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