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+//Example 5.12
+clear;
+clc;
+
+//Given
+HfNH4NO3=-365;//enthalpy of formation of NH4OH in kJ mol^-1
+HfH2=0;//enthalpy of formation of H2 in kJ mol^-1
+HfH2O=-242;//enthalpy of formation of H2O in kJ mol^-1
+HfN2H4=50;//enthalpy of formation of N2H4 in kJ mol^-1
+SoNH4NO3=150;//Standard entropy of NH4NO3 molecule in J K^- mol^-1
+SoH2=130;//Standard entropy of Hydrogen molecule J K^- mol^-1
+SoH2O=189;//Standard entropy of H2O molecule J K^- mol^-1
+SoN2H4=120;//Standard entropy of N2H4 molecule J K^- mol^-1
+T=298;//Temperature in K
+
+//To determine the free energy change
+delHo=(3*HfH2O)+HfN2H4-HfNH4NO3-(3*HfH2);
+delSo=(SoH2O*3)+SoN2H4-SoNH4NO3-(3*SoH2);
+delGo=delHo-(T*delSo*10^(-3));
+mprintf('Free energy change = %f kJ',delGo);
+//end
+\ No newline at end of file