What happens to the equilibrium position when the concentration of a reactant is
Practice Questions
Q1
What happens to the equilibrium position when the concentration of a reactant is increased?
The equilibrium shifts to the right
The equilibrium shifts to the left
No change occurs
The reaction stops
Questions & Step-by-Step Solutions
What happens to the equilibrium position when the concentration of a reactant is increased?
Step 1: Understand what equilibrium means. Equilibrium is a state where the rate of the forward reaction equals the rate of the reverse reaction in a chemical process.
Step 2: Know what a reactant is. A reactant is a substance that starts a chemical reaction.
Step 3: Learn about concentration. Concentration refers to how much of a substance is present in a given volume.
Step 4: Recognize 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 5: Apply the principle to the question. If you increase the concentration of a reactant, the system will try to reduce that concentration.
Step 6: Determine the direction of the shift. To reduce the concentration of the added reactant, the equilibrium will shift to the right, which means it will favor the formation of products.
