PLEASE HELP CHEM!!
posted by scilover .
5.6 x 106 mol of A and 5 x 105 mol of B are mixed in a 200 mL flask. The system is represented by the equation:
2A(G) + B(G) <> 3C(G)
At equilibrium, there is 4.8 x 105 mol of B. Calculate the value of the equilibrium constant.

(A) = 5.6E6/0.2 = 2.8E5M
(B) = 5E5/0.2 = 2.5E4M
.........2A + B ==> 3C
I.....2.8E5..2.5E4..0
C.......2x...x....3x
E...2.8E52x..2.5E4x...3x
We know B at equilibrium = 4.8E5 mol/0.2L = 2.4E4; therefore,
2.5E4x = 2.4E4
Solve for x which lets you work out A and C at equilibrium. Then substitute into Keq expression and solve for K.
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