For the equilibrium 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the concentration of A?
Practice Questions
1 question
Q1
For the equilibrium 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the concentration of A?
Increase
Decrease
Remain the same
Cannot be determined
According to Le Chatelier's principle, increasing the concentration of B will shift the equilibrium to the left, resulting in a decrease in the concentration of A.
Questions & Step-by-step Solutions
1 item
Q
Q: For the equilibrium 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the concentration of A?
Solution: According to Le Chatelier's principle, increasing the concentration of B will shift the equilibrium to the left, resulting in a decrease in the concentration of A.
Steps: 5
Step 1: Understand the equilibrium reaction: 2A(g) ⇌ B(g) + C(g). This means that A can turn into B and C, and B and C can turn back into A.
Step 2: Identify what happens when the concentration of B is increased. This means there is more B available in the reaction.
Step 3: 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 4: Since the concentration of B is increased, the system will try to reduce the amount of B by shifting the equilibrium to the left.
Step 5: Shifting the equilibrium to the left means that more B will turn back into A, which will decrease the concentration of A.
