For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibrium shift if the temperature is decreased?
Practice Questions
1 question
Q1
For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibrium shift if the temperature is decreased?
Shift to the right
Shift to the left
No change
Increase in pressure
Decreasing the temperature for an endothermic reaction will shift the equilibrium to the left, favoring the formation of HCl.
Questions & Step-by-step Solutions
1 item
Q
Q: For the equilibrium reaction 4HCl(g) ⇌ 2H2(g) + 2Cl2(g), how will the equilibrium shift if the temperature is decreased?
Solution: Decreasing the temperature for an endothermic reaction will shift the equilibrium to the left, favoring the formation of HCl.
Steps: 6
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.
