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Question

The value of Kc=4.24 at 800K for the reaction
CO(g)+H2OCO2(g)+H2(g)
Calculate equilibrium concentrations of CO2,H2,CO and H2O at 800K, if any CO and H2O are present initially at concentration of 0.10 M each?

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Solution

CO(g)+H2O(g)CO2(g)+H2(g)
moles
at t=0 0.1 0.1 - -
at Eqbm 0.1x 0.1x x x

KC=[CO2][H2][CO][H2O]=x2(0.1x)2
4.24=x2(0.1x)2
x0.1x=2.05
x=0.2052.05x
x=0.0675
Thus concentration at Eqbm of
[CO2]=[H2]=x=0.0675M
[CO]=[H2O]=0.1x=0.0324M

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