Imagine that you have an ideal gas in a 4.30 L container, and that 1250 molecules of this gas collide with a square-inch area of the container at any given instant. If the volume is increased to 21.5 L at constant temperature, how many collisions will occur per square inch of this larger container

250 collisions per square inch

Explanation:

According to Boyle's law, at constant temperatures, the pressure exerted by gas molecules is inversely proportional to the volume of the gas. Hence;

    P1V1 = P2V2 where P1 = initial pressure, V1 = initial volume, P2 = final pressure, and V2 = final volume

In this case, the collision that occurred is taken as the pressure.

P1 = 1250, V1 = 4.30 , V2 = 21.5 P2 = ?

P2 = P1V1/V2

        = 1250 x 4.30/21.5

                 = 250

Hence, at a constant temperature, 250 collisions per square inch of the larger container will occur.