For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?
Practice Questions
1 question
Q1
For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?
Increase
Decrease
Remain the same
Cannot be determined
According to Le Chatelier's principle, increasing the concentration of a product will shift the equilibrium to the left, decreasing the concentration of A.
Questions & Step-by-step Solutions
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Q
Q: For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?
Solution: According to Le Chatelier's principle, increasing the concentration of a product will shift the equilibrium to the left, decreasing the concentration of A.
Steps: 7
Step 1: Understand that A and B are in a reversible reaction, meaning they can change back and forth.
Step 2: Recognize that A is a reactant and B is a product in the reaction A(g) ⇌ B(g).
Step 3: Know that equilibrium is the point where the concentrations of A and B remain constant.
Step 4: Learn about 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: When the concentration of B (the product) is increased, the system will try to reduce this increase.
Step 6: To counteract the increase in B, the equilibrium will shift to the left, which means it will favor the formation of A.
Step 7: As a result, the concentration of A will increase while the concentration of B will decrease until a new equilibrium is reached.
