Changing the concentration of reactants in a chemical reaction can affect both the reaction rate and the position of the equilibrium, but it does not change the equilibrium constant.First, let's consider the reaction between iodine I2 and propanone CH3COCH3 in acidic solution:I2 + CH3COCH3 + H+ CH3COCH2I + HI1. Effect on reaction rate:The reaction rate is directly proportional to the concentration of the reactants. According to the rate law, the rate of the reaction can be expressed as:Rate = k[I2][CH3COCH3][H+]where k is the rate constant, and [I2], [CH3COCH3], and [H+] are the concentrations of iodine, propanone, and hydrogen ions, respectively. If the concentration of any of the reactants increases, the reaction rate will also increase, and if the concentration decreases, the reaction rate will decrease.2. Effect on equilibrium position:When the concentration of reactants changes, the position of the equilibrium will shift to either the left or the right to re-establish equilibrium. According to Le Chatelier's principle, if the concentration of a reactant increases, the equilibrium will shift to the right toward the products to counteract the change. Conversely, if the concentration of a reactant decreases, the equilibrium will shift to the left toward the reactants to counteract the change.3. Effect on equilibrium constant:The equilibrium constant Kc for a reaction is a fixed value at a given temperature and is independent of the initial concentrations of the reactants. Therefore, changing the concentration of the reactants does not affect the equilibrium constant. The equilibrium constant for this reaction can be expressed as:Kc = [CH3COCH2I][HI] / [I2][CH3COCH3][H+] In summary, changing the concentration of reactants in the reaction between iodine and propanone in acidic solution will affect the reaction rate and the position of the equilibrium, but it will not change the equilibrium constant.