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The following reversible reaction is at equilibrium. If the concentration of HCl is increased, how would the system react?

[tex]\[ NH_4Cl \rightleftharpoons NH_3 + HCl \][/tex]

A. Nothing would change.
B. The reaction would move to the right, producing more [tex]\( NH_3 \)[/tex].
C. The reaction would move to the left, producing more [tex]\( NH_4Cl \)[/tex].
D. There would only be HCl remaining.

Sagot :

GinnyAnsweridn
To determine how the system will react when the concentration of HCl is increased, we need to consider Le Chatelier's principle. This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.

The reaction given is:
[tex]\[ NH_4Cl \square NH_3 + HCl \][/tex]

Here we have a system at equilibrium.

Step-by-step analysis:

1. Identify the Change: The concentration of HCl is increased. This means we are adding more HCl to the reaction.

2. Le Chatelier's Principle Application: According to Le Chatelier's principle, the system will try to counteract the increase in concentration of HCl. To counteract the addition of HCl, the equilibrium will shift in such a way to decrease the amount of HCl.

3. Shift in Equilibrium: To decrease the amount of HCl, the reaction will shift to the left, where HCl is consumed. In other words, the reaction will favor the formation of more [tex]\( NH_4Cl \)[/tex] and use up [tex]\( NH_3 \)[/tex] and [tex]\( HCl \)[/tex].

So, when the concentration of HCl is increased, the reaction will move to the left to produce more [tex]\( NH_4Cl \)[/tex].

Therefore, the correct answer is:

C. The reaction would move to the left, producing more [tex]\( NH_4Cl \)[/tex].
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