One mole of a perfect monatomic gas, initially at 300 K and a pressure 15.0 atm, expands to a final pressure of 1.00 atm. Consider the expansion via each of the following paths: (a) isothermal and reversible, (b) isothermal and irreversible, (c) adiabatic and reversible, (d) adiabatic and irreversible. In these irreversible processes, the expansion occurs against an external pressure of 1.00 atm. For each case, calculate the values of q, w, ΔU and ΔH.

One mole of a perfect monatomic gas, initially at 300 K and a pressure 15.0 atm, expands to a final pressure of 1.00 atm. Consider the expansion via each of the following paths: (a) isothermal and reversible, (b) isothermal and irreversible, (c) adiabatic and reversible, (d) adiabatic and irreversible. In these irreversible processes, the expansion occurs against an external pressure of 1.00 atm. For each case, calculate the values of q, w, ΔU and ΔH.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 19P

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