Using the ideal gas equation, find the pressure of 22.4L of helium at 273K when n=1.00 mol. Adjust this calculation using the real gas equation to find the actual pressure. What are the ideal and real pressures?
Explanation
Answer: B. Solution is as follows:
PV=nRT
P=pressure (atm)
V=volume (22.4L)
n=amount (1 mol)
R = constant (0.08206 L*atm/mol*K)
T = temperature (273K)
Ideal gas equaion gives P=1.0atm
a=0.03412 (L2*atm/mol2)
b= 0.02370 (L/mol)
(P+(an2/V2))(V-nb)=nRT
By substituting in the known values of V, n, R, and T, you solve for P=1.001atm, or 1.00atm with significant figures.
