Develop a python code for the example 5.7

Example 5.7 Hydrogen can be manufactured from the Solution For the first reaction: reaction between methane and steam over a catalyst. Two principal reactions occur: CH4+H2O3H2+CO=30+(209,084)30,358(187,052)Ka1=307.42 carbonmonoxideCO+waterH2OhydrogenH2+carbondioxideCO2 For the second reaction: Assuming the reaction takes place at 1100K and 20bar, calculate the equilibrium conversion for a molar ratio of steam to methane in the feed of 3,4,5 and 6 . Assume ideal gas behavior (K=1, R=8.3145kJK1kmol1). Thermodynamic data for a standard pressure of 1 bar are given in Table 5.12. G2ORTlnKa2Ka2=GH2O+GCO2OGCOOGH2OO=0+(359,984)(209,084)(187,052)=36,152kJ=36,152=1.9201102 Let r be the molar ratio of water to methane in the feed, X1 be the Table 5.12 conversion of the first reaction and X2 be the conversion of the Thermodynamic data for hydrogen manufacture (Lida, 2010). second reaction. 1X1CH4+rX1X2H2O3X1+X1X2COX1X2CO+rX1X2H2OX2X2H2 Total moles at equilibrium =(1X1)+(rX1X2)+3X1+ (X1X2)+X2+X2 =r+1+2X1 Mole fractions are presented in Table 5.13. Table 5.13 Mole fractions at equilibrium for the manufacture of hydrogen