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+clc
+clear
+//Input data
+E=20;//Methanol burned with excess air in percentage 
+p=1;//Pressure of air in bar
+t=27;//Temperature of air in degree centigrade
+O=32;//The molecular weight of oxygen
+N=28;//The molecular weight of nitrogen
+R=8314;//Universal gas constant in Nm/kmolK
+C=32;//Molecular weight of methanol
+CO=44;//Molecular weight of the carbondioxide 
+H=18;//Molecular weight of the water
+
+//Calculations
+S=[(1.8*O)+(6.768*N)]/C;//Stoichiometric air/fuel ratio
+A=[(1.8*O)+(6.768*N)]/C;//Actual air/fuel ratio
+M=1.8+6.768;//1 kmole of fuel reacts with air in kmole
+V=(M*R*(t+273))/(p*10^5);//Volume of air in m^3/kmole fuel
+T=(1+1.8+6.768);//The total number of moles in the reactants when excess air is supplied in moles
+Cm=(1/T);//Mole fraction of the methanol
+Om=(1.8/T);//Mole fraction of the oxygen
+Nm=(6.768/T);//Mole fraction of the nitrogen
+Mr=(Cm*C)+(Om*O)+(Nm*N);//Molecular weight of reactants 
+Tp=(1+2+6.768+0.3);//Total number of moles in the products in moles
+COm=(1/Tp);//Mole fraction of the carbondioxide
+Hp=(2/Tp);//Mole fraction of the water 
+Np=(6.768/Tp);//Mole fraction of the nitrogen
+Op=(0.3/Tp);//Mole fraction of the oxygen
+Mp=(COm*CO)+(Hp*H)+(Np*N)+(Op*O);//Molecular weight of products
+Pp=(Hp*p);//Partial pressure of water vapour in bar
+D=60;//The dew point is the saturation temp corresponding to partial pressure in degree centigrade
+
+//Output
+printf(' (a) The volume of air supplied per kmole of fuel = %3.1f m^3/kmole fuel \n (b) The molecular weight of the reactants = %3.2f \n The molecular weight of the products = %3.2f \n (c) The dew point of the products = %3.0f degree centigrade ',V,Mr,Mp,D)