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

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

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.