At high temperatures and low pressures, hydrogen sulfide and sulfur dioxide undergo the following reactions with associated partial pressure equilibrium ratios (K): HS H+0.5-S2, Kp1= 0.45 atm2 2.HS+SO 2 HO+1.5-S2, Kp2 = 28.5 atm/2 Initially, there is 1 mole of gas present with the following initial composition: 50 mol % HS, 25 mol % SO2, and the balance inert N. Assume that all species are in their gaseous state and exhibit ideal gas behavior. a) Based on Le Chatelier's Principle, what do you expect will be the effect of increasing pressure on the equilibrium conversion of HS in this reaction system? Explain why. Do you expect that the extent of reaction for reaction 1 (51) will have a different pressure dependency than that for reaction #2 (52)? In other words, do you expect that the ratio of (H/HO) produced will vary with pressure? b.) Compute and plot the equilibrium mole fractions of all species as a function of total pressure between 1 atm < P < 10 atm in increments of 1 atm.