AT 400 degree C the gas-phase reaction CO(g) + H_2O(g) CO_2(g) + H_2(g) was expl

Question

AT 400 degree C the gas-phase reaction CO(g) + H_2O(g) CO_2(g) + H_2(g) was explored. The initial concentrations used were as follows: 2.00 M CO, 2.00 M H_2O, 0.00 M CO_2, 0.15 M H_2. The reaction was followed until the concentrations of the reactants and products showed no further change with time. At this point, the concentration of H_2 was found to be 1.65 M. The equilibrium constant of this reaction at 400 degree C is: At 1000 K, iron metal is produced through the reaction FeO(s) + CO_(g) Fe(s) + CO_2(g). At this temperature, the equilibrium constant of the reaction is K_c = 0.259. An experiment is conducted starting from a mixture containing a solid phase consisting of 4 moles of FeO and 2 moles of F_e and a gas phase consisting of 1.000 M CO and 0.500 M CO_2. The reaction was followed until the concentrations of the reactants and products showed no further change with time. At this point, the concentration of CO_2 attained a constant level of:

Explanation / Answer

CO + H2O <-> CO2 + H2

[CO] = 2

[H2O] = 2

[CO2] = 0

[H2] = 0.15

In equilibrium

[CO] = 2 - x

[H2O] = 2 - x

[CO2] = 0 + x

[H2] = 0.15 + x

and [H2] = 0.15 + x = 1.65

solve for x = x = 1.65-0.15 = 1.5

then

[CO] = 2 - 1.5 = 0.5

[H2O] = 2 - 1.5 = 0.5

[CO2] = 0 + 1.5 = 1.5

[H2] = 0.15 + x = 1.65

K = [H2][CO]/ [CO2][H2O] = 1.65*1.5 / (0.5*0.5)= 9.9

K = 9.9

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