In a reversible reaction, if the concentration of products is increased, what wi
Practice Questions
Q1
In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium? (2021)
Shift to the right
Shift to the left
No change
Increase in temperature
Questions & Step-by-Step Solutions
In a reversible reaction, if the concentration of products is increased, what will happen to the equilibrium? (2021)
Step 1: Understand that a reversible reaction can go in both directions: from reactants to products and from products to reactants.
Step 2: Know that equilibrium is the point where the rate of the forward reaction equals the rate of the reverse reaction.
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: Recognize that increasing the concentration of products means there are more products present in the reaction.
Step 5: According to Le Chatelier's principle, the system will try to reduce the effect of this increase by shifting the equilibrium to the left, which means favoring the formation of reactants.
