Description: Slide 1: THE IDEAL-GAS EQUATION OF
Slide 2: Equation of state

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Slide 4: Real gas

Slide 5: Ideal-gas state

Slide 6: Compressibility factor (Z)

Slide 7: The farther away Z is from unity, the more the gas deviates from ideal-gas
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Slide 10: The experimentally determined Z values are plotted against PR and TR for
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Slide 12: When P and v, or T and v, are given instead of P and T, the generalized

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Slide 16: The ideal-gas equation of state is very simple, but its range of applicability

Slide 17: Van der Waals intended to improve the ideal-gas equation of state by

Slide 18: The determination of the two constants appearing
Slide 19: By performing the differentiations and eliminating vcr, the constants a and
Slide 20: Despite its limitations, the van der Waals equation of state has a historical

Slide 21: The constants appearing in the above equation are given in Table 3–4 for

Slide 22: Benedict-Webb-Rubin Equation of State

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Slide 24: Virial Equation of State
Slide 25: Volumetric data for fluids are useful for many purposes, from the
Slide 26: PV along an isotherm may be expressed as a function of P by a power
Slide 27: Parameters B’, C’, D’ in above equation are species dependent and
Slide 28: (PV)* is directly proportional to T, with R as the proportionality constant:

Slide 29: From eq (b)

Slide 30: Two Forms of the Virial Equation

Slide 31: An alternative expression for Z is also in common use

Slide 32: For ideal gases, where no molecular interaction exists, Virial coefficients B
Slide 33: The P-v-T behaviour of a substance can be represented accurately with

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