Changing the temperature affects the equilibrium constant Kc and the formation of the Fe SCN 2+ complex ion from Fe3+ and SCN- ions according to Le Chatelier's principle. Le Chatelier's principle states that if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of reactants or products, the system will adjust its position to counteract the change and re-establish equilibrium.In the case of the reaction between Fe3+ and SCN- ions to form the Fe SCN 2+ complex ion, the balanced chemical equation is:Fe3+ aq + SCN- aq Fe SCN 2+ aq The equilibrium constant Kc for this reaction is given by:Kc = [Fe SCN 2+] / [Fe3+] [SCN-] Now, let's consider the effect of temperature on this reaction. The reaction between Fe3+ and SCN- ions is an exothermic reaction, meaning it releases heat as it proceeds. According to Le Chatelier's principle, if the temperature of the system is increased, the equilibrium will shift in the direction that absorbs heat, which in this case is the reverse left direction. As a result, the formation of the Fe SCN 2+ complex ion will decrease, and the concentrations of Fe3+ and SCN- ions will increase. Consequently, the value of Kc will decrease.On the other hand, if the temperature of the system is decreased, the equilibrium will shift in the direction that releases heat, which in this case is the forward right direction. As a result, the formation of the Fe SCN 2+ complex ion will increase, and the concentrations of Fe3+ and SCN- ions will decrease. Consequently, the value of Kc will increase.In summary, increasing the temperature will decrease the equilibrium constant Kc and the formation of the Fe SCN 2+ complex ion, while decreasing the temperature will increase the equilibrium constant Kc and the formation of the Fe SCN 2+ complex ion.