Adding more reactant or product to a chemical reaction affects the equilibrium position according to Le Chatelier's principle. Le Chatelier's principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust its equilibrium position to counteract the change.Here are three examples to illustrate this principle:1. Example 1: The Haber processN2 g + 3H2 g 2NH3 g In the Haber process, nitrogen gas reacts with hydrogen gas to form ammonia gas. If we increase the concentration of nitrogen gas N2 or hydrogen gas H2 , the equilibrium will shift to the right to produce more ammonia gas NH3 to counteract the change. Conversely, if we increase the concentration of ammonia gas NH3 , the equilibrium will shift to the left to produce more nitrogen gas N2 and hydrogen gas H2 .2. Example 2: The esterification reactionCH3COOH aq + CH3OH aq CH3COOCH3 aq + H2O l In the esterification reaction, acetic acid reacts with methanol to form methyl acetate and water. If we increase the concentration of acetic acid CH3COOH or methanol CH3OH , the equilibrium will shift to the right to produce more methyl acetate CH3COOCH3 and water H2O . On the other hand, if we increase the concentration of methyl acetate CH3COOCH3 or water H2O , the equilibrium will shift to the left to produce more acetic acid CH3COOH and methanol CH3OH .3. Example 3: The decomposition of dinitrogen tetroxide2N2O4 g 4NO2 g In this reaction, dinitrogen tetroxide decomposes into nitrogen dioxide. If we increase the concentration of dinitrogen tetroxide N2O4 , the equilibrium will shift to the right to produce more nitrogen dioxide NO2 to counteract the change. Conversely, if we increase the concentration of nitrogen dioxide NO2 , the equilibrium will shift to the left to produce more dinitrogen tetroxide N2O4 .In summary, adding more reactant or product to a chemical reaction affects the equilibrium position according to Le Chatelier's principle. The system will adjust its equilibrium position to counteract the change in concentration, either by shifting to the right toward the products or to the left toward the reactants .