The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached? The equilibrium constant, K c, is equal to 1.4 at 1200° K for the reaction: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) If 0.35 moles of CO2 and 0.35 moles of H2 are introduced into a 1.0-L flask, what will be the concentration of CO when equilibrium is reached?
A.0.19 M
B.0.24 M
C.0.22 M
D. 0.16 M
since volume is 1 L, concentration will be same as number of moles
CO2(g) + H2(g) ⇌ CO(g) + H2O(g)
0.35 0.35 0 0 (initial)
0.35 -x 0.35-x x x (at equilibrium)
Kc = [CO][H2O]/[CO2][H2]
1.4 = x*x / (0.35-x)*(0.35-x)
1.4 = x^2 / (0.35-x)^2
sqrt(1.4) = x / (0.35-x)
x / (0.35-x) = 1.18
x = 0.413 - 1.18*x
2.18*x = 0.413
x = 0.19 M
So,
[CO] = x = 0.19 M
Answer: A
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