HELP PLEASE! Chemistry - Equilibrium problem!

Posted on 2013-11-28 16:05:00 in Chemistry by JACKY

This is a question on my test review and I have absolutely no idea how to solve it. Please help!!



2.50 mole of ethanoic acid, 3.50 moles of ethanol and 1.00 mole of water were mixed in a conical flask and heated up to 30?. When equilibrium was reached, 0.70 mole of ethanoic acid was found in the reaction mixture.

CH3COOH (l) + C2H5OH (l) ? CH3COOC2H5 (l) + H2O (l)

(a) How many mole of ethyl ethanoate is formed?

(b) Calculate the equilibrium constant Kc(1) for the esterification reaction.

(c) In another conical flask, predict the amount of ethyl ethanoate formed when 2.00 mole of ethanoic acid, 5.00 moles of ethanol and 4.00 moles of water are allowed to come to equilibrium at 30 ?.

(d) If another alcohol CH3OH was added to the equilibrium mixture in (b), there will be another equilibrium reaction as following:

CH3COOH (l) + CH3OH (l) ? CH3COOCH3 (l) + H2O(l)

(i) If the equilibrium constant for this equilibrium is Kc(2). Express Kc(2) in term of Kc(1).

(ii) If there is 3.00 mole of methyl ethanoate, 2.50 mole of ethyl ethanoate, 0.40 mole of both alcohol were found, calculate the equilibrium constant Kc(2).

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