**6. Algorithm of the Calculation in AsTher **

6.1.1. Ideal gas - Clapeyron, 1834

6.1.2. Van der Waals, 1873

6.1.3. Redlich-Kwong, 1949

6.1.4. Generalized Redlich-Kwong, 1949

6.1.5. Redlich-Kwong Vapour-Liquid-Equilibrium, 1949

6.1.6. Soave Modification of Redlich-Kwong Vapour-Liquid-Equilibrium, 1972

6.1.7. Peng Robinson Vapour-Liquid-Equilibrium, 1976

6.2.1. State functions in depend of specific heat capacity and compressibility

6.2.2. Residual value of state function based on cubic equation of state

6.2.3. State functions based on correlation of measurements

6.4. Calculation of the Equilibrium

**6. 1. Behaviour of the System **

When the critical constants Tc, Pc are known, the state functions can be calculated
using real gases rules.

The behaviour of the system can be selected separately in each AsTher application.

The Generalized Redlich-Kwong equation of state (1949) is set as default.

Menu **System -> Behaviour** shows a window, in which the equation of state
can be selected to calculation.

6.1.1. Ideal gas - Clapeyron, 1834

State Functions are calculated corresponding to the equations in Cap. 6.2.1

*a = 27 ^{ . }R^{2} ^{.}T_{c}^{2}/( 64
^{. }P_{c} )*

b =R

State Functions are calculated corresponding to the equations in
Cap. 6.2.1

6.1.3. Redlich-Kwong, 1949

*a = 0.42748 ^{ . }R^{2} ^{.}Tc^{5/2} / Pc*

*b = 0.08664 .R .Tc / Pc*

State Functions are calculated corresponding to the equations in Cap. 6.2.1

6.1.4. Generalized Redlich-Kwong, 1949

*a = 0.42748 ^{ . }R^{2} ^{.}Tc^{2} / Pc*

b = 0.08664

h = 0.08664

State Functions are calculated corresponding to the equations in Cap. 6.2.1

6.1.5. Redlich-Kwong Vapour-Liquid-Equilibrium, 1949

State Functions, compressibility and liquid volume are calculated corresponding
to the equations in Cap. 6.2.2

**6.1.6. Soave Modification of Redlich-Kwong** Vapour-Liquid-Equilibrium,
1972

* α(T,ω)* equation is
due to

State Functions, compressibility and liquid volume are calculated corresponding to the equations in Cap. 6.2.2

**6.1.7. Peng Robinson **
Vapour-Liquid-Equilibrium, 1976

State Functions, compressibility and liquid volume are calculated corresponding to the equations in Cap. 6.2.2

Reference of the enthalpy values: enthalpy of elementar substances is zero at 25C and 1 bar in usual natural state.

The Cp –Function is calculated according to

*Cp = *
*a** + 10 ^{-3 .} *

* a, b, c, d, e, f: *empiric values in the
AsTher Database from different sources, T [K]: Temperature.

If the constants are known according to the **Shomate
Equation**

*Cp = A + B .(T/1000) + C .(T/1000)² + D
.(T/1000)³ + E .(T/1000)*^{-}²

then the constants can be replaced in AsTher database corresponding to the
following table

**Important**: **Ref**.-Field in the dataset must not contain "[<**hgt**>]",
when ** Shomate **constants are
used in a dataset

Constants in Shomate Equation |
equal to the constantsin AsTher database |

A |
a |

B |
b |

E |
c |

C |
d |

0 (Zero) |
e |

D |
f |

**6.2.1. State functions in depend of specific heat
capacity and compressibility**

The molar enthalpy is calculated according to

The molar entropy is calculated according to

The molar free energy is calculated according to

**6.2.2. Residual value of state function based on cubic equation of state**

from Smith, Van Ness, and Abbott (Introduction to Chemical Engineering
Thermodynamics, 7th ed.)

Z: compressibility for **vapours**:

Z: compressibility for **liquids**:

**6.2.3. State functions based on correlation of measurements **

In several datasets, the calculations of H(T) and G(T) base on the measured data
in small
temperature range in non-ideal equilibrium state, without the
Cp-correlation,
when **reference is [<hgt>]**.

In such case.

* a, b, c, d, e, f: *empiric values in the
AsTher Database according to different sources.

When the extrapolation is not enabled, the calculations will be not are carried out and the reason is shown in the a messages window.

6.4.
Calculation of the Equilibrium in
the Application Equilibrium

The state of equilibrium is defined by following relations:

or

Free enthalpy of the pure substance at temperature and pressure of the thermodynamic system

** a_{i}:** Activity of the compound in the thermodynamic system

For the mass balance, following relations is valid:

* N_{e}*: Mol number of the element

For any reaction the criteria of the equilibrium have to be fulfilled.

Evidence of the Correctness and Consistency:

Take any possible reaction within a given system:

*a A (s) + b B (g) = c C (l) *

First calculate the equilibrium constant K using the calculated values of the partial pressures and/or activities:

then calculate the equilibrium constant K via the Gibbs (free) energy:

Compare the *K* values from both equation

The Gibbs free energies can be calculated by the AsTher-Application **Pure Substance** at the given temperature of the system.

The change of the free energy can be calculated also by the AsTher-Application **Reaction**.

The results are allways within the selected accuracy.

Abs. 3.3. shows an example for the argumentation of consistency.