Increasing the temperature in this reaction will shift the equilibrium to the right.
To understand why, we need to consider Le Chatelier's principle. Le Chatelier's principle states that if a system at equilibrium is subjected to a change, it will adjust to minimize the effect of that change and restore equilibrium.
In this reaction, the formation of SO3 is exothermic, meaning it releases heat. By increasing the temperature, we are essentially adding more heat to the system. According to Le Chatelier's principle, the reaction will try to counteract this increase in temperature by moving in the direction that consumes heat.
To consume heat, the reaction needs to produce more SO3 molecules, as 2SO2(g) + O2(g) → 2SO3(g) + Heat is the forward reaction. Therefore, increasing the temperature will shift the equilibrium to the right, favoring the formation of more SO3 molecules.
In summary, increasing the temperature will shift the equilibrium of this reaction to the right.