Sorry Steve for asking dumb questions. My brain is somewhere else these couple of days.
At a particular temperature, Kc = 54.3 for the reaction:
H2 + I2 <-> 2HI
If the initial concentrations of both H2 and I2 are 0.5M, what are the equilibrium concentrations of each gas involved?
My lecturer said to use the ICE table, so I figured
H2 I2 2HI
Initial 0.5 0.5 0.0
Change -x -x +2x
Equi. (0.5-x) (0.5-x) 2x
Kc = [HI]^2 / [H2][I2]
54.3 = (2x)^2 / (0.5-x)(0.5-x)
Is it right so far? How do I go on from here?
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