To determine the new equilibrium concentrations, we first need to know the reaction's equilibrium constant K and whether the reaction is exothermic or endothermic. However, this information is not provided in the problem. Assuming we know the reaction is exothermic releases heat and the initial equilibrium constant K1 at the initial temperature, we can use Le Chatelier's Principle to predict the effect of the temperature increase on the equilibrium.Le Chatelier's Principle states that if a change is applied to a system at equilibrium, the system will adjust itself to counteract that change. In this case, increasing the temperature will cause the equilibrium to shift in the direction that absorbs the added heat, which is the endothermic reverse direction:2 SO3 g 2 SO2 g + O2 g Now, let's use an ICE Initial, Change, Equilibrium table to find the new equilibrium concentrations: SO2 O2 SO3Initial 0.15 M 0.025 M 0 MChange +x +x/2 -xEquilibrium 0.15+x 0.025+x/2 xSince the reaction is exothermic, K will decrease as the temperature increases. Let's assume the new equilibrium constant is K2. We can now set up the equilibrium expression:K2 = [SO2]^2 * [O2] / [SO3]^2K2 = [ 0.15+x ^2 * 0.025+x/2 ] / x^2To solve for x, we would need the values of K1 and K2. Unfortunately, these values are not provided in the problem. If they were given, we could solve for x and find the new equilibrium concentrations of SO2, O2, and SO3.In summary, without the equilibrium constants and the nature of the reaction exothermic or endothermic , it is impossible to calculate the new equilibrium concentrations. However, we can predict that the equilibrium will shift towards the reactants SO2 and O2 due to the temperature increase if the reaction is exothermic.