The van der Waals equation is:
(P + a(n/V)^2)(V-nb) = nRT
where P is the pressure, n is the number of moles, V is the volume, T is the temperature, a and b are the van der Waals constants, and R is the gas constant.
Substituting the given values:
P + (4.17 atm.L^2/mol^2)((1.00 mol)/(7.00 L))^2)(7.00 L - (1.00 mol)(0.0371 L/mol)) = (1.00 mol)(0.08206 L.atm/mol.K)(77 + 273.15)K
P + (4.17 atm.L^2/mol^2)(0.02053 mol^2/L^2)(6.963 L) = 24.684 atm
P + 0.0595 atm = 24.684 atm
P = 24.624 atm
Therefore, the pressure exerted by the 1.00 mol of NH2 is 24.624 atm.
1.00 mol of NH2 is stored at 77 oC in a 7.00 L container. Use the van der Waals equation to determine the pressure exerted by the 1.00 mol of NH2. (a= 4.17 atm.L2/mol2 and b= 0.0371L/mol. (R = 0.08206 L.atm/mol.K)
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