Question

Please Explain! Thank you so much.

An aqueous solution of ethyl acetate at room temperature has an itial concentration of 0.15 M. Calculate the equilibrium concentrations of ethyl acetate (CH3COOC2H5), ethanol (C2H5OH) and acetic acid if the equilibrium constant at this temperature is Kc= 3.00.

Part B. Repeat this calculation for initial ehtyl acetate concentrations of 0.25 M and 0.35 M. Are your answers in agreement with Le Chatelier's Principle?

Answer 1

a)                      CH3COOC2H5 (aq)    <-------------> C2H5OH + CH3COOH         Kc = 3.00

    Initial              0.15 M                                              0                     0

At equilibrium      0.15-x                                              x                     x

         Kc = x.x / 0.15-x

       3 = x²/ 0.15-x

     0.45 - 3x = x²

    x² + 3x -0.45 = 0

On solving,

x = 0.1432

Therefore, equilibrium concentrations are

[ CH3COOC2H5 (aq)] = 0.15- x= 0.15 -0.143 = 0.0068 M

[C2H5OH] = x = 0.1432 M

[CH3COOH] = x = 0.1432 M

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