Final answer:
Increasing the temperature of a chemical reaction results in a higher reaction rate and shifts the equilibrium to the right. According to kinetic-molecular theory, raising the temperature increases the average kinetic energy of particles, resulting in more extensive vibrations and translations. Higher temperatures also lead to a broader distribution of kinetic energies and an increase in entropy for any substance.
Step-by-step explanation:
Raising the temperature of the system is akin to increasing the amount of a reactant, and so the equilibrium will shift to the right. Lowering the system temperature will likewise cause the equilibrium to shift left. For exothermic processes, heat is viewed as a product of the reaction and so the opposite temperature dependence is observed.
According to kinetic-molecular theory, the temperature of a substance is proportional to the average kinetic energy of its particles. Raising the temperature of a substance will result in more extensive vibrations of the particles in solids and more rapid translations of the particles in liquids and gases. At higher temperatures, the distribution of kinetic energies among the atoms or molecules of the substance is also broader (more dispersed) than at lower temperatures. Thus, the entropy for any substance increases with temperature.
Increasing the temperature of a chemical reaction results in a higher reaction rate. When the reactant particles are heated, they move faster and faster, resulting in a greater frequency of collisions. An even more important effect of the temperature increase is that the collisions occur with a greater force, which means the reactants are more likely to surmount the activation energy barrier and go on to form products. Increasing the temperature of a reaction increases the frequency of collisions and the percentage of those collisions that are effective, resulting in an increased reaction rate.