For the exothermic reaction A + B ⇌ C + D, what effect does increasing the tempe

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Question: For the exothermic reaction A + B ⇌ C + D, what effect does increasing the temperature have on the equilibrium? (2020)

Options:

Correct Answer: Shifts to the left

Exam Year: 2020

Solution:

For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.

For the exothermic reaction A + B ⇌ C + D, what effect does increasing the temperature have on the equilibrium? (2020)

For the exothermic reaction A + B ⇌ C + D, what effect does increasing the temperature have on the equilibrium? (2020)

Step 1: Understand that an exothermic reaction releases heat.
Step 2: Recognize that in the reaction A + B ⇌ C + D, the products (C and D) are formed from the reactants (A and B).
Step 3: Know that increasing the temperature adds heat to the system.
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: Since the reaction is exothermic, adding heat will shift the equilibrium to the left, meaning it will favor the reactants (A and B).
Step 6: Conclude that increasing the temperature causes the equilibrium to shift towards the reactants.

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 – In exothermic reactions, heat is released, and increasing temperature can shift the equilibrium towards the reactants.