Why does gas particle velocity affect rate of effusion?

I understand why smaller particles have more velocity, but I don't understand what velocity has to do with the rate of effusion:

My reasoning is thus:

1. Pressure is the number of impacts of particles in a given period of time.

2. If He and Ar are both in balloons at, say, 1.5 atm, both gasses have the same average Kinetic energy but He is moving faster (because it's smaller). Simple enough.

3. If both gasses are subject to the same pressure, they have the same number of impacts over a given area over a given period of time.

4. This should mean that each gas has an equal number of particles approaching a hole over a given period of time.

5. If a hole is big enough for both particles to fit through, the rate of effusion should be the same, since the same number of particles are approaching the exit hole.

For an analogy to explain my thinking ... if you have two lanes of cars going through a checkpoint, one has 30 cars per minute at 50 miles per hour and one has 30 cars per minute at 30 miles per hour, the resulting number of cars through the checkpoint should still be 30 cars per minute in each lane, regardless of their velocity.

My book (and professor, and Wikipedia...) say that it is the higher velocity of He particles that cause the faster rate of effusion; however, from my reasoning, that doesn't make sense except with small enough holes where the size of the particles would affect, i.e. the holes are very small in size and He could fit through but Ar could not, or there are simply more holes that He could fit through.

But Graham's law is referring to pinholes, which should be large enough for either atom to fit through.

So why does velocity affect the rate of effusion?

Your point 1 is mistaken (or incomplete) $$P=\frac{F}{A}=\frac1A\frac{\Delta p}{\Delta t}=\frac1A\times\frac{2nmv}{\Delta t}$$

This is assuming all particles hit perpendicularly (you can always modify this for all colissions by taking the average component of velocity in the perpendicular direction).

So, pressure is proportional to number of impacts, mass, and velocity. Pressure is not simply "number of impacts", rather it is a combination of number of impacts with other stuff. Since the energies are equal, we can say that $v\propto m^{-\frac12}$, and we get $P\propto n m^{\frac12}$. P is also the same, so $n\propto\frac1{\sqrt m}\propto v$.

Thus, when avg KE and pressure are the same, rate of diffusion is inversely proportional to square root of mass.

• But if I know this is pretty late ... but isn't it still the same number of impacts? i.e. a 5L balloon of helium has the same n as a 5L balloon of Xe. The difference is that the Xe is slower with more mass, but it should still be the same number of impacts shouldn't it? Nov 27 '12 at 17:19

Hey Daniel I'll try to explain in a simple manner.

Since Helium has higher velocity don't you think that it will have a higher collision frequency than Argon which will shorten it's mean free path. As a result He will take more time to travel a given distance along a straight line. So velocity does affect effusion rate.

(I would have written this in comments but my reputation is too low.)

• Your reasoning is wrong. Helium actually has a (~ 3 times) longer mean free path than Argon. Aug 19 '18 at 19:23
• I didn't said that helium's mean free path will be shorter than Argon but it's mean free path will be short than what it would be if we do not consider collision frequency.
– user66707
Aug 20 '18 at 8:29