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Consider the reaction: AC(g)+2B(g) ↔ AB2 (g) + C(g)  ΔH=+56.9kJ The system is sitting at equilibrium. Describe...

Consider the reaction:

AC(g)+2B(g) ↔ AB2 (g) + C(g)  ΔH=+56.9kJ

The system is sitting at equilibrium. Describe what will happen when each of the following stresses are applied.

A)The K for the reaction will lower. B)The K for the reaction will get larger. C)The K for the reaction will not change. 1)B is selectively removed from the reaction vessel.
A)The K for the reaction will lower. B)The K for the reaction will get larger. C)The K for the reaction will not change. 2)Additional C is added to the reaction vessel.
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Answer #1

Equilibrium constant is the product of the concentration of products divided by the product of the concentration of reactant with each term raised to their coefficients as power. According to Lechatelier's principle any change in factor at equilibrium will shift the equilibrium in that direction where it's effect get reduced.

1) When B is removed then equilibrium shift in backward direction and hence K of the reaction lowered. Answer is A)

2) On adding C, equilibrium shift in backward direction and thus K of the reaction will lower. Answer is A).

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