A + 2 B ⇌ C What are the equilibrium concentrations of A, B and C if 2.6 mol A and 2.6 mol B are added to a 1.0 L flask? Assume that the equilibrium constant for this reaction is Kc = 1.7x10^15.
A + 2 B <----------------> C
2.6mol 2.6 mol 0
2.6-x 2.6-2x x
Kc = [C] / [A] [B]^2
1.7 x 10^15 = x / (2.6-x)(2.6 - 2x)^2
1.7 x 10^15 = x / (2.6 - x) (4x^2 - 10.4x + 6.76)
1.7 x 10^15 = x / (2.6 - x) (4x^2 - 10.4x + 6.76)
by solving the above equation :
x = 1.30
equilibrium concentrations :
[A] = 1.3 M
[B] = 0.0 M
[C] = 1.3 M
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