The reaction between potassium iodate KIO3 and sodium sulfite Na2SO3 in an acidic medium can be represented as:2IO3- + 5SO3^2- + 6H+ I2 + 5SO4^2- + 3H2OThe effect of temperature on the reaction rate and equilibrium can be explained using two principles: the Arrhenius equation and Le Chatelier's principle.1. Arrhenius equation: The reaction rate is directly proportional to the temperature. As the temperature increases, the kinetic energy of the molecules also increases, leading to more frequent and energetic collisions between the reactants. This results in a higher reaction rate. Mathematically, the Arrhenius equation is given by:k = Ae^-Ea/RT where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin. From this equation, it is evident that as the temperature T increases, the rate constant k also increases, leading to a faster reaction rate.2. Le Chatelier's principle: This principle states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants or products, the system will adjust itself to counteract the change and restore a new equilibrium. In the case of the reaction between potassium iodate and sodium sulfite in an acidic medium, increasing the temperature will affect the position of the equilibrium. If the reaction is exothermic releases heat , increasing the temperature will shift the equilibrium towards the reactants, favoring the reverse reaction. Conversely, if the reaction is endothermic absorbs heat , increasing the temperature will shift the equilibrium towards the products, favoring the forward reaction.In summary, increasing the temperature will generally increase the reaction rate between potassium iodate and sodium sulfite in an acidic medium. However, the effect of temperature on the position of the equilibrium depends on whether the reaction is exothermic or endothermic.