In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the temperature is increased, what will be the effect on the equilibrium if the reaction is exothermic? (2020)
Practice Questions
1 question
Q1
In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the temperature is increased, what will be the effect on the equilibrium if the reaction is exothermic? (2020)
The equilibrium shifts to the left
The equilibrium shifts to the right
No effect on the equilibrium
The reaction rate increases
For an exothermic reaction, increasing the temperature shifts the equilibrium to the left (towards the reactants) to absorb the added heat, according to Le Chatelier's principle.
Questions & Step-by-step Solutions
1 item
Q
Q: In the reaction A(g) + B(g) ⇌ C(g) + D(g), if the temperature is increased, what will be the effect on the equilibrium if the reaction is exothermic? (2020)
Solution: For an exothermic reaction, increasing the temperature shifts the equilibrium to the left (towards the reactants) to absorb the added heat, according to Le Chatelier's principle.
Steps: 6
Step 1: Understand that the reaction A(g) + B(g) ⇌ C(g) + D(g) can go in both directions: from reactants (A and B) to products (C and D) and back.
Step 2: Identify that this reaction is exothermic, meaning it releases heat when it goes from reactants to products.
Step 3: Recognize 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 releases heat, increasing the temperature will cause the equilibrium to shift in the direction that absorbs heat, which is towards the reactants (A and B).
Step 6: Conclude that the effect of increasing the temperature on this exothermic reaction is to shift the equilibrium to the left.
