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The ester, ethyl acetate is formed by the reaction between ethanol and acetic acid and equilibrium is represented as :

CH3COOH(I) +C2H5OH(I) ⇌  CH3COOC2H5(aq) + H2O(I)

(a) Write the concentration ratio (reaction quotient), Qc, for this reaction. Note that water is not in excess and is not a solvent in this reaction. 

(b) At 293 K, if one starts with 1.00 mole of acetic acid and 0.180 of ethanol, there is 0.171 mole of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant. 

(c) Starting with 0.500 mole of ethanol and 1.000 mole of acetic acid and maintaining it at 293 K, 0.214 mole of ethyl acetate is found after some time. Has equilibrium been reached?

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∴ Equilibrium has not been reached.

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