Porous silicon as base material of MEMS-compatible fuel cell components

Size: px
Start display at page:

Download "Porous silicon as base material of MEMS-compatible fuel cell components"

Transcription

1 Porous silicon as base material of MEMS-compatible fuel cell components José Geraldo Alves Brito Neto Tokyo University of Science - Faculty of Science and Technology Department of Mechanical Engineering - Hayase Group

2

3 Cathode Anode Galvanic Cells

4 Galvanic Cells Load Cathode Anode Salt Bridge

5 Anions Electrons Anode Side Reduced Reagent Cations Oxydized Product

6 Electrons Load Salt Bridge Cations Cathode Anode Anions

7 Cations Electrons Cathode side Anions Reduced Product Oxidized Reagent

8 Galvanic Cells Load Current Cathode Anode Salt Bridge

9 Galvanic Cells Current Load Anode Cathode

10 Galvanic Cells Current Load Ri Anode Cathode

11 Fuel Cells Electron donor: Fuel (H2, methanol, ethanol, glucose??) Electron acceptor: O2 Salt bridge: aqueous alkaline solution, molten alkaline carbonate, O2- conducting ceramic, polymeric electrolyte

12 Polymer Electrolyte Membrane Fuel Cells

13 Polymer Electrolyte Membrane Fuel Cells Nafion

14 Polymer Electrolyte Membrane Fuel Cells

15 Polymer Electrolyte Membrane Fuel Cells

16 Polymer Electrolyte Membrane Fuel Cells Current collector/ Field flow plates

17 Polymer Electrolyte Membrane Fuel Cells Gas diffusion layer

18 Polymer Electrolyte Membrane Fuel Cells Oxidation Catalyst Layer

19 Polymer Electrolyte Membrane Fuel Cells Anode

20 Polymer Electrolyte Membrane Fuel Cells Cathode Current collector Gas diffusion layer Reduction catalyst layer

21 Polymer Electrolyte Membrane Fuel Cells Polymer Electrolyte Membrane

22 Polymer Electrolyte Membrane Fuel Cells

23 Polymer Electrolyte Membrane Fuel Cells H2 O2

24 Current Collector Gas Diffusion Layer H2 Catalyst Layer Polymer Electrolyte Membrane H2 Electrons H+

25 Electrons Load H2 O2

26 Polymer Electrolyte Membrane Catalyst Layer Gas Diffusion Layer Current Collector H2O H+ O2 O2 Electrons

27 Polymer Electrolyte Membrane Fuel Cells Typically employed materials: Gas diffusion layer: carbon cloth Catalyst layer: platinum nanoparticles supported on finely divided carbon black Polymer electrolyte membrane: Nafion

28 source: Li et al - Electrochimica Acta

29 2 He (...) B C N O F Ne Al Si P S Cl Ar Cu Zn Ga Ge As Se Br Kr (...)

30 2 He (...) B C N O F Ne Al Si P S Cl Ar Cu Zn Ga Ge As Se Br Kr (...)

31 We must synthesize and manipulate porous materials by MEMS-compatible methods

32 We must synthesize and manipulate porous materials by MEMS-compatible methods Porous Silicon

33 Porous Silicon Silicon Wafer Counter electrode HF-containing bath

34 Porous Silicon Facile synthesis Compatible to MEMS technologies Wide range of pore morphologies can be obtained by changing simple parameters.

35 Porous Silicon Porous layer 5 m Bulk silicon

36 Porous Silicon

37 Porous Silicon Porous layer Bulk silicon 500nm

38 Porous Silicon

39 Immersion plating By immersion of the porous silicon sample in a solution containing PtCl62ions and HF, the following reactions take place: PtCl62-(aq) + Si(s) + 2H2O - SiO2(s) + 6F (aq) + 4H+(aq) - Pt(s) + SiO2(s) + 4H+(aq) + 6Cl (aq) SiF62-(aq) + 2H2O

40 Porous layer 5 m Bulk silicon

41 Porous platinum!! Porous layer Bulk silicon 5 m

42 138 Pt M line 810 Si K line 5 m Porous layer Bulk Silicon 5 m 0 0

43

44 Porous Platinum Roughness factors on the order of 600; Area/volume rations on the order of 80 m2/cm3

45

46 Cell assembly Silicon wafer Oxide layer

47 Cell assembly Removal of oxide layers by dipping in concentrated HF

48 Cell assembly Sputtering of a Cu layer

49 Cell assembly Patterned dissolution of the Cu layer

50 Cell assembly Formation of a porous silicon layer on the opposite face

51 Cell assembly Immersion plating of the Pt catalyst

52 Cell assembly Deposition of Ti and Au contact bands

53 Cell assembly Plasma etching of the fuel channels

54

55 Cell assembly Anode Cathode

56 Cell assembly Anode Polymer Electrolyte Membrane Cathode

57 Cell assembly Hot pressing of the membrane-electrode assembly Anode Polymer Electrolyte Membrane Cathode

58

59 Electrons H2 A Load Anode Cathode O2

60

61 Next Steps Extend the synthetic method to other metals Improve the characteristics of the porous Pt layers Solve problems of the cell assembly procedure Develop methods to produce other components of the cell based on porous silicon

