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+// Y.V.C.Rao ,1997.Chemical Engineering Thermodynamics.Universities Press,Hyderabad,India.
+
+//Chapter-14,Example 3,Page 491
+//Title: Equilibrium constant
+//================================================================================================================
+clear 
+clc
+
+//INPUT
+//The water gas shift reaction is given by: CO2(g)+H2(g)--->CO(g)+H2O(g)
+T1=298.15;//initial temperature in K
+Ka1=8.685*10^-6;//equilibrium constant for the water-gas shift reaction at T1 (no unit)
+T2=1000;//temperature at which the equilibrium constant has to be determined in K
+R=8.314;//universal gas constant in J/molK
+del_Hf=[-110.532;-241.997;-393.978;0];//the standard enthalpy of formation of CO(g),H2O(g),CO2(g) and H2(g) in kJ
+n=[1;1;-1;-1];//stoichiometric coefficients of CO(g),H2O(g),CO2(g) and H2(g) respectively (no unit)
+
+//CALCULATION
+//It is assumed that del_H is constant in the temperature range T1 and T2
+del_H=(n(1,:)*del_Hf(1,:))+(n(2,:)*del_Hf(2,:))+(n(3,:)*del_Hf(3,:))+(n(4,:)*del_Hf(4,:));//calculation of the standard enthalpy of the reaction in kJ
+Ka2=Ka1*exp(((del_H*10^3)/R)*((1/T1)-(1/T2)));//calculation of the equilibrium constant at T2 (no unit)
+
+//OUTPUT
+mprintf('The equilibrium constant for the water gas shift reaction at 1000K=%f \n',Ka2);
+
+
+//===============================================END OF PROGRAM===================================================
+
+
+
+