Give typed full explanation The equilibrium constant, K, for the following reaction is 1.80x10-4 at 298 K.NH4HS(s)NH3(g) + H₂S(g)An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.343 molNH4HS, 1.34x102 M NH3 and 1.34x10-2 M H₂S. If the concentration of H₂S(g) is suddenlyincreased to 1.89x10-2 M, what will be the concentrations of the two gases once equilibrium hasbeen reestablished?[NH3] =[H₂S]BMM

Answer:For any reaction, value of equilibrium constant is equal to the ratio of molar concentration…

The equilibrium constant, K, for the following reaction is 1.80x104 at 298 K. NH4HS(s) NH3(g) + H₂S(8) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.343 mol NH4HS, 1.34×102 M NH3 and 1.34x102 M H₂S. If the concentration of H₂S(g) is suddenly increased to 1.89x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] 33

The equilibrium constant, K, for the following reaction is 1.80x104 at 298 K. NH4HS(s) NH3(g) + H₂S(8) An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.343 mol NH4HS, 1.34×102 M NH3 and 1.34x102 M H₂S. If the concentration of H₂S(g) is suddenly increased to 1.89x10-2 M, what will be the concentrations of the two gases once equilibrium has been reestablished? [NH3] = [H₂S] 33

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

Give typed full explanation

The equilibrium constant, K, for the following reaction is 1.80x10-4 at 298 K.
NH4HS(s)
NH3(g) + H₂S(g)
An equilibrium mixture of the solid and the two gases in a 1.00 L flask at 298 K contains 0.343 mol
NH4HS, 1.34x102 M NH3 and 1.34x10-2 M H₂S. If the concentration of H₂S(g) is suddenly
increased to 1.89x10-2 M, what will be the concentrations of the two gases once equilibrium has
been reestablished?
[NH3] =
[H₂S]
B
M
M

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Step 1: Defining equilibrium constant

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Step 2: Molar concentration of solid ammonium hydrogen sulfide

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Step 3: Formation for ICE table

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Step 4: Calculation for unknown y

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Step 5: Calculation for the equilibrium concentration of both the gases

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