g For the reaction Ag2S(s)⇌2Ag+(aq)+S2−(aq)Ag2S(s)⇌2Ag+(aq)+S2−(aq), Keq=2.4×10−4Keq=2.4×10−4, and the equilibrium concentration of sulfide

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g For the reaction Ag2S(s)⇌2Ag+(aq)+S2−(aq)Ag2S(s)⇌2Ag+(aq)+S2−(aq), Keq=2.4×10−4Keq=2.4×10−4, and the equilibrium concentration of sulfide ion is [S2−]=0.0023M[S2−]=0.0023M. What is [Ag+]atequilibrium?

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Thành Công 5 months 2021-08-10T01:45:35+00:00 1 Answers 45 views 0

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  1. thienthanh
    0
    2021-08-10T01:47:19+00:00
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    Answer:

    0.32 M

    Explanation:

    Step 1: Write the balanced reaction at equilibrium

    Ag₂S(s) ⇌ 2 Ag⁺(aq) + S²⁻(aq)

    Step 2: Calculate the concentration of Ag⁺ at equilibrium

    We will use the formula for the concentration equilibrium constant (Keq), which is equal to the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients. It only includes gases and aqueous species.

    Keq = [Ag⁺]² × [S²⁻]

    [Ag⁺] = √{Keq / [S²⁻]}

    [Ag⁺] = √{2.4 × 10⁻⁴ / 0.0023} = 0.32 M

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