A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentratio

Question

A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species.

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Khánh Gia 6 months 2021-07-12T10:40:05+00:00 1 Answers 18 views 0

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    2021-07-12T10:41:06+00:00

    Answer:

    Equlibrium concentration for each species ae as follows:

    [CO] = 0.043 mol/L

    [Br₂] = 0.043 mol/L

    [COBr₂] = 0.01 mol/L

    Explanation:

    Let take a look at the chemical equation taking place at equilibrium

    COBr2(g) ⇄ CO(g) + Br2(g)

    The concentration of COBr2 i.e.

    [COBr2] = no of moles/volume

    = 0.50 mol/9.50 L

    [COBr2] = 0.0530 mol/L

    At standard conditions

    Kc for COBr2 = 0.190

    Now, the ICE table for the above reaction can be computed as follows:

                           COBr2(g)              ⇄       CO(g)         +           Br2(g)

    Initial               0.053                                   0                           0

    Change             -x                                       +x                          +x

    Equilibrium     (0.053 – x)                              x                           x

    \mathsf{K_c = \dfrac{[CO][Br_2]}{[COBr_2]}}

    K_c = \dfrac{(x) (x)}{(0,053 -x)}

    0.190= \dfrac{x^2}{(0.053 -x)}

    x² = 0.190(0.053 – x)

    x² = 0.01007 – 0.190x

    x² + 0.190x – 0.01007 = 0

    Using quadratic formula:

    x ≅ 0.043 mol/L

    SInce: x = [CO][Br₂] = 0.043 mol/L

    [COBr₂] = 0.053 – x

    [COBr₂] = 0.053 – 0.043 mol/L

    [COBr₂] = 0.01 mol/L

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