GOT A QUESTION ON AP CHEMISTRY?

J

James B

New member
Consider 20.0 moles of CO2 in a 1.0 liter container at 300.0 K. What is the pressure predicted by the van der Waals equation? The ideal gas law constant is 0.08206 [L•atm]/[mol•K]. For CO2, the pressure correction constant is 3.658 L2•atm/mol2, and the volume correction constant is 0.04286 L/mol.

a. 3500 atm
b. -1198 atm
c. 1728 atm
d. 492 atm

I had trouble with this one, but the answer I got was kinda close to B
 
Yeah, for me too, the van der Waals equation is quite confusing.

[P + (n^2 x a/V^2)](V - nb) = nRT

so P = nRT - ((n^2a/V^2)(V-nb))

= 20 mol x .0821 x 300 K - ((20^2 x .04286/1^2)(1 - (20 x 3.658)))

Okay, so my answer is 1729 atm.

Your answer is C.
 
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