When an equilibrium reaction is exothermic, it releases heat as it proceeds from reactants to products. According to Le Chatelier's principle, if a change is made to a system at equilibrium, the system will adjust itself to counteract the change and restore a new equilibrium.In this case, the concentration of reactant A is increased, and the concentration of product B is decreased. According to Le Chatelier's principle, the system will try to counteract these changes by shifting the equilibrium position to consume the excess reactant A and produce more product B. This means the reaction will shift to the right toward the products .However, it's important to note that the equilibrium constant K is not affected by changes in concentration. The equilibrium constant is only affected by changes in temperature. Since there is no mention of a change in temperature in this problem, the equilibrium constant K will remain the same.In summary, the equilibrium position will shift to the right, favoring the formation of more product B, but the equilibrium constant K will not change as it is not affected by changes in concentration.