# Answer to Question #19873 in Inorganic Chemistry for Brittany

Question #19873
8kg of gaseous N2 occupy 100 L flask at 300C. What&#039;s the pressure of the gas, using van der Waals equation? What&#039;s the pressure of the gas, using the ideal gas equation? What are the shortcomings of kinetic molecular theory that lead to the deviation in this calculation?
1
2012-12-03T09:06:47-0500
1) The van der Waal&#039;sequation is
[P + (n^2a)/V^2]*[V - nb] = nRT
P = (nRT/(V - nb)) - ((n^2a)/V^2)

For nitrogen, a = 1.408 and b = 0.03913. Plugging in these values, along with n
and V, we get

P is pressure in atm = ???
V is volume in L = 100L
n is mol = 8000/28 = 285,714
R is the universal gas constant = 0.08206
T is temperature in K = 300K

P = (nRT/(V - nb)) - ((n^2a)/V^2) = (( 285,714 * 0.08206 *300)/(100L - (
285,714 * 0.03913 ))) - ( 285,714 * 285,714 *1.408/100*100) = 67.79
atm = 6867.45 kPa

2) P = nRT/V = 285,714 *8.31*300/100 = 7122.85 kPa

3) This theory rejects the volumes of gases, considered them ideal.

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