In a reversible reaction, if the concentration of reactants is increased, what will happen to the equilibrium position? (2021)
Practice Questions
1 question
Q1
In a reversible reaction, if the concentration of reactants is increased, what will happen to the equilibrium position? (2021)
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, if the concentration of reactants is increased, the equilibrium will shift to the right to favor the formation of products.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reversible reaction, if the concentration of reactants is increased, what will happen to the equilibrium position? (2021)
Solution: According to Le Chatelier's principle, if the concentration of reactants is increased, the equilibrium will shift to the right to favor the formation of products.
Steps: 6
Step 1: Understand what a reversible reaction is. It means the reaction can go in both directions: from reactants to products and from products back to reactants.
Step 2: Know what equilibrium means. Equilibrium is the point where the rate of the forward reaction equals the rate of the reverse reaction, and concentrations of reactants and products remain constant.
Step 3: Learn 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 reactants is increased.
Step 5: Apply Le Chatelier's principle. Since the concentration of reactants is increased, the system will try to reduce this change by using up some of the reactants.
Step 6: Determine the direction of the shift. To use up the added reactants, the equilibrium will shift to the right, favoring the formation of products.
