At 500 o C , K p = 5.5 for thereaction CO (g) + H 2 O = CO 2(g) + H 2(g) a) If a

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At 500 oC , Kp = 5.5 for thereaction             CO(g) + H2O = CO2(g) + H2(g) a) If a mixture of 1 mol of Co and 5 mol ofH2O is passed over a catalyst at this temperature and apressure of 2 bar what will be the equilibrium mole fraction ofH2O. b) What effect will there be of reducing the temperature ofthe reaction to 400K. State any assumptions you make in answeringthis. At 500 oC , Kp = 5.5 for thereaction             CO(g) + H2O = CO2(g) + H2(g) a) If a mixture of 1 mol of Co and 5 mol ofH2O is passed over a catalyst at this temperature and apressure of 2 bar what will be the equilibrium mole fraction ofH2O. b) What effect will there be of reducing the temperature ofthe reaction to 400K. State any assumptions you make in answeringthis. a) If a mixture of 1 mol of Co and 5 mol ofH2O is passed over a catalyst at this temperature and apressure of 2 bar what will be the equilibrium mole fraction ofH2O. b) What effect will there be of reducing the temperature ofthe reaction to 400K. State any assumptions you make in answeringthis.

Explanation / Answer

   We know that :         The given Reactionis :          CO(g) +H2O  <--------> CO2(g)+ H2(g)    I:    1             5                           0         0    C: -x              -x                         +x          +x     E: 1-x          5-x                        + x          +x              5.5 =   [ x ] [ x ] / [ 1-x ] [ 5-x]             solving the above equation we get :           x = 0.9586 M       The equilibrium molesof H2O is 5 - 0.9586 =   4.014moles          Totalequilibrium moles = 6 ( 1-x + 5-x + x +x )          XH2O =  4.014 moles / 6moles                     =       0.669      If we decrease the temperature theequilibrium constant value decreases so correspondingly theequilibrium concentration also decreases.                       

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