62

Electrochemical Cells

Electrochemical Cells CH302 LaBrake and Vanden Bout Electrochemical Cells Experimental Observations of Electrochemical Cells 1. Consider the voltaic cell that contains standard Co 2+ /Co and Au 3+ /Au electrodes. The following

More information

Ch 11 Practice Problems

Ch 11 Practice Problems Ch 11 Practice Problems 1. How many electrons are transferred in the following reaction? 2Cr 2O 7 2- + 14H + + 6Cl 2Cr 3+ + 3Cl 2 + 7H 2O A) 2 B) 4 C) 6 D) 8 2. Which metal, Al or Ni, could reduce Zn 2+

More information

e - Galvanic Cell 1. Voltage Sources 1.1 Polymer Electrolyte Membrane (PEM) Fuel Cell

e - Galvanic Cell 1. Voltage Sources 1.1 Polymer Electrolyte Membrane (PEM) Fuel Cell Galvanic cells convert different forms of energy (chemical fuel, sunlight, mechanical pressure, etc.) into electrical energy and heat. In this lecture, we are interested in some examples of galvanic cells.

More information

Chemistry Instrumental Analysis Lecture 18. Chem 4631

Chemistry Instrumental Analysis Lecture 18. Chem 4631 Chemistry 4631 Instrumental Analysis Lecture 18 Oxidation/Reduction Reactions Transfer of electrons in solution from one reactant to another. Ce +4 + Fe +2 Ce +3 + Fe +3 Ce +4 and Fe 3+ Fe 2+ and Ce 3+

More information

25. A typical galvanic cell diagram is:

25. A typical galvanic cell diagram is: Unit VI(6)-III: Electrochemistry Chapter 17 Assigned Problems Answers Exercises Galvanic Cells, Cell Potentials, Standard Reduction Potentials, and Free Energy 25. A typical galvanic cell diagram is: The

More information

Introduction. can be rewritten as follows: Oxidation reaction. H2 2H + +2e. Reduction reaction: F2+2e 2F. Overall Reaction H2+F2 2H + +2F

Introduction. can be rewritten as follows: Oxidation reaction. H2 2H + +2e. Reduction reaction: F2+2e 2F. Overall Reaction H2+F2 2H + +2F Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to

More information

Chapter 7 Electrochemistry

Chapter 7 Electrochemistry Chapter 7 Electrochemistry Outside class reading Levine: pp. 417 14.4 Galvanic cells: pp. 423 14.5 types of reversible electrodes 7.6.1 Basic concepts of electrochemical apparatus (1) Electrochemical apparatus

More information

ELECTROCHEMICAL CELLS

ELECTROCHEMICAL CELLS ELECTROCHEMICAL CELLS Electrochemistry 1. Redox reactions involve the transfer of electrons from one reactant to another 2. Electric current is a flow of electrons in a circuit Many reduction-oxidation

More information

lect 26:Electrolytic Cells

lect 26:Electrolytic Cells lect 26:Electrolytic Cells Voltaic cells are driven by a spontaneous chemical reaction that produces an electric current through an outside circuit. These cells are important because they are the basis

More information

Introduction to electrochemistry

Introduction to electrochemistry Introduction to electrochemistry Oxidation reduction reactions involve energy changes. Because these reactions involve electronic transfer, the net release or net absorption of energy can occur in the

More information

Electrical Conduction. Electrical conduction is the flow of electric charge produced by the movement of electrons in a conductor. I = Q/t.

Electrical Conduction. Electrical conduction is the flow of electric charge produced by the movement of electrons in a conductor. I = Q/t. Electrical Conduction e- in wire e- out Electrical conduction is the flow of electric charge produced by the movement of electrons in a conductor. The rate of electron flow (called the current, I, in amperes)

More information

ELECTROCHEMISTRY. Oxidation/Reduction

ELECTROCHEMISTRY. Oxidation/Reduction ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Examples: voltaic cells, batteries. NON-SPONTANEOUS

More information

18.3 Electrolysis. Dr. Fred Omega Garces. Chemistry 201. Driving a non-spontaneous Oxidation-Reduction Reaction. Miramar College.

