When the temperature of a system at equilibrium is increased, Le Chatelier's principle states that the equilibrium will shift in the direction that absorbs the added heat. In this case, the balanced chemical equation is:A + B C + heatSince the reaction is exothermic, heat is released when the reaction proceeds in the forward direction from reactants A and B to product C . Therefore, when the temperature is increased, the equilibrium will shift in the direction that absorbs the added heat, which is the reverse direction from product C to reactants A and B .As a result, the concentration of the reactants A and B will increase, while the concentration of the product C will decrease. This shift in equilibrium will continue until a new equilibrium position is established at the higher temperature.In summary, increasing the temperature of an exothermic reaction will cause the equilibrium to shift towards the reactants, resulting in an increase in the concentration of reactants A and B and a decrease in the concentration of product C. This observation can be explained using Le Chatelier's principle, which states that a system at equilibrium will adjust to minimize the effect of any changes in temperature.