Asked by Tyler o
Use the reaction to answer the question.
N2(g) + 3H2(g) ⇄ 2NH3(g) + energy
When this reaction has reached equilibrium, how will it respond when the temperature of the system increases?
(1 point)
Responses
The concentration of H2 will decrease.
The concentration of H 2 will decrease.
The equilibrium will shift to the right.
The equilibrium will shift to the right.
The equilibrium will shift to the left.
The equilibrium will shift to the left.
The concentration of N2 will decrease
N2(g) + 3H2(g) ⇄ 2NH3(g) + energy
When this reaction has reached equilibrium, how will it respond when the temperature of the system increases?
(1 point)
Responses
The concentration of H2 will decrease.
The concentration of H 2 will decrease.
The equilibrium will shift to the right.
The equilibrium will shift to the right.
The equilibrium will shift to the left.
The equilibrium will shift to the left.
The concentration of N2 will decrease
Answers
Answered by
GPT-4o mini
When the temperature of the system increases for the given reaction:
\[ \text{N}_2(g) + 3\text{H}_2(g) ⇄ 2\text{NH}_3(g) + \text{energy} \]
This reaction is exothermic, meaning it releases energy as a product. According to Le Chatelier's Principle, increasing the temperature of an exothermic reaction will shift the equilibrium to the left in order to absorb the excess heat.
Therefore, the correct response is:
**The equilibrium will shift to the left.**
\[ \text{N}_2(g) + 3\text{H}_2(g) ⇄ 2\text{NH}_3(g) + \text{energy} \]
This reaction is exothermic, meaning it releases energy as a product. According to Le Chatelier's Principle, increasing the temperature of an exothermic reaction will shift the equilibrium to the left in order to absorb the excess heat.
Therefore, the correct response is:
**The equilibrium will shift to the left.**
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