For the following reaction if the reaction temperature was increased would the equilibrium shift to the right or the left,not shift at all,or you cant answer the question because Keq is not given?

2SO3(g)<-->2SO2(g)+O2(g)..(deltaH degrees =198kj)
Why???

To determine the effect of temperature on the equilibrium position of a reaction, we need to consider the reaction's enthalpy change (ΔH). In this case, the reaction is as follows:

2SO3(g) ⇌ 2SO2(g) + O2(g) (ΔH° = 198 kJ)

The reaction is exothermic, as indicated by the positive value of ΔH. When temperature is increased in an exothermic reaction, the equilibrium will shift to the left, favoring the reactants. Conversely, if the temperature is decreased, the equilibrium will shift to the right, favoring the products.

In this particular case, increasing the temperature would cause the equilibrium to shift to the left, producing more SO3(g) and reducing the concentration of SO2(g) and O2(g). This shift occurs because the forward reaction is exothermic, meaning it releases heat. By Le Chatelier’s principle, increasing the temperature prompts the system to counteract the change by favoring the endothermic (reverse) reaction.

Please note that this answer assumes the reaction is at equilibrium and Keq is not given. If you have the value of Keq, you can numerically determine the equilibrium shift based on the temperature using the Van't Hoff equation.