The kinetic molecular theory makes four main assumptions about an ideal gas: a g

Question

The kinetic molecular theory makes four main assumptions about an ideal gas: a gas is a collections of atoms or molecules in constant straight line mission. Gas particulars collide with one atom pod. There is a lot of surface between the particles compared with the since of particulars themselves the speed of gas particulars increases in temperature increases imagine that you have ideal gas in a 4.10 L container, and that 1450 molecules of the gases collide with a square inch area of the container if any gases instant if the volume is increased to 25.0 L at constant temperature how many will occur per Enter the number of colleens per square inch.

Explanation / Answer

The ideal gas behavior equation, PV = nRT.

Molecules of gas colliding with the walls of the container cause pressure. All other things being equal, as volume increases, pressure decreases. So we have the equation at 2 different states.

P1V1 = n1RT1 and P2V2 = n2RT2

Since the number of moles is not changing and temperature is constant, n1 = n2 and T1 = T2 we can say that:

P1V1 = n1RT1 and P2V2 = n1RT1 and therefore: P1V1 = P2V2

Plugging the known values:

1450 * 4.10 L = 20.5 L x

x = 1450 * 4.10 / 20.5

x = 290

Hope this helps

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