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An aqueous solution of ethyl acetate at room temperature has an itial concentration of 0.15 M....

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Chemistry

An aqueous solution of ethyl acetate at room temperature has anitial concentration of 0.15 M. Calculate the equilibriumconcentrations of ethyl acetate (CH3COOC2H5), ethanol (C2H5OH) andacetic acid if the equilibrium constant at this temperature is Kc=3.00. Part B. Repeat this calculation for initial ehtyl acetateconcentrations of 0.25 M and 0.35 M. Are your answers in agreementwith Le Chatelier's Principle?

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Pertinent equation for hydrolysis of Ethyl acetate isCH3COOC2H5 H2O CH3COOH HOC2H5Ethyl acetate Acetic acid EthanolExpression for equilibrium constant Kc is given asKc CH3COOHHOC2H5 CH3COOC2H5 1H2Oalmost unchanged at equilibrium so not appeared in expressionLet at equilibrium x ML of the ethyl acetate get hydrolyzedhence we write the concentrations at equilibrium asCH3COOH x MLHOC2H5 x MLCH3COOC2H5 015 x MLUsing    See Answer
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