Aa 22 The equilibrium constant, K, for the following reaction is 1.31×10-² at 307 K.NH4HS(s)NH3(g) + H₂S(g)An equilibrium mixture in a 13.0 L container at 307 K contains 0.370 mol NH4HS(s), 0.143 M NH3 and 9.16x10-² M H₂S. What will bethe concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constanttemperature to a volume of 5.34 L?[NH3] =[H₂S] =ΣΣ

The balanced equilibrium reaction is: NH4HS(s) ⇌ NH3(g) + H2S(g) ; K = 1.31*10-2 Equilibrium…

The equilibrium constant, K, for the following reaction is 1.31×10¹² at 307 K. NH4HS(s) NH3(9) + H₂S(9) An equilibrium mixture in a 13.0 L container at 307 K contains 0.370 mol NH4HS(s), 0.143 M NH3 and 9.16x10-2 M H₂S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.34 L? [NH3] = [H₂S] = M M

The equilibrium constant, K, for the following reaction is 1.31×10¹² at 307 K. NH4HS(s) NH3(9) + H₂S(9) An equilibrium mixture in a 13.0 L container at 307 K contains 0.370 mol NH4HS(s), 0.143 M NH3 and 9.16x10-2 M H₂S. What will be the concentrations of the two gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 5.34 L? [NH3] = [H₂S] = M M

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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