Aluminum forms a tough oxide layer that protects the metal underneath from abrasion and further oxidation. A thin layer of this oxide forms naturally when in contact with air, but with electrochemical anodization one can produce a thicker layer that can significantly extend the lifetime of metal parts. The main form of aluminum oxide is Al2O3, which is a non-conductive network solid. It forms from aluminum via the following series of reactions: Al₂O3 (s) + 6 H+ (aq) + 6 e¯ = 2 Al (s) + 3 H₂0 (1) H₂ (g) = 2 H+ (aq) + 2 e¯ Eº = 0.00 V When exposed to a strong base such as sodium hydroxide, the aluminum oxide can etch away, dissolving: Al₂O3 (s) + 2OH(aq) + 3 H₂O (1) → 2 Al(OH) (aq) You will perform the anodization under acidic conditions, using concentrated sulfuric acid (approximately 18 M) as the electrolyte. Under acidic anodization conditions, aluminum forms first a "barrier layer" of dense oxide coating the electrode, then a thicker and more porous oxide coating (thickness depends on the duration of anodization) [1]. Eº = -1.55 V 3. Reaction studied: Based on the approximate concentration of H* in concentrated sulphuric acid, and assuming 0.212 M of H₂(g) initially present in the acid (based on typical atmospheric compositions), determine the Ecell expected under these conditions. Using the reaction on the top how would u solve question 3. Using the equations ecathode=ecathode- 0.0562(log(k))/ne and the similar equation for eanode the reaction must have H2 gas as a product
Aluminum forms a tough oxide layer that protects the metal underneath from abrasion and further oxidation. A thin layer of this oxide forms naturally when in contact with air, but with electrochemical anodization one can produce a thicker layer that can significantly extend the lifetime of metal parts. The main form of aluminum oxide is Al2O3, which is a non-conductive network solid. It forms from aluminum via the following series of reactions: Al₂O3 (s) + 6 H+ (aq) + 6 e¯ = 2 Al (s) + 3 H₂0 (1) H₂ (g) = 2 H+ (aq) + 2 e¯ Eº = 0.00 V When exposed to a strong base such as sodium hydroxide, the aluminum oxide can etch away, dissolving: Al₂O3 (s) + 2OH(aq) + 3 H₂O (1) → 2 Al(OH) (aq) You will perform the anodization under acidic conditions, using concentrated sulfuric acid (approximately 18 M) as the electrolyte. Under acidic anodization conditions, aluminum forms first a "barrier layer" of dense oxide coating the electrode, then a thicker and more porous oxide coating (thickness depends on the duration of anodization) [1]. Eº = -1.55 V 3. Reaction studied: Based on the approximate concentration of H* in concentrated sulphuric acid, and assuming 0.212 M of H₂(g) initially present in the acid (based on typical atmospheric compositions), determine the Ecell expected under these conditions. Using the reaction on the top how would u solve question 3. Using the equations ecathode=ecathode- 0.0562(log(k))/ne and the similar equation for eanode the reaction must have H2 gas as a product
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
![Aluminum forms a tough oxide layer that protects the metal underneath from abrasion and further oxidation.
A thin layer of this oxide forms naturally when in contact with air, but with electrochemical anodization one
can produce a thicker layer that can significantly extend the lifetime of metal parts.
The main form of aluminum oxide is Al2O3, which is a non-conductive network solid. It forms from aluminum
via the following series of reactions:
Al₂O3 (s) + 6 H+ (aq) + 6 e¯ ⇒ 2 Al (s) + 3 H₂0 (1)
H₂ (g) 2 H+ (aq) + 2 e¯ Eº = 0.00 V
When exposed to a strong base such as sodium hydroxide, the aluminum oxide can etch away, dissolving:
Al₂O3 (s) + 2OH(aq) + 3 H₂O (1) → 2 Al(OH) (aq)
You will perform the anodization under acidic conditions, using concentrated
sulfuric acid (approximately 18 M) as the electrolyte. Under acidic anodization
conditions, aluminum forms first a "barrier layer" of dense oxide coating the
electrode, then a thicker and more porous oxide coating (thickness depends on
the duration of anodization) [1].
Eº = -1.55 V
3. Reaction studied: Based on the approximate concentration of H* in concentrated sulphuric acid, and
assuming 0.212 M of H₂(g) initially present in the acid (based on typical atmospheric compositions),
determine the Ecell expected under these conditions.
Using the reaction on the top how would u solve question 3. Using the equations ecathode=ecathode-
0.0562(log(k))/ne and the similar equation for eanode
the reaction must have H2 gas as a product](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F008f31aa-ffde-472d-81b9-49fb75f4a0c2%2F65cfb312-397b-4504-98a0-da7954edd020%2F2b8rxfu_processed.png&w=3840&q=75)
Transcribed Image Text:Aluminum forms a tough oxide layer that protects the metal underneath from abrasion and further oxidation.
A thin layer of this oxide forms naturally when in contact with air, but with electrochemical anodization one
can produce a thicker layer that can significantly extend the lifetime of metal parts.
The main form of aluminum oxide is Al2O3, which is a non-conductive network solid. It forms from aluminum
via the following series of reactions:
Al₂O3 (s) + 6 H+ (aq) + 6 e¯ ⇒ 2 Al (s) + 3 H₂0 (1)
H₂ (g) 2 H+ (aq) + 2 e¯ Eº = 0.00 V
When exposed to a strong base such as sodium hydroxide, the aluminum oxide can etch away, dissolving:
Al₂O3 (s) + 2OH(aq) + 3 H₂O (1) → 2 Al(OH) (aq)
You will perform the anodization under acidic conditions, using concentrated
sulfuric acid (approximately 18 M) as the electrolyte. Under acidic anodization
conditions, aluminum forms first a "barrier layer" of dense oxide coating the
electrode, then a thicker and more porous oxide coating (thickness depends on
the duration of anodization) [1].
Eº = -1.55 V
3. Reaction studied: Based on the approximate concentration of H* in concentrated sulphuric acid, and
assuming 0.212 M of H₂(g) initially present in the acid (based on typical atmospheric compositions),
determine the Ecell expected under these conditions.
Using the reaction on the top how would u solve question 3. Using the equations ecathode=ecathode-
0.0562(log(k))/ne and the similar equation for eanode
the reaction must have H2 gas as a product
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps with 1 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY