LeChatelier's Principle !!!! ?

plz help me with this problem
the following reaction may be used to remove sulfur compounds from power plant smokestack emission.

2HS(g) + SO2 >>>> 3S + 2H2O ...... DELTA h = -145 KJ
the value of the euilibrium constant for this reaction is 8.0*10^15 at 25 degree celsius.

a). given the value of K, is this reaction an effective way to clean smokestack emissions of sulfur compounds.?

b) would the efficiency of this reaction increase or decrease with increase in pressure?

c). how does the efficiency of this reaction in removing sulfur dioxide change as the temperature is increased?

Is that HS(g) or HS^-(g)? Is that S(s)?

A. A huge K means the equilibrium is far to the right.
B. If that is S(s) there are two moles on the right and 3 on the left so increased P would shift the equilibrium to the right.
c. Increased T shifts the equilibrium to the left.

a) To determine if the reaction is an effective way to clean smokestack emissions of sulfur compounds, we need to analyze the value of the equilibrium constant (K). The equilibrium constant tells us about the extent to which the reaction proceeds in the forward direction.

Since the value of K is very large (8.0*10^15), it indicates that the reaction significantly favors the production of products (S and H2O) at equilibrium. This means that the reaction is highly effective in removing sulfur compounds from power plant smokestack emissions.

b) Le Chatelier's Principle states that if a system at equilibrium is subjected to a change, it will respond in a way that partially counteracts the change. In the case of pressure, an increase in pressure shifts the equilibrium towards the side with fewer moles of gas.

In the given reaction, there are 3 moles of gas on the left-hand side (2HS and SO2) and only 2 moles of gas on the right-hand side (3S and 2H2O). Therefore, increasing the pressure will shift the equilibrium towards the left, reducing the efficiency of the reaction in removing sulfur compounds from smokestack emissions.

c) Similarly, Le Chatelier's Principle also applies to changes in temperature. If the temperature is increased, the reaction will respond by favoring the endothermic direction to absorb the additional heat. In this case, the forward reaction is endothermic as indicated by the negative delta H (-145 KJ).

By increasing the temperature, the equilibrium will shift to the right (forward reaction) in order to consume the excess heat. This will increase the efficiency of the reaction in removing sulfur dioxide from smokestack emissions.

In summary:
a) Yes, the reaction is an effective way to clean smokestack emissions of sulfur compounds due to the large value of the equilibrium constant.
b) The efficiency of the reaction will decrease with an increase in pressure.
c) The efficiency of the reaction will increase with an increase in temperature.