The decomposition of NOCl has an equilibrium constant of K=1.6x10 -5 at 35 °C. W
ID: 103689 • Letter: T
Question
The decomposition of NOCl
has an equilibrium constant of K=1.6x10-5 at 35 °C. When sodium is added to the reaction vessel it scavenges the chlorine gas in an exothermic reaction. What will the impact of adding sodium be on the equilibrium of the decomposition of NOCl?
(A) Shift towards products.
(B) Shift towards reactants.
(C) There will be no change because the sodium isn’t participating in the chemical reaction.
(D) This question cannot be answered with the information provided.
The decomposition of NOCl
2NOCl (g) Cl2 (g) + 2NO (g)
has an equilibrium constant of K=1.6x10-5 at 35 °C. When sodium is added to the reaction vessel it scavenges the chlorine gas in an exothermic reaction. What will the impact of adding sodium be on the equilibrium of the decomposition of NOCl?
(A) Shift towards products.
(B) Shift towards reactants.
(C) There will be no change because the sodium isn’t participating in the chemical reaction.
(D) This question cannot be answered with the information provided.
Explanation / Answer
1)
when sodium is added, it removes the Cl2
So, we are removing a product
According to Le Chatelier's Principle,
Removing product will shift reaction towards product side
Equilibrium moves to product side
Answer: A
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