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Understanding Thermodynamics of Wet, Saturated & Superheated Vapor

Dive into the complexities and properties of vapor mixtures, critical points, and compressibility factors with detailed equations and explanations. Explore the behavior of real gases with Van der Waals EOS, compressibility charts, and more.

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Understanding Thermodynamics of Wet, Saturated & Superheated Vapor

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  1. Thermodynamics of Wet, Saturated & Superheated Vapor P M V Subbarao Professor Mechanical Engineering Department I I T Delhi Insearch of Simple Pfaffian Substance …..

  2. Specific Volume of Wet Mixture

  3. More Properties of Wet Mixture

  4. Let Y be any extensive property and let y be the corresponding intensive property, Y/m, then

  5. Vapour Dome • Saturated Liquid Line and Saturated vapour line intersect at the critical point and form what is often called the “vapour dome.” Water Critical Point:

  6. Pressure – Temperature Diagram of a Pure Substance

  7. Vapour • Temperature of the substance is higher than the saturation temperature at a given pressure. • Pressure of the substance is lower than the saturation pressure at a given temperature. • Molecules of substance move in random paths. • Weak inter-molecular forces. • Occupy entire volume of the container : No free surface. • Very low density • Highly compressible.

  8. p-v-T Relations for Vapour Phase • At high Temperature and low pressure pv is constant at a given temperature. • This nature is called Ideal gas behaviour of gases. T1 T2

  9. Behaviour of Vapour •  = interatomic potential, Joules. • r = separation of molecules, nm (mean Free path). • r = equivalent “hard sphere” radius of molecule (overlap of electron clouds). • At high T, high p, collisions in the repulsive part of – positive deviations from constancy. • At low T, moderate p, collisions in the attractive portion of  – negative deviations from constancy.

  10. The specific volume of A vapour: • v = f (p,T) P – v- T Relation • Greatest need for EoS of saturated and superheated steam. • R and a are constants. • The is called as Rankine’s Equation of state, 1849.

  11. The specific volume of A vapour: • v = f (p,T) P – v- T Relation • Callender’s Characteristic Equation for saturated and superheated vapours. • R and b are constants. • c is a function of temperature and itis called as co-aggregation volume.

  12. Pressure Volume Diagram

  13. Van der Waals EOS • One of the oldest but most extensively used of the EOS of non ideal gases • Any EOS model must reproduce graphs such as that of the previous • a, b are the Van der Waals constants for the particular gas; • for water: a = 0.5658 J-m3/mole2; b = 3.049x10-5m3/mole,

  14. JO H A N N E S D . V A N D E R W A A L SThe equation of state for gases and liquidsNobel Lecture, December 12, 1910 I intend to discuss in sequence: (1) the broad outlines of my equation of state and how I arrived at it; (2) what my attitude was and still is to that equation; (3) how in the last four years I have sought to account for the discrepancies which remained between the experimental results and this equation; (4) how I have also sought to explain the behaviour of binary and ternary mixtures by means of the equation of state.

  15. Van der Waals EOS • a, b are the Van der Waals constants for the particular gas; • for water: a = 0.5658 J-m3/mole2; b = 3.049x10-5 m3/mole,

  16. Van der Waals Isotherms

  17. Isotherms of Real Gases

  18. Improved Cubic Equations of State

  19. The constants a, b, c, Ao, Bo varies with substance

  20. Compressibility Factor • The deviation from ideal gas behaviour can also be expressed by compressibility factor, Z. • The ratio of volume of real gas, Vreal to the ideal volume of that gas, Vperfect calculated by ideal gas equation is known as compressibility factor.

  21. Compact description of non-ideality: the compressibility factor, Z  1 as p  0 (ideality) Z < 1 at low T, moderate p (point A) Z > 1 at high p, high T (point B)

  22. Generalized Compressibility Chart Reduced Temperature TR = T/Tc Reduced Pressure pR= p/pc

  23. VdW EOS & Compressibility • arepresents the attractive part of the potential; with b = 0, the VdW EOS gives a smaller v for the same T than the ideal gas • brepresents the repulsive portion of the potential; with a= 0, the VdW EOS gives a larger v for the same T than the ideal gas • The VdW EOS is easily expressed in the forms p(T,v) or T(p,v). • For the v(T,p) form, or, equivalently, Z(p,T):

  24. The ideal gas equation of state may be written several ways.

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