Question

Imagine that you have an ideal gas in a 4.00 L container, and that 2950 molecules...

Imagine that you have an ideal gas in a 4.00 L container, and that 2950 molecules of this gas collide with a square-inch area of the container at any given instant.

If the volume is increased to 28.0 L at constant temperature, how many collisions will occur per square inch of this larger container?

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Answer #1

P1V1 = n1RT1 and   P2V2 = n2RT2

Temperature is same T1= T2

no of moles are same n1 = n2

P1 = 2950atm              P2 =

V1 = 4L                        V2 = 28L

P1V1 = P2V2

P2 = P1V1/V2

        = 2950*4/28   = 421.42 will collide in squar inch area of new container.

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