For the reaction: A(g) ⇌ B(g) + C(g), if the concentration of A is increased, what will happen to the equilibrium position?
Practice Questions
1 question
Q1
For the reaction: A(g) ⇌ B(g) + C(g), if the concentration of A is increased, what will happen to the equilibrium position?
Shift to the left
Shift to the right
No change
Depends on temperature
According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium to the right.
Questions & Step-by-step Solutions
1 item
Q
Q: For the reaction: A(g) ⇌ B(g) + C(g), if the concentration of A is increased, what will happen to the equilibrium position?
Solution: According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium to the right.
Steps: 6
Step 1: Identify the reaction: A(g) ⇌ B(g) + C(g).
Step 2: Understand that A is a reactant in this reaction.
Step 3: Recognize that increasing the concentration of A means there is more of it available.
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 we increased the concentration of A, the system will try to reduce the amount of A by producing more products (B and C).
Step 6: Therefore, the equilibrium position will shift to the right, favoring the formation of B and C.
