Final answer:
Increasing the temperature of an exothermic reaction like the combination of H2 and I2 to form HI will shift the equilibrium to the left, increasing the reactants and decreasing the product. For endothermic reactions, higher temperatures generally increase the product yield.
Step-by-step explanation:
Increasing the temperature of a reaction affects the yields of products and reactants based on Le Chatelier's Principle. For example, in the reaction H2(g) + I2(g) → 2 HI(g) + heat, increasing the temperature will increase the internal energy of the system. This will cause the reaction to shift left, increasing the concentration of H2 and I2 and decreasing the concentration of HI because the reaction gives off heat, making it an exothermic process. Conversely, an endothermic reaction would require more energy to maximize the yield, and thus a higher temperature may increase the production of products. An example is the dissolution of sugar in water, which occurs faster at higher temperatures. According to the ideal gas law, changes in temperature also influence the pressure and volume of gases involved, impacting the reaction equilibrium.