[mcduffels]

Calculate of the value of the equilibrium constant K for the following reaction:

A + B <=> C

from the following information:

2C <=> D    Kc = 5.7 x 10^-4

D <=> 2A + 2B   Kc = 5.5x10^-2


So, I think you'd solve the problem like this:

1/(5.7x10^-4)^.5 + 1/(5.5x10^-2)^.5

I've tried many different variations of this, but nothing really seems to be working.

[sjb]

Calculate of the value of the equilibrium constant K for the following reaction:

A + B <=> C

from the following information:

2C <=> D    Kc = 5.7 x 10^-4

D <=> 2A + 2B   Kc = 5.5x10^-2


So, I think you'd solve the problem like this:

1/(5.7x10^-4)^.5 + 1/(5.5x10^-2)^.5

I've tried many different variations of this, but nothing really seems to be working.

You're getting there.

Can you write the equilibrium constant expressions for each of the 3 reactions?

[mcduffels]

1) [C] / [A](B)
2) [D] / [C]^2
3) [A]^2(B)^2 / [D]

I think these formulas combined would make:

 [A]^2(B)^2 / [C]^2

(I had to change the format of the B's so that they didn't bold  my answers.)