For an exothermic reaction, an increase in temperature causes the equilibrium to shift in the direction that consumes heat, which is the reverse reaction.
According to Le Chatelier's principle, when a system at equilibrium is subjected to a change, it responds by shifting the equilibrium position in a way that counteracts the effect of that change.
In the case of an exothermic reaction, where heat is released, increasing the temperature is considered an external stress. To counteract this stress and relieve the excess heat, the equilibrium will shift in the endothermic direction (the forward reaction), which absorbs heat.
By shifting the equilibrium towards the endothermic direction, the system consumes the additional heat, partially offsetting the temperature increase. This helps to restore equilibrium and maintain a relatively constant temperature.
It's important to note that the specific shift in equilibrium depends on other factors such as the reaction's enthalpy change, the concentration of reactants and products, and the activation energies involved. These factors collectively determine the magnitude and direction of the equilibrium shift in response to changes in temperature.