For the reaction: N2 (g) + C2H2 (g) 2 HCN (g), Kc is 2.3x10-4 at 300 ºC. What are the equilibrium concentrations of all species if the initial concentration of HCN was 5.0 M?
ICE Table:
Equilibrium constant expression is
Kc = [HCN]^2/[N2]*[C2H2]
2.3*10^-4 = (5-2*x)^2/(1*x)^2
sqrt(2.3*10^-4) = (5-2*x)/(1*x)
0.0151658 = (5-2*x)/(1*x)
1.517*10^-2*x = 5-2*x
-5 + 2.015*x = 0
x = 2.48119
At equilibrium:
[N2] = +1x = +1*2.48119 = 2.48119 M
[C2H2] = +1x = +1*2.48119 = 2.48119 M
[HCN] = 5.0-2x = 5.0-2*2.48119 = 0.03763 M
Answer:
[N2] = 2.48 M
[C2H2] = 2.48 M
[HCN] = 0.0376 M
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