Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be? Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to1.2 x 10- at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibriumconcentration of NH3 be?NH.SH(s) = NH:(g) + H:S(g)NEXT12Based on the given values, set up ICE table in order to determine the unknown.NH (g)H:S(g)NH.SH(s)1.2 x 10Initial (M)+2xChange (M)1.2 * 104=*1.2 * 104-*1.2 * 10+ 2xEquilibrium (M)5 RESET+2x-2x1.2 * 10 +*1.2 x 10中N1.2 10-*1.2 x 10 +2x1.2 10 -2x

Answered: Consider the equilibrium system…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 1ALQ: Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed...

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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2×10-4 at a certain temperature. If a solid sample of NH4SH decomposes, what is the equilibrium concentration of NH3 be?

Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to
1.2 x 10- at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium
concentration of NH3 be?
NH.SH(s) = NH:(g) + H:S(g)
NEXT
1
2
Based on the given values, set up ICE table in order to determine the unknown.
NH (g)
H:S(g)
NH.SH(s)
1.2 x 10
Initial (M)
+2x
Change (M)
1.2 * 104=*
1.2 * 104-*
1.2 * 10+ 2x
Equilibrium (M)
5 RESET
+2x
-2x
1.2 * 10 +*
1.2 x 10
中N
1.2 10-*
1.2 x 10 +2x
1.2 10 -2x

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