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

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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 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] =
ΣΣ
Transcribed Image Text: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 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] = ΣΣ
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