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An ideal monoatomic gas at 298 K and 1 bar is expanded in a reversible adiabatic process to a final pressure of ½ bar. Calculate the (a) change in heat (q) per mole (b) final temperature (c) initial and final volumes (in L) for 1 mole of gas Useful relation: 1 atm = 1.01325 bar.     Please type answer note write by hend.

An ideal monoatomic gas at 298 K and 1 bar is expanded in a reversible adiabatic process to a final pressure of ½ bar. Calculate the (a) change in heat (q) per mole (b) final temperature (c) initial and final volumes (in L) for 1 mole of gas Useful relation: 1 atm = 1.01325 bar.     Please type answer note write by hend.

Introduction to Chemical Engineering Thermodynamics
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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An ideal monoatomic gas at 298 K and 1 bar is expanded in a reversible adiabatic process to a final pressure of ½ bar. Calculate the (a) change in heat (q) per mole (b) final temperature (c) initial and final volumes (in L) for 1 mole of gas Useful relation: 1 atm = 1.01325 bar.  

 

Please type answer note write by hend. 

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