Consider the following reactions at equilibrium. NH4SH (s) <--> NH3 (g) + H2S (g
ID: 519924 • Letter: C
Question
Consider the following reactions at equilibrium.
NH4SH (s) <--> NH3 (g) + H2S (g)
Which of the following statement is INCORRECT?
A) Addition of H2S (g) results in the formation of more NH4SH (s).
B) Addition of more NH3 (g) results in a decrease in the amount of H2S (g).
C) Addition of more NH4SH (s) results in an increase in the amount of NH3 (g).
D)Decreasing the volume of the reaction container results in the formation of more NH4SH (s).
Could you please explain specifically why C) is the answer to this question (chemically incorrect) and options A, B, D are chemically correct. I thought that since NH4SH is in solid its state, it doesn't affect equilibrium at all.
Explanation / Answer
Yes . you are correct . NH4HS is a solid . solids and pure liquids have no effect on equilibrium position .
so statement C) is incorrect.
According to Lechatlier's priciple :
on addition of any one of the reactant the equilibrium shifts to product sides
on addition of any one of the product the equilibrium shifts to reactants sides.
if volume decreases the equilibrium will shift towards where moles decreases side.
based on these statements only C is wrong
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