# Thermodynamics nitrogen molecules help

1. Apr 29, 2008

### houseguest

1. The problem statement, all variables and given/known data

At 100 Celcius the rms speed of nitrogen molecules is 576 m/s. Nitrogen at 100 Celcius and a pressure of 2.0 atm is held in a container with a 10cm x 10cm square wall.

2. Relevant equations

rate of collisions: N_coll/ $$\Delta$$t = (N*A*v_x)/(2V) (this is from my textbook)
ideal gas law: N = PV/k_bT (k_b == boltzmann constant)

3. The attempt at a solution

I took that equation and applied the ideal gas law to replace N,
number of collisions = (P*A*v_x)/(2*k_b*T)
= (2 * 101325 Pa)(.1*.1 m^2)(576m/s) / ( 2 * 1.38 * 10^-23 * (100+273.15) )

after plugging in the numbers I got 1.13 * 10^26, but that's wrong. I'm not sure why.

Thanks!!

Last edited: Apr 29, 2008
2. Apr 30, 2008

### kkaplanoz

The equation that you use for the rate of collisions is asking for v_x, not v. v_rms is v. The relationship between the two is 3*v_x^2 = v_rms^2. This is because v_x^2+v_y^2+v_z^2=3*v_x^2=v^2.

3. Apr 30, 2008

### houseguest

Ooooh yeeeeeaaah.

THANKS!