The equilibrium constant, Kc, for the following reaction is 1.80 × 10-4 at 298 K. NH4HS(8) ⇒ NH3(g) + H₂S(9) Calculate the equilibrium concentration of H₂S when 0.216 moles of NH₂HS(s) are introduced into a 1.00 L vessel at 298 K. M [H₂S] = =
The equilibrium constant, Kc, for the following reaction is 1.80 × 10-4 at 298 K. NH4HS(8) ⇒ NH3(g) + H₂S(9) Calculate the equilibrium concentration of H₂S when 0.216 moles of NH₂HS(s) are introduced into a 1.00 L vessel at 298 K. M [H₂S] = =
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.3: Determining An Equilibrium Constant
Problem 15.3CYU: A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent...
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![The equilibrium constant,
Ke, for the following reaction is
1.80 x 10-4 at 298 K.
NH4HS (8) NH3(g) + H₂S(g)
Calculate the equilibrium concentration of
H₂S when 0.216 moles of
NH₂HS(s) are introduced into a 1.00 L vessel at 298 K.
[H₂S]
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16a37137-8b78-43ba-b725-b608920c77a8%2F0352a16d-f9cd-47be-bb87-7d15d5a763f7%2Fwtxqf3b_processed.png&w=3840&q=75)
Transcribed Image Text:The equilibrium constant,
Ke, for the following reaction is
1.80 x 10-4 at 298 K.
NH4HS (8) NH3(g) + H₂S(g)
Calculate the equilibrium concentration of
H₂S when 0.216 moles of
NH₂HS(s) are introduced into a 1.00 L vessel at 298 K.
[H₂S]
M
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