In a reversible reaction, if the concentration of products increases, what happe

In a reversible reaction, if the concentration of products increases, what happens to the rate of the forward reaction? (2021)

In a reversible reaction, if the concentration of products increases, what happens to the rate of the forward reaction? (2021)

Step 1: Understand that a reversible reaction can go in two directions: forward (reactants to products) and backward (products to reactants).
Step 2: Recognize that when the concentration of products increases, it means there are more products present in the reaction mixture.
Step 3: Apply Le Chatelier's principle, which states that if a system at equilibrium is disturbed, it will shift to counteract the disturbance.
Step 4: Since the concentration of products has increased, the system will shift to the left to reduce the amount of products.
Step 5: This leftward shift means that the rate of the forward reaction (reactants forming products) will decrease.

No concepts available.