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Question 14.7: Predicting the Direction of a Reaction by Comparing Q and K ...

Predicting the Direction of a Reaction by Comparing Q and K
Consider the reaction and its equilibrium constant:
I_{2}(g) + Cl_{2}(g) \xrightleftharpoons[]{}2 ICl(g)                    K_{p} = 81.9
A reaction mixture contains P_{I_{2}} = 0.114 atm, P_{Cl_{2}} = 0.102 atm, and P_{ICl} = 0.355 atm. Is the reaction mixture at equilibrium?
If not, in which direction will the reaction proceed?

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To determine the progress of the reaction relative to the equilibriumstate, calculate Q. Q_{p} = \frac{P^{2}_{ICl}}{P_{I_{2}}P_{Cl_{2}}}
= \frac{0.355^{2}}{(0.114)(0.102)}
= 10.8
Compare Q to K. Q_{p} = 10.8; K_{p} = 81.9
Since Q_{p} < K_{p}, the reaction is not at equilibrium and will proceed to the right.

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