The question is incomplete. The complete question is
In principle, is this reaction a feasible method of removing SO_2 from power-plant emissions?
The reaction:
SO_2 (g) + 2 H2S (g) <=> 3 S(s) + 2 H2O(g)
is the basis of a suggested method for removal of {SO2} from power-plant stack gases.
Kp = 8×10^15
In principle, is this reaction a feasible method of removing SO_2 from power-plant emissions?
1. No; the reaction is highly spontaneous at 298 K, but a significant amount of SO2 will remain at equilibrium.
2. Yes; the reaction is highly spontaneous at 298 K, even though a significant amount of SO2 will remain at equilibrium.
3. Yes; the reaction is highly spontaneous at 298 K and almost no SO2 will remain at equilibrium.
4. No; the reaction is not spontaneous at 298 K, even though almost no SO2 will remain at equilibrium.
5. No; the reaction is not spontaneous at 298 K and a significant amount of SO2 will remain at equilibrium.
Answer:
3. Yes; the reaction is highly spontaneous at 298 K and almost no SO2 will remain at equilibrium.
Step-by-step explanation:
The equilibrium constant of the reaction Kp = 8×10^15. This value is very high. When the equilibrium constant is high, it implies that the reaction almost tends to completion. In this case completion of the reaction of the reaction implies the complete removal of SO2. Hence given the high equilibrium constant , almost all the SO2 is removed in the reaction.
∆G for the reaction is negative hence the reaction is spontaneous at 298K.