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MCS,PHD
Argosy University/ Phoniex University/
Nov-2005 - Oct-2011
Professor
Phoniex University
Oct-2001 - Nov-2016
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:
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Substance |
Amount/mol |
Ethanoic acid (CH3COOH) Ethanol (CH3CH2OH) Ethyl ethanoate (CH3COOCH2CH3) Water (H2O) |
0.09 0.21 0.18 0.42 |
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The equation for the reaction is:
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CH3COOH(aq) + CH3CH2OH(aq) <=> CH3COOCH2CH3(aq) + H2O(l)
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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:
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CH3COOCH2CH3(aq) + H2O(l) <==> CH3COOH(aq) + CH3CH2OH(aq)
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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?
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