One kmol of an ideal gas at 500 K is taken through an adiabatic expansion from 5 to 3 bar. Theprocess is reversible. ̄CV= 21.686J mol−1K−1and ̄Cp= 30J mol−1K−1. Calculate Q, W, ∆Uand∆Hfor the process. Draw the path/process on thePV diagram. What is the final temperature of the gas?
One kmol of an ideal gas at 500 K is taken through an adiabatic expansion from 5 to 3 bar. Theprocess is reversible. ̄CV= 21.686J mol−1K−1and ̄Cp= 30J mol−1K−1. Calculate Q, W, ∆Uand∆Hfor the process. Draw the path/process on thePV diagram. What is the final temperature of the gas?
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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One kmol of an ideal gas at 500 K is taken through an adiabatic expansion from 5 to 3 bar. Theprocess is reversible. ̄CV= 21.686J mol−1K−1and ̄Cp= 30J mol−1K−1. Calculate Q, W, ∆Uand∆Hfor the process. Draw the path/process on thePV diagram. What is the final temperature of the gas?
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Introduction
VIEWIsentropic process on a P-V diagaram
VIEWFinal Temperature of the gas
VIEWCalculation of Work , W
VIEWCalculation of change in internal energy
VIEWCalculation of change in enthalpy
VIEWAnswer / Summary
VIEWBasic Thermodynamic Processes in a P-V quadrants (for both expansion and compression)
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