The concentration of reactants affects the rate of an inorganic reaction according to the collision theory and the rate law. The collision theory states that for a reaction to occur, reactant particles must collide with the correct orientation and with sufficient energy to overcome the activation energy barrier. As the concentration of reactants increases, the number of particles in a given volume also increases, leading to a higher probability of successful collisions and thus a faster reaction rate.This relationship can be quantified using the rate law, which is an equation that relates the rate of a reaction to the concentrations of the reactants raised to some power. The general form of the rate law is:Rate = k[A]^m[B]^nwhere Rate is the reaction rate, k is the rate constant, [A] and [B] are the concentrations of reactants A and B, and m and n are the reaction orders with respect to A and B, respectively. The reaction orders m and n are determined experimentally and indicate how the rate is affected by the concentration of each reactant.To determine the rate law and the reaction orders, you can perform a series of experiments in which you vary the initial concentrations of the reactants and measure the initial reaction rate. By analyzing the data, you can determine the relationship between the concentration of each reactant and the reaction rate, and thus determine the reaction orders and the rate constant.For example, if you find that doubling the concentration of reactant A doubles the reaction rate while the concentration of reactant B remains constant, the reaction order with respect to A m would be 1. If you find that doubling the concentration of reactant B quadruples the reaction rate while the concentration of reactant A remains constant, the reaction order with respect to B n would be 2. In this case, the rate law would be:Rate = k[A]^1[B]^2This rate law quantitatively describes how the concentration of reactants affects the rate of the inorganic reaction, allowing you to predict the reaction rate under different conditions.