Respuesta :
Answer:
the gas particles strike the walls of the container more often
Explanation:
Following Boyle's law, if the amount of gas and the temperature remain constant, the product of the pressure for the volume remains constant, but when altering any of these conditions this value changes and is expressed through the equation:
[tex]P_{1} V_{1} = P_{2}V_{2}[/tex]
So, when the volume decreases, the distance that the particles have to travel is smaller and therefore more collisions between particles and between the walls occur per unit of time, that is, the system pressure increases.
The volume and pressure of the gas are inversely related to a constant temperature. The pressure increases because gas particles strike the wall of the container more often.
Boyle's law:
The volume of the ideal gas at a constant temperature is inversely proportional to the pressure exerted.
[tex]\bold {P_1 V_1 = P_2V_2}[/tex]
Where,
P- pressure of the gas
V- volume of the gas
When the volume of gas is decreased the gas particles come closer to each other. Hence the chances of the collision increased. This increases the pressure of the gas.
Therefore, the pressure increases because gas particles strike the wall of the container more often.
To know more about Boyle's Law, refer to the link:
https://brainly.com/question/1437490
