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 for Engineering Students
3rd Edition
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter13: Electrochemistry
Section: Chapter Questions
Problem 13.88PAE
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3.15 (a) and (b) please help!
![### Corrosion of Elemental Iron in Anaerobic Waters
**Problem 3.15**
Consider the corrosion of elemental iron in anaerobic waters where iron (Fe⁰) is oxidized to Fe²⁺ with the reduction of protons (H⁺) to form hydrogen gas (H₂):
\[ \text{Fe}^0 + 2\text{H}^+ \rightarrow \text{Fe}^{2+} + \text{H}_2(g) \]
**Questions:**
(a) From thermodynamic considerations, calculate the equilibrium constant \( K \) at 25°C.
(b) For \( T = 25°C \), pH = 10, and \([\text{Fe}^{2+}] = 10^{-3} \, \text{M}\), at what partial pressure of \( \text{H}_2 \) does this reaction become unfavorable?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F726affd8-d374-453a-83e1-8f2ca39cc059%2Ff5cdc46c-2146-4a9f-9c67-7449965b683c%2F782di_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Corrosion of Elemental Iron in Anaerobic Waters
**Problem 3.15**
Consider the corrosion of elemental iron in anaerobic waters where iron (Fe⁰) is oxidized to Fe²⁺ with the reduction of protons (H⁺) to form hydrogen gas (H₂):
\[ \text{Fe}^0 + 2\text{H}^+ \rightarrow \text{Fe}^{2+} + \text{H}_2(g) \]
**Questions:**
(a) From thermodynamic considerations, calculate the equilibrium constant \( K \) at 25°C.
(b) For \( T = 25°C \), pH = 10, and \([\text{Fe}^{2+}] = 10^{-3} \, \text{M}\), at what partial pressure of \( \text{H}_2 \) does this reaction become unfavorable?
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