In principle, is this reaction a feasible method of removing SO2 from power-plant emissions? View Available Hint(s) In principle, is this reaction a feasible method of removing from power-plant emissions? No; the reaction is highly spontaneous at 298 K, but a significant amount of SO2 will remain at equilibrium. Yes; the reaction is highly spontaneous at 298 K, even though a significant amount of SO2 will remain at equilibrium. Yes; the reaction is highly spontaneous at 298 K and almost no SO2 will remain at equilibrium. No; the reaction is not spontaneous at 298 K, even though almost no SO2 will remain at equilibrium. No; the reaction is not spontaneous at 298 K and a significant amount of SO2 will remain at equilibrium.

The question is incomplete, the complete question is:

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.

3. Yes; the reaction is highly spontaneous at 298 K and almost no SO2 will remain at equilibrium

Explanation:

Looking at the Kp of the of the reaction, we expect that almost no sulphur IV oxide should remain at equilibrium. The Kp has a a large value of 8×10^15 which indicates that the reaction should proceed to completion. The reaction is also spontaneous at 298K.

d.) circle motion requires a force to give it a centripetal acceleration.