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16.4 Exercise 20

Avg difficulty 2.5

Hydrogen sulfide is a pollutant found in natural gas. Following its removal, it is converted to sulfur by the reaction 2H2S(g)+SO2(g)⇌38S8(s,rhombic)+2H2O(l).\text{2H}_{2} \text{S} \left(g\right) + \text{SO}_{2} \left(g\right) \rightleftharpoons \frac{3}{8} \text{S}_{8} \left(s , \text{rhombic}\right) + \text{2H}_{2} \text{O} \left(l\right) . What is the equilibrium constant for this reaction? Is the reaction endothermic or exothermic?

OpenStax Chemistry 2e, 16.4 Free Energy, exercise 20

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Adapted from General Chemistry © 2019 Rice University. Licensed under CC BY 4.0. Sources: Chemistry 2e, Chemistry: Atoms First 2e. Imported at revision 32c7196.