The reaction between potassium iodide KI and lead nitrate Pb NO3 2 is a precipitation reaction that forms lead iodide PbI2 and potassium nitrate KNO3 . The balanced chemical equation for this reaction is:2 KI aq + Pb NO3 2 aq 2 KNO3 aq + PbI2 s The effect of varying reactant concentrations on the rate and yield of this reaction can be understood through the principles of chemical kinetics and equilibrium.1. Reaction rate: The rate of a chemical reaction is directly proportional to the concentration of the reactants, as described by the rate law. For this reaction, the rate law can be expressed as:Rate = k [KI]^m [Pb NO3 2]^nwhere k is the rate constant, m and n are the reaction orders with respect to KI and Pb NO3 2, respectively. As the concentration of either or both reactants increases, the reaction rate will generally increase, leading to a faster formation of products.2. Reaction yield: The yield of a chemical reaction is the amount of product formed compared to the theoretical maximum amount that could be formed based on the limiting reactant. In the case of the KI and Pb NO3 2 reaction, the yield is mainly determined by the stoichiometry of the reaction and the solubility product constant Ksp of the precipitate PbI2 .If the reactant concentrations are increased, the amount of product formed PbI2 will also increase until the solubility limit is reached. Beyond this point, any additional reactant will not increase the yield of PbI2, as it will remain undissolved in the solution. However, the yield of the soluble product KNO3 will continue to increase as the reactant concentrations increase.In summary, increasing the reactant concentrations in the reaction between potassium iodide and lead nitrate will generally lead to an increased reaction rate and yield, up to the solubility limit of the precipitate. Beyond this point, the yield of the precipitate will not increase, but the yield of the soluble product will continue to increase.