Take nitrogen to be a van der Waals gas with a = 1.352 dm6 atm mol2 and b = 0.0387 dm3
Chapter 2, Problem 2.19(choose chapter or problem)
Take nitrogen to be a van der Waals gas with a = 1.352 dm6 atm mol2 and b = 0.0387 dm3 mol1, and calculate Hm when the pressure on the gas is decreased from 500 atm to 1.00 atm at 300 K. For a van der Waals gas, = {(2a/RT) b}/Cp,m. Assume Cp,m = 72R.
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