For the exothermic reaction: N2(g) + 3H2(g) ⇌ 2NH3(g), what will happen if the temperature is increased? (2023)
Practice Questions
1 question
Q1
For the exothermic reaction: N2(g) + 3H2(g) ⇌ 2NH3(g), what will happen if the temperature is increased? (2023)
The equilibrium will shift to the right
The equilibrium will shift to the left
No change in equilibrium
The reaction will stop
According to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants.
Questions & Step-by-step Solutions
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Q
Q: For the exothermic reaction: N2(g) + 3H2(g) ⇌ 2NH3(g), what will happen if the temperature is increased? (2023)
Solution: According to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants.
Steps: 6
Step 1: Understand that the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is exothermic, meaning it releases heat.
Step 2: Recall Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 3: Identify the disturbance in this case, which is an increase in temperature.
Step 4: Recognize that increasing the temperature adds heat to the system.
Step 5: Since the reaction is exothermic, the system will try to reduce the added heat by shifting the equilibrium to the left, towards the reactants (N2 and H2).
Step 6: Conclude that increasing the temperature will favor the formation of reactants over products.
