The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. NH4 HS(s) NH3 (9) + H₂S(9) If an equilibrium mixture of the three compounds in a 4.73 L container at 298 K contains 2.68 mol of NH4HS(s) and 0.461 mol of NH3, the number of moles of H₂S present is mol.
The equilibrium constant, Ke, for the following reaction is 1.80 x 104 at 298 K. NH4 HS(s) NH3 (9) + H₂S(9) If an equilibrium mixture of the three compounds in a 4.73 L container at 298 K contains 2.68 mol of NH4HS(s) and 0.461 mol of NH3, the number of moles of H₂S present is mol.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K.
\[
\text{NH}_4\text{HS} (\text{s}) \rightleftharpoons \text{NH}_3 (\text{g}) + \text{H}_2\text{S} (\text{g})
\]
If an equilibrium mixture of the three compounds in a 4.73 L container at 298 K contains 2.68 mol of \(\text{NH}_4\text{HS} (\text{s})\) and 0.461 mol of \(\text{NH}_3\), the number of moles of \(\text{H}_2\text{S}\) present is \(\boxed{\phantom{00}}\) mol.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb8d8ce1c-d1ae-4fbf-bbe3-121c6915374e%2F69788557-f6a4-420a-8cd1-4458be2474bf%2Fqossp0h_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K.
\[
\text{NH}_4\text{HS} (\text{s}) \rightleftharpoons \text{NH}_3 (\text{g}) + \text{H}_2\text{S} (\text{g})
\]
If an equilibrium mixture of the three compounds in a 4.73 L container at 298 K contains 2.68 mol of \(\text{NH}_4\text{HS} (\text{s})\) and 0.461 mol of \(\text{NH}_3\), the number of moles of \(\text{H}_2\text{S}\) present is \(\boxed{\phantom{00}}\) mol.
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Kc is the ratio of product of concentration of products raised to their stoichiometric coefficient to the product of concentration of reactants raised to their stoichiometric coefficients.
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