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+//Example 8.9
+clear;
+clc;
+
+//Given
+T1=298;//initial temperature in K
+T2=1073;//final temperature in K
+R=8.314;//gas constant in J K^-1 mol^-1
+delGfoH2=0;//standard free energy change in the formation of hydrogen in kJ mol^-1
+delGfoC0=-137.27;//standard free energy change in the formation of CO in kJ mol^-1
+delGfoH2O=-228.59;//standard free energy change in the formation of water in kJ mol^-1
+delGfoC02=-394.38;//standard free energy change in the formation of CO2 in kJ mol^-1
+delHfoH2=0;//standard enthalpy in the formation of hydrogen in kJ mol^-1
+delHfoC0=-110.52;//standard enthalpy in the formation of CO in kJ mol^-1
+delHfoH2O=-241.83;//standard enthalpy in the formation of water in kJ mol^-1
+delHfoC02=-392.51;//standard enthalpy in the formation of CO2 in kJ mol^-1
+
+//To determine the value of Kp at T1 and T2
+delGo=delGfoH2+delGfoC02-(delGfoC0+delGfoH2O);//free energy change in kJ mol^-1
+delHo=delHfoH2+delHfoC02-(delHfoC0+delHfoH2O);//standard enthalpy change in kJ mol^-1
+k1=(-1000*delGo)/(R*T1);//k=log(Kp)
+Kp1=exp(k1);//equillibrium constant Kp at 298 K
+mprintf('Equillibrium constant,Kp at 298 K = %f ',Kp1);
+k2=((-1000*delHo/R)*((1/1073)-(1/298)))+k1;//equillibrium constant at 1073 K
+Kp2=exp(k2);//equillibrium constant Kp at 1073 K
+mprintf('\n Equillibrium constant,Kp at 1073 K = %f ',Kp2);
+//end
+\ No newline at end of file