2.30 Consider the following set of equilibrium reactions: CH4(g)+H2O(g)CO(g)+H2O(g)CO(g)+3H2(g)CO2(g)+H2(g) At 2000K the equilibrium constants for these reactions are 1.930104 and 5.528, respectively. Initially, a gas containing 20%CH4(g) and 80%H2O(g) is present at 2000K and 1.0 atmosphere pressure. Choose a basis of 10 moles of gas, and let e1 be the degree of reaction for the first reaction and 2 the degree of reaction for the second reaction. The equilibrium constants can be written as Now the equilibrium mole fractions can be written as YCOYH2YH2OYCO2YCH4=10+2e1e1e2=10+2e13e1+e2=10+2e18e1e2=10+2e1e2=10+2e12e1 Substituting these relationships into the equilibrium constant expressions yields (2e1)(8e1e2)(10+2e1)2(e1e2)(3e1+e2)3(e1e2)(8e1e2)e2(3e1+e2)=1.930104=5.528 Solve for the equilibrium gas composition for this system