In a dynamic equilibrium, the rates of the forward and backward reactions are equal, which means the concentrations of reactants and products remain constant over time. When the temperature is changed, it does affect the equilibrium position and the rate of the forward and backward reactions, particularly if the reactions involve an endothermic or exothermic process.
If the forward reaction is endothermic, meaning it absorbs heat from the surroundings, increasing the temperature will favor the forward reaction according to Le Chatelier's principle. This is because by increasing the temperature, you are providing additional energy to the system, which helps overcome the activation energy barrier and allows more reactant molecules to have sufficient energy to convert into products. Consequently, the rate of the forward reaction will increase, and the equilibrium will shift towards the product side.
Conversely, if the forward reaction is exothermic, meaning it releases heat to the surroundings, increasing the temperature will favor the backward reaction. In this case, raising the temperature will provide additional energy to the products, enabling more product molecules to have sufficient energy to convert back into reactants. As a result, the rate of the backward reaction will increase, and the equilibrium will shift towards the reactant side.
In summary, the effect of changing temperature on a dynamic equilibrium depends on the endothermic or exothermic nature of the forward reaction. Increasing the temperature favors the reaction that absorbs heat (endothermic) and shifts the equilibrium towards the products. Conversely, it favors the reaction that releases heat (exothermic) and shifts the equilibrium towards the reactants.