For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibriu

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Question: For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibrium shift if the temperature is decreased?

Options:

Correct Answer: Shift to the left

Solution:

Decreasing the temperature for an endothermic reaction will shift the equilibrium to the left, favoring the formation of HCl.

For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibrium shift if the temperature is decreased?

For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibrium shift if the temperature is decreased?

Step 1: Identify the reaction type. The given reaction is 4HCl(g) ⇌ 2H2(g) + 2Cl2(g).
Step 2: Determine if the reaction is endothermic or exothermic. For this reaction, it is endothermic, meaning it absorbs heat.
Step 3: Understand what happens when temperature decreases. Lowering the temperature means there is less heat available.
Step 4: Apply Le Chatelier's Principle. This principle states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 5: Since the reaction is endothermic, decreasing the temperature will shift the equilibrium to the left to produce more heat.
Step 6: Conclude that the equilibrium will favor the formation of HCl when the temperature is decreased.

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.
Endothermic vs Exothermic Reactions – Understanding the difference between endothermic and exothermic reactions is crucial for predicting how temperature changes affect equilibrium.