The reaction between hydrogen gas H2 and iodine gas I2 to form hydrogen iodide HI is an exothermic reaction, which can be represented by the following equation:H2 g + I2 g 2HI g + heatThe effect of temperature on the equilibrium constant K of this reaction can be explained using Le Chatelier's principle, which states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants and products, the system will adjust itself to counteract the change and restore a new equilibrium.In the case of an exothermic reaction like the one between hydrogen and iodine, increasing the temperature will cause the equilibrium to shift towards the reactants H2 and I2 to absorb the excess heat. This means that the equilibrium constant K will decrease as the temperature increases. Conversely, if the temperature is decreased, the equilibrium will shift towards the products HI to release heat, and the equilibrium constant K will increase.Now, let's discuss the effect of temperature on the reaction rate. The reaction rate is directly related to the kinetic energy of the reacting molecules. As the temperature increases, the kinetic energy of the molecules also increases, causing them to collide more frequently and with greater force. This leads to an increase in the reaction rate. Conversely, as the temperature decreases, the kinetic energy of the molecules decreases, resulting in fewer collisions and a slower reaction rate.In summary, for the reaction between hydrogen gas and iodine gas, increasing the temperature will decrease the equilibrium constant K and increase the reaction rate, while decreasing the temperature will increase the equilibrium constant K and decrease the reaction rate.