Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 10-4 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) 3 NEXT Based on the given values, set up ICE table in order to determine the unknown. NH:SH(s) NH:(g) H:S(g) Initial (M) Change (M) Equilibrium (M) 5 RESET 1.2 x 10 +x +2x -2x 1.2 x 104+x 1.2 x 104-x 1.2 x 10+ 2x 1.2 x 10-2x

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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to
1.2 x 104 at a certain temperature. If a solid sample of NH:SH decomposes, what will the equilibrium
concentration of NH: be?
NH:SH(s) = NH:(g) + H2S(g)
1
2
3
NEXT
>
Based on the given values, set up ICE table in order to determine the unknown.
NH:SH(s)
NH:(g)
H:S(g)
Initial (M)
Change (M)
Equilibrium (M)
2 RESET
1.2 x 104
+x
-x
+2x
-2x
1.2 x 104+x
1.2 x 104-x
1.2 x 10*+ 2x
1.2 x 10-2x
Transcribed Image Text:Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH:SH decomposes, what will the equilibrium concentration of NH: be? NH:SH(s) = NH:(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH:SH(s) NH:(g) H:S(g) Initial (M) Change (M) Equilibrium (M) 2 RESET 1.2 x 104 +x -x +2x -2x 1.2 x 104+x 1.2 x 104-x 1.2 x 10*+ 2x 1.2 x 10-2x
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