What is the effect of increasing the concentration of a product in a reaction at equilibrium?
Practice Questions
1 question
Q1
What is the effect of increasing the concentration of a product in a reaction at equilibrium?
Shifts equilibrium to the right
Shifts equilibrium to the left
No change occurs
Increases reaction rate
Increasing the concentration of a product will shift the equilibrium to the left, favoring the formation of reactants, according to Le Chatelier's Principle.
Questions & Step-by-step Solutions
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Q
Q: What is the effect of increasing the concentration of a product in a reaction at equilibrium?
Solution: Increasing the concentration of a product will shift the equilibrium to the left, favoring the formation of reactants, according to Le Chatelier's Principle.
Steps: 6
Step 1: Understand that a chemical reaction can reach a state called equilibrium, where the rate of the forward reaction equals the rate of the reverse reaction.
Step 2: Recognize that at equilibrium, the concentrations of reactants and products remain constant.
Step 3: 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 4: Identify that increasing the concentration of a product means there is more of that product present in the reaction mixture.
Step 5: Apply Le Chatelier's Principle: when the concentration of a product increases, the system will try to reduce that concentration by favoring the reverse reaction (the formation of reactants).
Step 6: Conclude that increasing the concentration of a product shifts the equilibrium to the left, leading to more reactants being formed.
