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CHEE 311Lecture 111 Fugacity of Non-Ideal Mixtures (SVNA 11.6 and 11.7) In our attempt to describe the Gibbs energy of real gas and liquid mixtures, we.

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Presentation on theme: "CHEE 311Lecture 111 Fugacity of Non-Ideal Mixtures (SVNA 11.6 and 11.7) In our attempt to describe the Gibbs energy of real gas and liquid mixtures, we."— Presentation transcript:

1 CHEE 311Lecture 111 Fugacity of Non-Ideal Mixtures (SVNA 11.6 and 11.7) In our attempt to describe the Gibbs energy of real gas and liquid mixtures, we examine two “sources” of non-ideal behaviour:  Pure component non-ideality due to PVT behaviour »concept of fugacity  Non-ideality in mixtures »partial molar properties »mixture fugacity and residual properties We will begin our treatment of non-ideality in mixtures by considering gas behaviour.  Start with an ideal gas mixture expression.  Modify this expression for cases where pure component non- ideality is observed.  Further modify this expression for cases in which non-ideal mixing effects occur.

2 CHEE 311Lecture 112 Ideal Gas Mixtures In an ideal gas mixture  all molecules have negligible volume  interactions between molecules of any type are negligible. Based on this model, the chemical potential of any component in a perfect gas mixture is: where the reference state, G i ig (T,P) is the pure component Gibbs energy at the given P,T.  For a pure ideal gas, we derived:

3 CHEE 311Lecture 113 Ideal Gas Mixtures Substitute to get: (11.29) which is the chemical potential of component i in an ideal gas mixture at T,P. The total Gibbs energy of the ideal gas mixture is the sum of the contributions from the individual components: (11.11) (11.30)

4 CHEE 311Lecture 114 Ideal Mixtures of Real Gases Consider an ideal solution of real gases.  The molecules have finite volume and interact, but assume these interactions are equivalent between components The appropriate model is that of an ideal solution: where G i (T,P) is the Gibbs energy of the real pure gas: (11.31) Our ideal solution model applied to real gases is therefore:

5 CHEE 311Lecture 115 Non-Ideal Mixtures of Real Gases In cases where molecular interactions differ between the components (polar/non-polar mixtures) the ideal solution model does not apply  Our knowledge of pure component fugacity is of little use in predicting the mixture properties  We require experimental data or correlations pertaining to the specific mixture of interest To cope with highly non-ideal gas mixtures, we define a mixture fugacity: (11.47) where f i is the fugacity of species i in solution, which replaces the product y i P in the perfect gas model, and y i f i of the ideal solution model.

6 CHEE 311Lecture 116 Non-Ideal Mixtures of Real Gases To describe non-ideal gas mixtures, we define the solution fugacity: and the fugacity coefficient for species i in solution: (11.52) In terms of the solution fugacity coefficient: Notation: f i,  i - fugacity and fugacity coefficient for pure species i f i,  i - fugacity and fugacity coefficient for species i in solution

7 CHEE 311Lecture 117 Calculating  i v from Compressibility Data Consider a two-component vapour of known composition at a given pressure and temperature  If we wish to know the chemical potential of each component, we must calculate their respective fugacity coefficients In the laboratory, we could prepare mixtures of various composition and perform PVT experiments on each.  For each mixture, the compressibility (Z) of the gas can be measured from zero pressure to the given pressure.  For each mixture, an overall fugacity coefficient can be derived at the given P,T:  How do we use this overall fugacity coefficient to derive the fugacity coefficients of each component in the mixture?

8 CHEE 311Lecture 118 Calculating  i v from Compressibility Data The mixture fugacity coefficients are partial molar properties of the residual Gibbs energy, and hence partial molar properties of the overall fugacity coefficient: In terms of our measured compressibility:

9 CHEE 311Lecture 119 Calculating  i v from the Virial EOS We know how to use the virial equation of state to calculate the fugacity and fugacity coefficient of pure, non-polar gases at moderate pressures.  The virial equation can be generalized to describe the calculation of mixture properties. The truncated virial equation is the simplest alternative: where B is a function of temperature and composition according to: (11.61) B ij characterizes binary interactions between i and j; B ij =B ji

10 CHEE 311Lecture 1110 Calculating  i v from the Virial EOS Pure component coefficients (B 11 ≡ B 1, B 22 ≡ B 2,etc) are calculated as previously and cross coefficients are found from: (11.69b) where, and ( ] B o and B 1 for the binary pairs are calculated using the standard equations 3.65 and 3.66 using T r =T/T cij.

11 CHEE 311Lecture 1111 Calculating  i v from the Virial EOS We now have an equation of state that represents non-ideal PVT behaviour of mixtures: or We are equipped to calculate mixture fugacity coefficients from equation 11.60

12 CHEE 311Lecture 1112 Calculating  i v from the Virial EOS The result of differentiation is: (11.64) with the auxiliary functions defined as: In the binary case, we have (11.63a) (11.63b)

13 CHEE 311Lecture Calculating  i v from the Virial EOS Method for calculating mixture fugacity coefficients: 1. For each component in the mixture, look up: T c, P c, V c, Z c,  2. For each component, calculate the virial coefficient, B 3. For each pair of components, calculate: T cij, P cij, V cij, Z cij,  ij and using T cij, P cij for B o,B 1 4. Calculate  ik,  ij and the fugacity coefficients from:


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