The rate of a chemical reaction between potassium permanganate KMnO4 and oxalic acid C2H2O4 can be affected by changing the concentration of the reactants. This relationship can be explained by the collision theory and the rate law.According to the collision theory, the rate of a reaction depends on the frequency of effective collisions between the reacting particles. When the concentration of the reactants is increased, the number of particles per unit volume also increases. This leads to a higher probability of effective collisions between the reactant particles, resulting in an increased reaction rate.The rate law for the reaction between potassium permanganate and oxalic acid can be expressed as:rate = k [KMnO4]^m [C2H2O4]^nwhere rate is the reaction rate, k is the rate constant, [KMnO4] and [C2H2O4] are the concentrations of potassium permanganate and oxalic acid, respectively, and m and n are the reaction orders with respect to each reactant.In general, if the reaction order m or n is positive, increasing the concentration of the reactant will increase the reaction rate. If the reaction order is negative, increasing the concentration will decrease the reaction rate. If the reaction order is zero, the reaction rate is independent of the concentration of that reactant.For the reaction between potassium permanganate and oxalic acid, both m and n are typically positive, meaning that increasing the concentration of either reactant will increase the reaction rate. However, the exact values of m and n depend on the specific experimental conditions and the mechanism of the reaction.In summary, changing the concentration of reactants in the reaction between potassium permanganate and oxalic acid will affect the rate of the chemical reaction. Generally, increasing the concentration of either reactant will lead to an increased reaction rate due to a higher probability of effective collisions and the positive reaction orders.