50 moles of an ideal gas initially has a volume of 0.8 m³, a pressure of 160 kPa, and a temperature of 280 K. The volume of the gas increases to 1.2 m³, while its pressure decreases to 80 kPa. At any temperature T, the internal energy of the gas is given by U = aT, 500 J K-1. During the expansion, the volume and pressure are related by V where A and B are constants. Assuming that the expansion is reversible, calculate: (a) The values of the constants A and B. (b) The work done by the gas during the expansion. (c) The heat absorbed by the gas during the expansion. where a = = AP + B,

50 moles of an ideal gas initially has a volume of 0.8 m³, a pressure of 160 kPa, and a temperature of 280 K. The volume of the gas increases to 1.2 m³, while its pressure decreases to 80 kPa. At any temperature T, the internal energy of the gas is given by U = aT, 500 J K-1. During the expansion, the volume and pressure are related by V where A and B are constants. Assuming that the expansion is reversible, calculate: (a) The values of the constants A and B. (b) The work done by the gas during the expansion. (c) The heat absorbed by the gas during the expansion. where a = = AP + B,

Physics for Scientists and Engineers: Foundations and Connections

1st Edition

ISBN:9781133939146

Author:Katz, Debora M.

Publisher:Katz, Debora M.

Chapter20: Kinetic Theory Of Gases

Section: Chapter Questions

Problem 42PQ

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