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If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, wha

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Question: If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, what will be the effect on the equilibrium position?

Options:

  1. Shift to the left
  2. Shift to the right
  3. No change
  4. Increase the rate of reaction

Correct Answer: Shift to the left

Solution: 

According to Le Chatelier\'s Principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants.

If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, wha

Practice Questions

Q1
If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, what will be the effect on the equilibrium position?
  1. Shift to the left
  2. Shift to the right
  3. No change
  4. Increase the rate of reaction

Questions & Step-by-Step Solutions

If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, what will be the effect on the equilibrium position?
  • Step 1: Understand that an exothermic reaction releases heat.
  • Step 2: Identify the reaction: A + B ⇌ C + heat.
  • Step 3: Recognize that heat can be treated like a product in this reaction.
  • Step 4: Apply Le Chatelier's Principle, which states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
  • Step 5: Note that increasing the temperature adds more heat to the system.
  • Step 6: Since heat is a product, adding more heat will shift the equilibrium to the left, favoring the reactants (A and B).
  • Step 7: Conclude that the effect of increasing the temperature is to shift the equilibrium position to the left.
  • 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 Reactions – Reactions that release heat, meaning that heat can be considered a product in the equilibrium expression.
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