An "empty" container is not really empty if it contains air. How may moles of nitrogen are in an "empty" two-liter cola bottle at atmospheric pressure and room temperature (25∘C)? Assume ideal behavior.

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Answer 1 · 2018-03-23T01:41:20

I'm going to use 78% as Nitrogen's component in "Air"
See below

Since nitrogen accounts for 78% of the air you breath in, it's partial pressure in a 1 atomosphere room is 0.78atm.

So to get the moles of nitrogen in that cola bottle, we'll use the ideal gas law
#PV = nRT# and solve for n

#n=(PV)/(RT)#
#n=((0.78atm)(2L))/((0.0821)(298K))#
#n = 0.064 mol N_2#