For the reaction 3H2(g) + N2(g) ⇌ 2NH3(g), if the temperature is decreased, what

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Question: For the reaction 3H2(g) + N2(g) ⇌ 2NH3(g), if the temperature is decreased, what will be the effect on the equilibrium position?

Options:

Correct Answer: Shift to the right

Solution:

If the reaction is exothermic, decreasing the temperature will shift the equilibrium to the right, favoring NH3 production.

For the reaction 3H2(g) + N2(g) ⇌ 2NH3(g), if the temperature is decreased, what will be the effect on the equilibrium position?

For the reaction 3H2(g) + N2(g) ⇌ 2NH3(g), if the temperature is decreased, what will be the effect on the equilibrium position?

Step 1: Identify the reaction: 3H2(g) + N2(g) ⇌ 2NH3(g).
Step 2: Determine if the reaction is exothermic or endothermic. (Exothermic means it releases heat, endothermic means it absorbs heat.)
Step 3: If the reaction is exothermic, decreasing the temperature means there is less heat available.
Step 4: According to Le Chatelier's principle, the system will try to counteract the change (decrease in temperature) by shifting the equilibrium position.
Step 5: Since the reaction produces heat, shifting to the right (towards NH3) will help produce more heat.
Step 6: Therefore, if the temperature is decreased, the equilibrium will shift to the right, favoring the production of NH3.

Le Chatelier's Principle – This principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
Exothermic vs Endothermic Reactions – Understanding whether a reaction releases or absorbs heat is crucial for predicting the effect of temperature changes on equilibrium.