18.3 Electrolysis. Dr. Fred Omega Garces. Chemistry 201. Driving a non-spontaneous Oxidation-Reduction Reaction. Miramar College. 18.3 Electrolysis Driving a non-spontaneous Oxidation-Reduction Reaction Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Electrolysis Voltaic Vs. Electrolytic Cells Voltaic Cell Energy is released

More information

11.3. Electrolytic Cells. Electrolysis of Molten Salts. 524 MHR Unit 5 Electrochemistry

11.3. Electrolytic Cells. Electrolysis of Molten Salts. 524 MHR Unit 5 Electrochemistry 11.3 Electrolytic Cells Section Preview/ Specific Expectations In this section, you will identify the components of an electrolytic cell, and describe how they work describe electrolytic cells using oxidation

More information

Redox and Electrochemistry

Redox and Electrochemistry Redox and Electrochemistry 1 Electrochemistry in Action! 2 Rules for Assigning Oxidation Numbers The oxidation number of any uncombined element is 0. The oxidation number of a monatomic ion equals the

More information

Electrochemistry. Electrochemical Process. The Galvanic Cell or Voltaic Cell

Electrochemistry. Electrochemical Process. The Galvanic Cell or Voltaic Cell Electrochemistry Electrochemical Process The conversion of chemical energy into electrical energy and the conversion of electrical energy into chemical energy are electrochemical process. Recall that an

More information

Chapter 18 Electrochemistry. Electrochemical Cells

Chapter 18 Electrochemistry. Electrochemical Cells Chapter 18 Electrochemistry Chapter 18 1 Electrochemical Cells Electrochemical Cells are of two basic types: Galvanic Cells a spontaneous chemical reaction generates an electric current Electrolytic Cells

More information

CHAPTER 5 REVIEW. C. CO 2 D. Fe 2 O 3. A. Fe B. CO

CHAPTER 5 REVIEW. C. CO 2 D. Fe 2 O 3. A. Fe B. CO CHAPTER 5 REVIEW 1. The following represents the process used to produce iron from iron III oxide: Fe 2 O 3 + 3CO 2Fe + 3CO 2 What is the reducing agent in this process? A. Fe B. CO C. CO 2 D. Fe 2 O 3

More information

Sample Exercise 20.2 Practice Exercise 1 with feedback

Sample Exercise 20.2 Practice Exercise 1 with feedback Homework Chapter 20 Due: 11:59pm on Wednesday, November 16, 2016 You will receive no credit for items you complete after the assignment is due. Grading Policy Sample Exercise 20.2 Practice Exercise 1 with

More information

(c) dilute solution of glucose (d) chloroform 12 Which one of the following represents the same net reaction as the electrolysis of aqueous H2SO4

(c) dilute solution of glucose (d) chloroform 12 Which one of the following represents the same net reaction as the electrolysis of aqueous H2SO4 1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy (d) none of these 2 Standard hydrogen electrode has an

More information

Electrochemistry Pulling the Plug on the Power Grid

Electrochemistry Pulling the Plug on the Power Grid Electrochemistry 18.1 Pulling the Plug on the Power Grid 18.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions 18.4 Standard Electrode Potentials 18.7 Batteries:

More information

CHM 213 (INORGANIC CHEMISTRY): Applications of Standard Reduction Potentials. Compiled by. Dr. A.O. Oladebeye

CHM 213 (INORGANIC CHEMISTRY): Applications of Standard Reduction Potentials. Compiled by. Dr. A.O. Oladebeye CHM 213 (INORGANIC CHEMISTRY): Applications of Standard Reduction Potentials Compiled by Dr. A.O. Oladebeye Department of Chemistry University of Medical Sciences, Ondo, Nigeria Electrochemical Cell Electrochemical

More information

OXIDATION-REDUCTIONS REACTIONS. Chapter 19 (From next years new book)

OXIDATION-REDUCTIONS REACTIONS. Chapter 19 (From next years new book) OXIDATION-REDUCTIONS REACTIONS Chapter 19 (From next years new book) ELECTROCHEMICAL REACTIONS: What are electrochemical reactions? Electrons are transferred from one species to another ACTIVATING PRIOR

More information

Standard reduction potentials are established by comparison to the potential of which half reaction?

