Derive the work of reversible isothermal compression of a van der Waals gas. How does it compare to the work needed to compress the ideal gas in the limit of (a) low pressure, and (b) high pressure? Calculate the work done by a sample of Ar of mass 7.60 g that initially occupies 1.750 dm3 at 350 K, and expands reversibly and isothermally by 0.350 dm3 . Assume that argon obeys the van der Waals equation of state with a = 1.373 Pa m6 mol−2 and b = 3.200 × 10−5 m3 mol−1 . Compare to the corresponding value obtained in the previous problem for an ideal gas.
Derive the work of reversible isothermal compression of a van der Waals gas. How does it compare to the work needed to compress the ideal gas in the limit of (a) low pressure, and (b) high pressure? Calculate the work done by a sample of Ar of mass 7.60 g that initially occupies 1.750 dm3 at 350 K, and expands reversibly and isothermally by 0.350 dm3 . Assume that argon obeys the van der Waals equation of state with a = 1.373 Pa m6 mol−2 and b = 3.200 × 10−5 m3 mol−1 . Compare to the corresponding value obtained in the previous problem for an ideal gas.
Physical Chemistry
2nd Edition
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Ball, David W. (david Warren), BAER, Tomas
Chapter2: The First Law Of Thermodynamics
Section: Chapter Questions
Problem 2.91E: The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants...
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Derive the work of reversible isothermal compression of a van der Waals gas. How does it compare to the work needed to compress the ideal gas in the limit of (a) low pressure, and (b) high pressure? Calculate the work done by a sample of Ar of mass 7.60 g that initially occupies 1.750 dm3 at 350 K, and expands reversibly and isothermally by 0.350 dm3 . Assume that argon obeys the van der Waals equation of state with a = 1.373 Pa m6 mol−2 and b = 3.200 × 10−5 m3 mol−1 . Compare to the corresponding value obtained in the previous problem for an ideal gas.
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