human
For a reversible reaction, how does the position of equilibrium change when the concentration of reactants is increased or decreased?
gpt
Increasing the concentration of reactants leads to equilibrium shifting to the right-hand side (forward reaction), while decreasing the concentration of reactants leads to equilibrium shifting to the left-hand side.
Explanation: Le Chatelier's principle states that when the concentration of reactants is increased, the equilibrium shifts to the right to consume some of the added reactant, producing more products. Conversely, when the concentration of reactants is decreased, the equilibrium shifts to the left to produce more reactants and reduce the concentration of products, therefore maintaining equilibrium.