Two moles of an ideal monatomic gas initially at 350 K is expanded from an initial pressure of 10 atm to a final pressure of 1 atm. Calculate ΔU, q, w, ΔH, and the final temperature T2 for this expansion carried out according to each of the following paths. The molar heat capacity at constant volume for a monatomic gas is C¯V,m = (3/2)R. (a) An isothermal, reversible expansion. (b) An expansion against a constant external pressure of 1 atm in a thermally isolated (adiabatic) system. (c) An expansion against zero external pressure (i.e. against a vacuum) in an adiabatic system.
Two moles of an ideal monatomic gas initially at 350 K is expanded from an initial pressure of 10 atm to a final pressure of 1 atm. Calculate ΔU, q, w, ΔH, and the final temperature T2 for this expansion carried out according to each of the following paths. The molar heat capacity at constant volume for a monatomic gas is C¯V,m = (3/2)R. (a) An isothermal, reversible expansion. (b) An expansion against a constant external pressure of 1 atm in a thermally isolated (adiabatic) system. (c) An expansion against zero external pressure (i.e. against a vacuum) in an adiabatic system.
Physics for Scientists and Engineers: Foundations and Connections
1st Edition
ISBN:9781133939146
Author:Katz, Debora M.
Publisher:Katz, Debora M.
Chapter21: Heat And The First Law Of Thermodynamics
Section: Chapter Questions
Problem 76PQ
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10. Two moles of an ideal monatomic gas initially at 350 K is expanded from an initial
pressure of 10 atm to a final pressure of 1 atm. Calculate ΔU, q, w, ΔH, and the final
temperature T2 for this expansion carried out according to each of the following paths.
The molar heat capacity at constant volume for a monatomic gas is C¯V,m = (3/2)R.
(a) An isothermal, reversible expansion.
(b) An expansion against a constant external pressure of 1 atm in a thermally isolated
(adiabatic) system.
(c) An expansion against zero external pressure (i.e. against a vacuum) in an adiabatic
system.
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