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(a)
Interpretation: The final temperature for the adiabatic expansion of 0.5 mol of an ideal gas with CV,m =3R/2. The initial pressure and temperature is 6.25 bar and 300 K respectively. Also, the final pressure is 1.25 bar.
Concept Introduction: For an adiabatic process, the heat involved is equal to zero. The molar heat capacity at constant volume is represented as CV,m and molar heat capacity at constant pressure is CP,m .
(b)
Interpretation: The final temperature needs to be determined, if the same gas undergoes adiabatic expansion with external and final pressure equals to 1.25 bar.
Concept Introduction: The change in internal energy is calculated as follows:
ΔU=nCV.m(Tf−Ti)
Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.
The work done is represented as follows:
w=−PexternalΔV
Here, P is external pressure and ΔV is change in volume.
The enthalpy of a reaction is represented as follows:
ΔH=ΔU+nRΔT
Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.
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Chapter 2 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
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- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
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