The reaction between hydrogen gas H2 and iodine gas I2 to form hydrogen iodide gas 2HI is an exothermic reaction, which means it releases heat. The balanced equation for this reaction is:H2 g + I2 g 2HI g According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants and products, the system will adjust its equilibrium position to counteract the change. In this case, increasing the temperature will cause the equilibrium to shift in the direction that absorbs the excess heat. Since the forward reaction is exothermic, the equilibrium will shift to the left toward the reactants to absorb the heat.As a result, the equilibrium constant K will decrease with an increase in temperature. This means that at higher temperatures, the reaction favors the formation of reactants H2 and I2 over the formation of the product HI .Regarding the reaction rate, increasing the temperature generally increases the reaction rate for both the forward and reverse reactions. This is because higher temperatures provide more kinetic energy to the molecules, increasing the frequency and energy of collisions between reactants. However, since the equilibrium shifts to favor the reactants, the overall rate of the forward reaction formation of HI will be slower at higher temperatures compared to lower temperatures.