Because (H/P) T = -C P J T , the change in enthalpy of a gas
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Because (∂H/∂P)T = -CP μ J −T , the change in enthalpy of a gas expanded at constant temperature can be calculated. To do so, the functional dependence of μ J −T on P must be known. Treating Ar as a van der Waals gas, calculate ΔH when 1 mol of Ar is expanded from 325 bar to 1.75 bar at 375 K. Assume that μ J −T is independent of pressure and is given by μ J −T = [(2a/RT) − b]/CP,m, and CP,m = 5/2R for Ar. What value would ΔH have if the gas exhibited ideal gas behavior?
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