At the Oak Ridge National Laboratory in Tennessee, soils are heavily contaminatedwith mercury (Hg*2). In some of the soils, sulfate-reducing bacteria are producingbisulfide (HS). In these soils, mercury precipitates with sulfide to form metacinnabar(HgS(s).HgS +H" Hg +HS(3),a. What is the equilibrium constant for this reaction? Assume a temperatureof 25 °C.b. What is the effective equilibrium constant for an ionic strength of 0.01 M(call it Kegeff)? Use the Davies equation to make the calculation

The complete balanced reaction = HgS (s) + H+ ↔ Hg+2 + HS-Given the temperature = 25∘CFor a general…

At the Oak Ridge National Laboratory in Tennessee, soils are heavily contaminated with mercury (Hg+2). In some of the soils, sulfate-reducing bacteria are producing bisulfide (HS'). In these soils, mercury precipitates with sulfide to form metacinnabar (HgS(). -2 HgS +H +Hg +HS (3), a. What is the equilibrium constant for this reaction? Assume a temperature of 25 °C. b. What is the effective equilibrium constant for an ionic strength of 0.01 M (call it Keeff)? Use the Davies equation to make the calculation

At the Oak Ridge National Laboratory in Tennessee, soils are heavily contaminated with mercury (Hg+2). In some of the soils, sulfate-reducing bacteria are producing bisulfide (HS'). In these soils, mercury precipitates with sulfide to form metacinnabar (HgS(). -2 HgS +H +Hg +HS (3), a. What is the equilibrium constant for this reaction? Assume a temperature of 25 °C. b. What is the effective equilibrium constant for an ionic strength of 0.01 M (call it Keeff)? Use the Davies equation to make the calculation

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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