Given the decomposition reaction: 2so3 (g) → 2so2 (g) + o2 (g) according to le châtelier's principle, which side of the reaction will be favored when more oxygen is added to the reaction chamber?

I believe that the answer A.)

A) The products will be favored.

Virtually all chemical reactions are accompanied by the liberation or uptake of heat. If we regard heat as a "reactant" or "product" in an endothermic or exothermic reaction respectively, we can use the Le Châtelier principle to predict the direction in which an increase or decrease in temperature will shift the equilibrium state. Thus for the oxidation of nitrogen, an endothermic process, we can write

[heat] + N2 (g) + O2 (g) → 2 NO (g)

Suppose this reaction is at equilibrium at some temperature T1 and we raise the temperature to T2. The Le Châtelier principle tells us that a net reaction will occur in the direction that will partially counteract this change. Since the reaction is endothermic, a shift of the equilibrium to the right will take place.