Question

Consider the chemical reaction given. The initial concentrations of CO (g) and H2O (g) are 0.35...

Consider the chemical reaction given. The initial concentrations of CO (g) and H2O (g) are 0.35 M and 0.40 M respectively (there is no CO2 of H2 present initially). At equilibrium it is found that the concentration of CO2(g) is 0.19 mol/L. What is the value of the equilibrium constant for this reaction?

CO(g)+H2O(g)-><- CO2(g) +H2 (g)

a. 1.1

b. 0.9

c. 0.56

d. 0.40

e. 0.36

The key says the answer is A, but I do not know how to solve it... please help!

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Answer #1

CO(g) + H2O(g) <------> CO2(g) +H2 (g)
0.35       0.40              0      0       (initial)
0.35-x     0.40-x            x      x    (at equilibrium)

At equilibrium,
[CO2] = 0.19 M
so, x = 0.19 M

Kc = [CO2][H2]/[CO][H2O]
Kc = x*x / (0.35-x)(0.40-x)
Kc = 0.19*0.19 / (0.35-0.19)(0.40-0.19)
Kc = 0.0361 / (0.16*0.21)
Kc = 1.1

Answer: a

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