The reaction between hydrogen peroxide H2O2 and iodide ions I- is a well-known redox reaction, which can be represented by the following equation:H2O2 aq + 2I- aq + 2H+ aq 2H2O l + I2 aq The effect of changing the concentration of the reactants on the reaction rate and reaction yield can be analyzed using the principles of chemical kinetics and equilibrium.1. Effect on reaction rate:According to the rate law and collision theory, the rate of a reaction is directly proportional to the product of the concentrations of the reactants raised to their respective orders in the rate law expression. For the reaction between H2O2 and I-, the rate law can be expressed as:Rate = k[H2O2]^m[I-]^nWhere k is the rate constant, m and n are the orders of the reaction with respect to H2O2 and I-, respectively. In general, increasing the concentration of either H2O2 or I- will increase the reaction rate, as there will be more collisions between the reactant particles per unit time, leading to a higher probability of successful reactions.2. Effect on reaction yield:The reaction yield is the amount of product formed at equilibrium. For the reaction between H2O2 and I-, the reaction goes to completion, meaning that all the limiting reactant is consumed, and the reaction yield is determined by the stoichiometry of the balanced equation. In this case, the reaction yield is not affected by the initial concentrations of H2O2 and I-, as long as there is enough of the other reactant to react completely with the limiting reactant.However, if there are side reactions or competing reactions that can occur, the reaction yield may be affected by the initial concentrations of the reactants. In such cases, optimizing the concentrations of the reactants can help maximize the desired product yield while minimizing the formation of undesired products.In summary, changing the concentration of the reactants in the reaction between hydrogen peroxide and iodide ions will affect the reaction rate, with higher concentrations leading to faster reaction rates. The reaction yield, in this case, is determined by the stoichiometry of the balanced equation and is not directly affected by the initial concentrations of the reactants, as long as there is enough of the other reactant to react completely with the limiting reactant.