Applied Thermodynamics MAE 321
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This 6 page Class Notes was uploaded by Ardith Gutmann on Saturday September 12, 2015. The Class Notes belongs to MAE 321 at West Virginia University taught by Staff in Fall. Since its upload, it has received 21 views. For similar materials see /class/202652/mae-321-west-virginia-university in Mechanical Engineering at West Virginia University.
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Date Created: 09/12/15
MAE 321 Applied Thermodynamics Extra Credit April 11 2009 The extra credit is due Wednesday April 15 2009 Each problem is worth the points indicated I encourage you to work in small groups to learn this material However copying of the solution from another is not acceptable 1 Explain the importance of Chapter 12 10 points 2 Starting with the Maxwell relationships estimate the change in entropy of 1 kg of R134a at a temperature of 120 OC when the pressure changes from 10 to 12 MPa Compare this value with the one obtained by using the entropy values in the R134a table located in the appendix 25 points 3 Explain the importance of Chapter 13 10 points 4 Air consists of approximately 21 oxygen 78 nitrogen ltl argon and N400 ppm carbon dioxide on a molar basis Determine a the mole fraction b mass fraction and 0 molar mass of air 25 points 5 Design a simple experiment to prove a Dalton s law of additive pressures and b Amagat s law of additive volumes 15 points 6 Under what conditi0ns is are the mole fraction pressure fraction and volume fraction of an ideal gas the same 15 points Suggested Book Problems to Review These problems will not be collected but are suggested as a review Chapter 12 2 6 9 16 20 21 24 35 56 63 70 73 Chapter 13 4 6 8 12 17 18 19 24 49 50 51 MAE 321 Applied Thermodynamics Extra Credit April 11 2009 The extra credit is due Wednesday April 15 2009 Each problem is worth the points indicated I encourage you to work in small groups to learn this material However copying of the solution from another is not acceptable 1 Explain the importance of Chapter 12 10 points Chapter 12 covers thermodynamic properties and relations to determine thermodynamic properties This chapter develops the relationships necessary to calculate unknown properties u h and s based on properties that are known or that can be measured P T m and V The methods discussed in chapter 12 were used to develop the property tables in the appendix 3 Explain the importance of Chapter 13 10 points Chapter 13 is an extension of chapter 12 in that it covers thermodynamic properties and relations to determine thermodynamic properties Whereas chapter 12 covered the general relations this chapter is only for gas mixtures Specifically chapter 13 covers nonreacting gas mixture properties Note that chapter 15 and 16 cover reacting systems and that we will only touch on reacting mixtures in chapter 15 when discussing combustion The methods discussed in chapter 13 allow us to look at how real or ideal gases interact with each other 5 Design a simple experiment to prove a Dalton s law of additive pressures and b Amagat s law of additive volumes 15 points a Dalton s law states that the pressure of a gas mixture is equal to the sum of the pressures each gas would exert if it existed alone at the mixture temperature and volume An example would be two containers A and B with equal volume 1 liter contain a gas air at the same temperature 20 OC The gas in one container is transferred to the other container in an isothermal manner so that gases A and B are contained in one of the containers at the same initial temperature b Amagat s law states that the volume of a gas mixture is equal to the sum of the volumes each gas would exert if it existed alone at the mixture temperature and pressure An example would be two containers A and B with equal pressure 1 atm contain a gas air at the same temperature 20 OC The two containers are then combined through an in nitely small valve so that the gases mix interact with each other at the same pressure and temperature 6 Under what conditi0ns is are the mole fraction pressure fraction and volume fraction of an ideal gas the same 15 points For ideal gases the mole pressure and volume fractions are the same See page 705 and equation 138 This is important since many concentrations are given in percent parts per million ppm molar basis umolmol or partial pressure and that these units are equivalent if the ideal gas assumption is used They only differ on unit conversion 9 10 partial pressure fraction 100l000000 ppm For instance you can purchase standard reference material from NIST at httpswwwsnistgovsrmorstablesview tablecfmtablelO7lhtm The first item on this page is SRM 1674b a 7 molmol CO2 bottle or 7 CO2 by volume The remaining 93 is nitrogen N2 The partial pressure of the CO2 is 007 and N2 is 093 2 AS a R Bqu 6 20 C GUM LO Io LZMPL Frvrx Pay 17 5 913 i A QM a 539 as v 12w 5 lt33 2 37 g Egt as 9 3VgtT 37 V 02425 35 S 02 19 3mm we wen r AS 6 120 C w bdo kj 4mm 104 111qu 03C UDLvxlr c G9a 04514 MLAQ T3 omsT l PP S Cum3643 MJ 3 gt 35 BT gt a f SV AND OXU44 L 3 AS 3 53 Alp W 51mm AP 4 Izo 02MPK 303 Low 0 we accouumL pm 41 UL quotPIcgtPL2MgtP A9 Lookq a PM 2 5510p 4w PPLOVf VPsmek 22 4AQLJJ Bump FM Lt Pb h ca Knew Y vP eg em k me foM 0 4n 30 C 13 a acme qFPrOXM w 0 EV 3 3T LOHPL 139 kiwi69 W 3 9 Mam 1 8 SWM 21 2 8 7 5 m3quot 5T M a I mo 326 ZMPc D boxT o Qlgtgt I r M3 Q loslzu 1 a AS quot 31 1wa T6584 lob1gtltOvZMP gtW cgt0t9397zz r oOICWQZ EEK Table A12 R134a vP10MPa vP12MPa 90 0026492 0021506 100 0027552 0022442 110 0028584 0023348 120 0029592 0024228 130 0030581 0025086 140 0031554 0025927 150 0033457 0026753 004 A 0035 E R2 9885E01 m 003 E D 0025 g 002 39 o P10MP gt V a R2 9995E01 lg 0015 I vP12MPa 39g 001 VP10MPa 839 0005 80 90 100 110 120 130 140 150 160 Temperature C EON A 3 5 N 5020 LOMR H580 2 lt 02009 LENA 39 394 12344 M 95 msW Lissa 00130 4amp4 00197lt92 00699 mo Diagram 3 Orme o I IZZ doom 294 oatzG Ba rh 23 LSLcr o J er af fa LJ za g 61 cu 45 N0 a PBX chd 50 JOE S US quotM Ii Dan3142 M Sin 4314 AS affroxiwfg va 4 A w 62W Oz 732 U1 00 ZDCOZ09 Ar 4 Ag UM 3 DO Mate S ISM 50 i000quot M lt S Qavlqm ltW5 dxe I00 kgswtb39h f M 6W hm339g4 b otg 971376 r23 min A 3979 We 28015 3 L 28478as OOLrl2Molt 4 Li l I 7704 0 lb km 333 h s W TOM 289687 5265 39J V 02 fl MNL MCOZ 2 WM anmw Q W 257087 K 539 M4532 9189997 3397543v a 177051 N M foz 7896997 AQOOOEB 3835 MW 2397 I quot mm IIO MAN qub397b 2 3 2 962 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