In a reversible reaction, if the concentration of the reactants is increased, what will happen to the position of equilibrium? (2023)
Practice Questions
1 question
Q1
In a reversible reaction, if the concentration of the reactants is increased, what will happen to the position of equilibrium? (2023)
It will shift to the right
It will shift to the left
It will remain unchanged
It will shift to the center
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reversible reaction, if the concentration of the reactants is increased, what will happen to the position of equilibrium? (2023)
Solution: According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Steps: 6
Step 1: Understand what a reversible reaction is. It means that the reaction can go in both directions: from reactants to products and from products back to reactants.
Step 2: Learn about equilibrium. Equilibrium is the point in a reversible reaction where the rate of the forward reaction equals the rate of the backward reaction.
Step 3: Know about Le Chatelier's principle. This principle states that if a change is made to a system at equilibrium, the system will adjust to counteract that change.
Step 4: Identify the change in this scenario. The concentration of the reactants is increased.
Step 5: Apply Le Chatelier's principle. When the concentration of reactants increases, the system will try to reduce that concentration by shifting the equilibrium position.
Step 6: Determine the direction of the shift. The equilibrium will shift to the right, which means it will favor the formation of more products.
