Final answer:
The reaction converting hydrogen sulfide to sulfur is likely to have a high equilibrium constant due to the production of solid sulfur and liquid water from gaseous reactants. Furthermore, the formation of these products typically releases energy, indicating that the reaction is exothermic. The correct option is C.
Step-by-step explanation:
The reaction in question, where hydrogen sulfide is converted to sulfur by a reaction with sulfur dioxide, can be represented as 2H₂S(g) + SO₂(g) = 3S(s, rhombic) + 2H₂O(l). The equilibrium constant for this reaction would depend on the specific conditions under which the reaction takes place, such as temperature and pressure.
However, given that the products include a solid (sulfur) and a liquid (water), and the reactants are gases, it is likely that the reaction will have a high equilibrium constant, indicating that the reaction proceeds to a great extent to form the products under standard conditions. This aligns with the principle that the formation of a solid from gaseous reactants typically drives the reaction towards the product side.
As for whether the reaction is endothermic or exothermic, considering the formation of solid sulfur and water, it is expected to be an exothermic process since the formation of strong chemical bonds typically releases energy. This is in line with the general understanding that the formation of solids from gases often releases energy. Thus, the most appropriate answer is that the reaction is exothermic with a high equilibrium constant.