8. At high temperatures (in this case 800°C), hydrogen sulfide exists in an equilibrium with hydrogen gas and disulfur (S2 molecules, instead of. the normal S8 rings found in the solid): 2 H2S(g) = 2 H2(g) + S2(g) If the equilibrium constant is K = 1.7×10-7, and the equilibrium concentrations are [H2S] = 1.0 M, and [H2] = 4.9×10-3 M, what is the concentration of disulfur (S2)?

8. At high temperatures (in this case 800°C), hydrogen sulfide exists in an equilibrium with hydrogen gas and disulfur (S2 molecules, instead of. the normal S8 rings found in the solid): 2 H2S(g) = 2 H2(g) + S2(g) If the equilibrium constant is K = 1.7×10-7, and the equilibrium concentrations are [H2S] = 1.0 M, and [H2] = 4.9×10-3 M, what is the concentration of disulfur (S2)?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter13: Electrochemistry

Section: Chapter Questions

Problem 13.101PAE

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