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25 February, 12:26

Consider the following reaction:

NH4HS (s) ⇌NH3 (g) + H2S (g)

An equilibrium mixture of this reaction at a certain temperature was found to have [NH3] = 0.276 M and [H2S] = 0.370 M. What is the value of the equilibrium constant (Kc) at this temperature?

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  1. 25 February, 14:55
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    Kc = 0.102

    Explanation:

    NH₄HS (s) ⇌ NH₃ (g) + H₂S (g)

    The equilibrium constant for the above reaction, can be written as the product of the concentration of product raised to the power of stoichiometric coefficients in a balanced equation of dissociation divided by the product of the concentration of reactant raised to the power of stoichiometric coefficients in the balanced equation of dissociation.

    Hence,

    Kc = [ NH₃ (g) ][ H₂S (g) ] / [ NH₄HS (s) ]

    Since, the state of NH₄HS is solid so, it's concentration will remain constant, hence, the equation can be rearranged as -

    Kc = [ NH₃ (g) ][ H₂S (g) ]

    From the question,

    [ NH₃ (g) ] = 0.276 M

    [ H2S (g) ] = 0.370 M

    Now, putting it in the above equation,

    Kc = [ NH₃ (g) ][ H₂S (g) ]

    Kc = 0.276 * 0.370

    Kc = 0.102
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