[joe_z_wales56]

Hello. I am trying to calculate the pressure in the following Problem.

It can be said  that one molecule of oxygen would fill a one cubic foot container. Under this condition what pressure would you expect to find in the container?

I understand how to calculate pressures with the combined Gas Laws but this question does not include the necessary relationships of pressure.

I have found some formulas on the internet with the help of a friend. I have attempted to make the calculation and wish to find out if it is done correctly or if there is another method of doing the calculation.

Here is the formula I used. Will this work? and is it correct?

P=NRT/V

N= Number of moles 1 or 2 moles.. O2 diatomic right?
I will do both calculations below

R=.082 L ATM  Is this a standard gas pressure?
What is this exactly? It was a given number.

T= 273 K  had to assume 273k. is this correct?

V= 1 cu ft must converted to 28.32 L ?


(1 Molecule/ 6.022 x 10^ -23) x .082x273/28.32L

1.6605 x 10^22 x .082 = 1.36 x 10^21


1.36 x 10^21 x 273 = 3.72 x 10^23


3.72 x 10^23 / 28.32 = 1.3126 x 10^22


Answer is 1.3126 x 10^22  Is this ATM ? Is it correct?


Calculation with 2 moles oxygen

(2 Molecule/ 6.022 x 10^ -23) x .082 x273/28.32L

2/6.022 x 10^ -23) =3.321 x 10^22

3.321 x 10^22 x .082 = 2.723 x 10 ^23

2.723 x 10 ^23 x 273 = 7.434 x 10 ^23

7.434 x 10 ^23 / 28.32L =2.625 x 10^ 22 ATM ??

Is this correct?

Is there another method?


Please email me if you have any info on this problem and how it is done correctly.

joe_z_wales56@yahoo.com

[AWK]

(1 Molecule/ 6.022 x 10^ -23) x .082x273/28.32L
should be (1 Molecule/ 6.022 x 10^23) x .082x273/28.32L