How many molecules of monotonic and diatomic gas are in a container?

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In a container of 3300 cm^3 filled with half diatomic oxygen and half monotonic helium, the pressure is 17 atm and the temperature is 25 degrees C. Using the equation N = 1.5 PV/K, calculations reveal a total of approximately 6.91 x 10^23 molecules. The number of diatomic oxygen molecules is about 4.15 x 10^23, which is roughly 3/5 of the total. An error in the initial pressure measurement was identified, indicating it should be 18 atm instead of 17 atm. This adjustment may affect the final calculations for the number of molecules present.
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1. You have a container of 3300 cm^3. Half of it is diatomic oxygen and half is monotonic helium. Pressure is 17 atm and temperature is 25 degrees C. How many molecules of each substance are in it?



2. PV = 2/3 N(1/2 mv^2) -> PV = 2/3 N (K) -> N = 1.5 PV/K

K_monotonic = 3/2kT = 3/2 (1.38*10^-23)(298k)

k_diatonic = 5/2kT = 5/2 (1.38*10^-23)(298k)




3. N=1.5(17atm*(1Pa/9.869*10^-6 atm)*1650 cm^3 * 1m^3/10^6 cm^3))/((3/2) 1.38*10^-23)(298k))

3/2 factors cancel out. after all the math I get 6.91*10^23.

diatomic is basically 3/5 of that number, 4.15*10^23
 
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masteringphysics is truly an awful piece of software. It turns out that the reason I was getting the wrong answer was because the gauge pressure undermeasures the pressure. It's supposed to be 18, not 17.
 
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