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:
|
Substance
|
Amount/mol
|
|
Ethanoic acid (CH3COOH)
Ethanol (CH3CH2OH)
Ethyl ethanoate (CH3COOCH2CH3)
Water (H2O)
|
0.09
0.21
0.18
0.42
|
The 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 Kuntil equilibrium is reached. How many moles of ethanoic acid are present in this mixture?