01 part2-ideal-gas-problems-01
Download as PPTX, PDF1 like3,730 views
The document discusses ideal gas properties including the ideal gas equation of state, units of pressure, gas constants for common gases, specific volume, molar volume, and specific heat. It provides sample problems and questions to calculate things like molecular weight and gas constant given specific heat values for a gas. The document is intended as a reference for understanding fundamental concepts relating to ideal gases and thermodynamics.
01 part2-ideal-gas-problems-01
- 1. Ideal Gas S.Gunabalan Associate Professor Mechanical Engineering Department Bharathiyar College of Engineering & Technology Karaikal - 609 609. e-Mail : gunabalans@yahoo.com Part - 2
- 2. Ideal Gas Equation of state
- 3. Ideal Gas Equation of state
- 4. Ideal Gas Equation of state
- 5. Ideal Gas Equation of state
- 6. Ideal Gas Equation of state
- 7. Units of Pressure • atmospheric pressure (1 Atm.) = 1.013 bar, = 101325 Pascal (Pa = N/m²); = 760 millimeters of mercury absolute (mmHgA) = 760 Torr (1 Torr = 1 mm HgA)
- 8. Gas Constant R Gas Molar Weight ( M)Kg/Kmol Gas Constant (R )KJ/KgK Air 28.97 0.287 Nitrogen 28.01 0.297 Oxygen 32 0.260 Hydrogen 2.016 4.124 Helium 4.004 2.077 Carbon dioxide 44.01 0.189 Steam 18.02 0.461
- 9. The specific volume of a substance is the ratio of the substance's volume to its mass. It is the reciprocal of density and is an intrinsic property of matter. Substance Name Density Specific Volume Kg/m3 m3/Kg Air 1.2 0.83 Ice 916.7 0.00109 Water (liquid) 1000 0.00100 Salt Water 1030 0.00097 Mercury 13546 0.00007
- 11. Specific heat
- 12. Specific heat • The specific heat - the amount of heat required to raise a unit mass of the substance through a unit rise in temperature. • The product of mass and specific heat (mCv) is called the heat capacity(Cv) at constant volume (J/K) • The latent heat is the amount of heat transfer required to cause a phase change in unit mass of a substance at a constant pressure and temperature
- 13. Questions -1
- 14. Gas Molar Weight ( M)Kg/Kmol Air 28.97 Nitrogen 28.01
- 19. Gas Molar Weight ( M)Kg/Kmol Air 28.97 Nitrogen 28.01 J = Nm
- 25. When work is done by a system, it is arbitrarily taken to be positive, and when work is done on a system, taken to be negative
- 27. Exercise-1
- 28. Question-2
- 29. Procedure
- 30. Procedure
- 31. Given data V = 60 liters of CO2 P = 10 bar T = 20 °C atmospheric pressure (1 Atm.) 1 Atm = 1.013 bar, 1 Atm = 101325 Pascal (Pa = N/m²); Unit conversion 1 bar = 1x 105 N/m2 1 m3 = 1000 liters J = Nm
- 32. Given data V = 60 liters of CO2 P = 10 bar T = 20 °C Gas Molar Weight ( M) Kg/Kmol Gas Constant (R) KJ/KgK Air 28.97 0.287 Nitrogen 28.01 0.297 Oxygen 32 0.260 Hydrogen 2.016 4.124 Helium 4.004 2.077 Carbon dioxide 44.01 0.189 Steam 18.02 0.461 atmospheric pressure (1 Atm.) 1 Atm = 1.013 bar, 1 Atm = 101325 Pascal (Pa = N/m²); Unit conversion 1 bar = 1x 105 N/m2 1 m3 = 1000 liters J = Nm
- 33. Gas Molar Weight ( M) Kg/Kmol Gas Constant (R) KJ/KgK Air 28.97 0.287 Nitrogen 28.01 0.297 Oxygen 32 0.260 Hydrogen 2.016 4.124 Helium 4.004 2.077 Carbon dioxide 44.01 0.189 Steam 18.02 0.461 atmospheric pressure (1 Atm.) 1 Atm = 1.013 bar, 1 Atm = 101325 Pascal (Pa = N/m²); Unit conversion 1 bar = 1x 105 N/m2 1 m3 = 1000 liters J = Nm
- 34. Gas Molar Weight ( M) Kg/Kmol Gas Constant (R) KJ/KgK Air 28.97 0.287 Helium 4.004 2.077 Carbon dioxide 44.01 0.189 Steam 18.02 0.461 P = 10 bar = 10 x 105 N/m2 V = 60 liters = 60/1000 m3 ⤫M = find ⤫R = cal for the substitution T = 20 °C = 20 +273 K
- 35. Given data V = 60 liters of CO2 P = 10 bar T = 20 °C
- 36. Given data V = 60 liters of CO2 P = 10 bar T = 20 °C
- 37. Exercise -2 Find the molecular weight and gas constant for the gas, whose specific heats are as follows Cp = 1.967 KJ/Kg K Cv = 1.507 KJ/Kg K
- 38. Exercise -2
- 39. Reference • Rajput, R. K. 2010. Engineering thermodynamics. Jones and Bartlett Publishers, Sudbury, Mass. • Singh, O. 2003. Applied thermodynamics. New Age International (P) Ltd., Publishers, New Delhi. • Nag, P. K. 2002. Basic and applied thermodynamics. Tata McGraw-Hill, New Delhi.
