At high temperatures and low pressures, hydrogen sulfide and sulfur dioxide unde

Question

At high temperatures and low pressures, hydrogen sulfide and sulfur dioxide undergo the following reactions with associated equilibrium constants H2S H2+0.5-S, K,-0.45 atm^0.5 The initial gas composition is 40 mol% H2S, 25 mol% SO2, and the balance inert N2. Assume ideal gas behavior. Assume that all species are in their gaseous state and exhibit ideal gas behavior. a) Based on Le Chatlier's Principle, what do you expect will be the effect of increasing pressure on the equilibrium conversion of H2S in this reaction system? Explain why. Do you expect that the extent of reaction for reaction l (5) will have a different pressure dependency than that for reaction #2 ()? In other words, do you expect that the ratio of (H2/H20) produced will vary with pressure? b.) Compute the equilibrium atm in increments of 1 atm. mole fractions of all species as a function of total pressure between 1 atm

Explanation / Answer

a.) According to Le Chatellier's principle, increase in pressure shifts the equilibrium to the side with less number of moles. So, for this reaction euilibrium moves to backward direction on increasing pressure. No, the ratio won't vary.

b.) Mole fraction of H2S= (0.4/0.65)= 0.615

Mole fraction of SO2= (0.25/0.65)= 0.384

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