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 NH: be? NH:SH(s) = NHs(g) + H:S(g) 1 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) Eguilibrium (M)

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Question 2 of 6
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 NHs be?
NH:SH(s) NH:(g) + H2S(g)
1.
2.
NEXT
へ
Based on the given values, set up ICE table in order to determine the unknown.
NH:SH(s)
NH:(g)
H:S(g)
**************t
Initial (M)
其刻其其其
***
其其
其
Change (M)
Equilibrium (M)
3.
1L
Transcribed Image Text:Question 2 of 6 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 NHs be? NH:SH(s) NH:(g) + H2S(g) 1. 2. NEXT へ Based on the given values, set up ICE table in order to determine the unknown. NH:SH(s) NH:(g) H:S(g) **************t Initial (M) 其刻其其其 *** 其其 其 Change (M) Equilibrium (M) 3. 1L
Expert Solution
Step 1-4

The value of Kc for the reaction of NH4SH is given and the reaction is

NH4SHNH3+H2S

The ICE tables give us information about the concentration of the compounds. In the ICE, I stand for the initial concentration, C is change in concentration and E is equilibrium concentration.

 

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