Editor's Notes
- #3: http://pages.towson.edu/ladon/gases.htmlhttp://rsnr.royalsocietypublishing.org/content/early/2009/10/12/rsnr.2009.0038.fullUse Kg mole = K moleAn ideal gas has the following properties: 1. An ideal gas is considered to be a "point mass". A point mass is a particle so small, its mass is very nearly zero. This means an ideal gas particle has virtually no volume. 2. Collisions between ideal Gases are "elastic". This means that no attractive or repulsive forces are involved during collisions. Also, the kinetic energy of the gas molecules remains constant since theses interparticle forces are lacking.
- #4: http://pages.towson.edu/ladon/gases.htmlhttp://rsnr.royalsocietypublishing.org/content/early/2009/10/12/rsnr.2009.0038.fullAn ideal gas has the following properties: 1. An ideal gas is considered to be a "point mass". A point mass is a particle so small, its mass is very nearly zero. This means an ideal gas particle has virtually no volume. 2. Collisions between ideal Gases are "elastic". This means that no attractive or repulsive forces are involved during collisions. Also, the kinetic energy of the gas molecules remains constant since theses interparticle forces are lacking.
- #5: http://pages.towson.edu/ladon/gases.htmlhttp://rsnr.royalsocietypublishing.org/content/early/2009/10/12/rsnr.2009.0038.fullAn ideal gas has the following properties: 1. An ideal gas is considered to be a "point mass". A point mass is a particle so small, its mass is very nearly zero. This means an ideal gas particle has virtually no volume. 2. Collisions between ideal Gases are "elastic". This means that no attractive or repulsive forces are involved during collisions. Also, the kinetic energy of the gas molecules remains constant since theses interparticle forces are lacking.
- #6: http://pages.towson.edu/ladon/gases.htmlhttp://rsnr.royalsocietypublishing.org/content/early/2009/10/12/rsnr.2009.0038.fullAn ideal gas has the following properties: 1. An ideal gas is considered to be a "point mass". A point mass is a particle so small, its mass is very nearly zero. This means an ideal gas particle has virtually no volume. 2. Collisions between ideal Gases are "elastic". This means that no attractive or repulsive forces are involved during collisions. Also, the kinetic energy of the gas molecules remains constant since theses interparticle forces are lacking.
- #7: http://pages.towson.edu/ladon/gases.htmlhttp://rsnr.royalsocietypublishing.org/content/early/2009/10/12/rsnr.2009.0038.fullAn ideal gas has the following properties: 1. An ideal gas is considered to be a "point mass". A point mass is a particle so small, its mass is very nearly zero. This means an ideal gas particle has virtually no volume. 2. Collisions between ideal Gases are "elastic". This means that no attractive or repulsive forces are involved during collisions. Also, the kinetic energy of the gas molecules remains constant since theses interparticle forces are lacking.
- #28: Ans: 1) 28 kg, 12.37 bar,0.089 m3/kg2) Cp = 1.038 kJ/kgkcv = 0.745 kJ/kgk3) 10.22 bar; 4) u= -52.16 KJ/Kgh = -72.69 KJ/KgS = -0.1536kJ/kgkQ= 1465.1 KJ
- #38: Ans 180.461 KJ/Kg K
- #39: Ans 180.461 KJ/Kg K