressure of a gas is inversely proportional to the volume of the gas, at constant temperature and amount of gas. This means that if you decrease the volume of a gas, you increase the number of collisions between the gas particles, which increases the pressure of the gas.
I hope this helps!