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An aqueous mixture of phenol and ammonia has initial concentrations of 0.302 M C6H5OH(aq) and 0.139 M NH3(aq). At equilibrium, the C6H5O–(aq) concentration is 5.00E-2 M. Calculate K for the reaction.

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Answer:

[tex]\large\boxed{\large\boxed{Keq=0.111}}[/tex]

Explanation:

1. Chemical equilibrium equation

    [tex]C_6H_5OH(aq)+NH_{3}(aq)\rightleftharpoons C_6H_5O^-(aq)+NH_4^+(aq)[/tex]

2. ICE (initial, change, equilibrium) table

Molar concentrations:

           [tex]C_6H_5OH(aq)+NH_{3}(aq)\rightleftharpoons C_6H_5O^-(aq)+NH_4^+(aq)[/tex]

I                0.302            0.139                 0                   0

C            - 0.0500         - 0.0500         + 0.0500      + 0.0500

E               0.252            0.0890            0.0500          0.0500

3. Constant equilibrium equation:

          [tex]Keq=\dfrac{[C_6H_5OH(aq)].[NH_{3}(aq)]}{[C_6H_5O^-(aq)].[NH_4^+(aq)]}[/tex]

           [tex]Keq=\dfrac{(0.0500)^2}{(0.252)(0.0890)}[/tex]

            [tex]Keq=0.111[/tex]

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