A solution containing a mixture of ethanoic acid ethanol ethyl ethanoate and wat

A
solution containing a mixture of ethanoic acid ethanol ethyl ethanoate and
water was allowed to come to equilibrium in a stoppered bottle at 373 K when
the amount of each of the four substances was measured. These were found to be
as in the table below:SubstanceAmount/molEthanoic
acid (CH3COOH)Ethanol
(CH3CH2OH) Ethyl
ethanoate (CH3COOCH2CH3) Water
(H2O) 0.09 0.21 0.18 0.42The
equation for the reaction is:CH3COOH(aq)
+ CH3CH2OH(aq)
<=> CH3COOCH2CH3(aq) + H2O(l) a) Write the equilibrium law for the
reaction.b)
Calculate the equilibrium constant for the reaction at this temperature.c)
Calculate the equilibrium constant for the reaction:CH3COOCH2CH3(aq)
+ H2O(l) <==> CH3COOH(aq) + CH3CH2OH(aq)d)
0.20 mol of ethyl ethanoate is mixed with 0.60 mol of water in a stoppered
bottle. The mixture is kept at 373 K
until equilibrium is reached. How many moles of ethanoic acid are present in
this mixture?