In a reversible reaction, if the concentration of reactants is increased, what w
Practice Questions
Q1
In a reversible reaction, if the concentration of reactants is increased, what will happen to the position of equilibrium? (2021)
It will shift to the right
It will shift to the left
It will remain unchanged
It will shift to the center
Questions & Step-by-Step Solutions
In a reversible reaction, if the concentration of reactants is increased, what will happen to the position of equilibrium? (2021)
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: Know what equilibrium means. Equilibrium is the point where the rate of the forward reaction equals the rate of the reverse reaction, and the 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. When the concentration of reactants increases, the system will try to reduce this change by using up the extra reactants.
Step 6: Determine the effect on equilibrium. To use up the extra reactants, the equilibrium will shift to the right, favoring the formation of products.
