3.15 Consider the corrosion of elemental iron in anaerobic waters (Fe° oxidized to Fe2+). with the reduction of protons (H*) to form hydrogen gas(H,): Fe + 2H* = Fe²+ + H2(g) (a) From thermodynamic considerations, calculate the equilibrium constant K at 25°C. (b) For T = 25°C, pH = 10, and [Fe"] = 10¬³ M, at what partial pressure of H, does this reaçtion become unfavorable?

3.15 Consider the corrosion of elemental iron in anaerobic waters (Fe° oxidized to Fe2+). with the reduction of protons (H) to form hydrogen gas(H,): Fe + 2H = Fe²+ + H2(g) (a) From thermodynamic considerations, calculate the equilibrium constant K at 25°C. (b) For T = 25°C, pH = 10, and [Fe"] = 10¬³ M, at what partial pressure of H, does this reaçtion become unfavorable?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter23: Organic Polymers, Natural And Synthetic

Section: Chapter Questions

Problem 47QAP: Plants synthesize carbohydrates from CO2 and H2O by the process of photosynthesis. For example,...

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