Standard reduction potentials are established by comparison to the potential of which half reaction? HW10 Electrochemical Poten al, Free Energy, and Applica ons This is a preview of the draft version of the quiz Started: Nov 8 at 5:51pm Quiz Instruc ons Question 1 What is the E for cell + 4+ 3+ Zn(s)

More information

Unit 12 Redox and Electrochemistry

Unit 12 Redox and Electrochemistry Unit 12 Redox and Electrochemistry Review of Terminology for Redox Reactions OXIDATION loss of electron(s) by a species; increase in oxidation number. REDUCTION gain of electron(s); decrease in oxidation

More information

Electrochemistry. Part One: Introduction to Electrolysis and the Electrolysis of Molten Salts

Electrochemistry. Part One: Introduction to Electrolysis and the Electrolysis of Molten Salts Part One: Introduction to Electrolysis and the Electrolysis of Molten Salts What do I need to know about electrochemistry? Electrochemistry Learning Outcomes: Candidates should be able to: a) Describe

More information

Chemistry 102 Chapter 19 OXIDATION-REDUCTION REACTIONS

Chemistry 102 Chapter 19 OXIDATION-REDUCTION REACTIONS OXIDATION-REDUCTION REACTIONS Some of the most important reaction in chemistry are oxidation-reduction (redox) reactions. In these reactions, electrons transfer from one reactant to the other. The rusting

More information

(c) Na is deposited at the cathode (d) Na appears at the anode

(c) Na is deposited at the cathode (d) Na appears at the anode year chemiry n0tes new CHAPTER 10 ELECTROCHEMISTRY MCQS Q.1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy

More information

mccord (pmccord) HW11 Electrochemistry I mccord (51520) 1

mccord (pmccord) HW11 Electrochemistry I mccord (51520) 1 mccord (pmccord) HW11 Electrochemistry I mccord (51520) 1 This print-out should have 27 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001

More information

Chapter 18. Electrochemistry

Chapter 18. Electrochemistry Chapter 18 Electrochemistry Section 17.1 Spontaneous Processes and Entropy Section 17.1 http://www.bozemanscience.com/ap-chemistry/ Spontaneous Processes and Entropy Section 17.1 Spontaneous Processes

More information

Galvanic Cells Spontaneous Electrochemistry. Electrolytic Cells Backwards Electrochemistry

Galvanic Cells Spontaneous Electrochemistry. Electrolytic Cells Backwards Electrochemistry Today Galvanic Cells Spontaneous Electrochemistry Electrolytic Cells Backwards Electrochemistry Balancing Redox Reactions There is a method (actually several) Learn one (4.10-4.12) Practice (worksheet)

More information

Electrochemistry Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry

Electrochemistry Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry 2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry Electricity from Chemistry Many chemical reactions involve the transfer of electrons between atoms or ions electron transfer

More information

possesses negative potential & undergoes oxidation preferably act as ANODE

possesses negative potential & undergoes oxidation preferably act as ANODE ELECTROCHEMISTRY Introduction: Electrochemistry is the area of Chemistry dealing with the interconversion of electrical energy and chemical energy. There are many applications of this in every day life.

More information

Electrochemistry. (Hebden Unit 5 ) Electrochemistry Hebden Unit 5

Electrochemistry. (Hebden Unit 5 ) Electrochemistry Hebden Unit 5 (Hebden Unit 5 ) is the study of the interchange of chemical energy and electrical energy. 2 1 We will cover the following topics: Review oxidation states and assigning oxidation numbers Redox Half-reactions

More information

Oxygen Reduction Reaction

Oxygen Reduction Reaction Electronic Supplementary Material (ESI) for RSC Advances. This journal is The Royal Society of Chemistry 2016 Oxygen Reduction Reaction Oxygen is the most common oxidant for most fuel cell cathodes simply

More information

Electrolytes for Fuel Cells

Electrolytes for Fuel Cells Electrolytes for Fuel Cells Tom Zawodzinski Materials Science and Technology Division Los Alamos National Laboratory Air-Breather Fuel Cell Stack Systems Laptop Demo DCH/Enable Prototype Small Battery

More information

Homework 11. Electrochemical Potential, Free Energy, and Applications

Homework 11. Electrochemical Potential, Free Energy, and Applications HW11 Electrochemical Poten!al, Free Energy, and Applica!ons Homework 11 Electrochemical Potential, Free Energy, and Applications Question 1 What is the E for Zn(s) Zn (aq) Ce (aq) Ce (aq) + cell + 4+ 3+

More information

Redox reactions Revision galvanic cells and fuel cells Lesson 7 Revise fuel cells by visiting the link below. www.dynamicscience.com.au/tester/solutions1/chemistry/redox/fuelcl.html 1) A fuel cell uses

More information

Nanowires and nanorods

Nanowires and nanorods Nanowires and nanorods One-dimensional structures have been called in different ways: nanowires, nanorod, fibers of fibrils, whiskers, etc. These structures have a nanometer size in one of the dimensions,

More information

(for tutoring, homework help, or help with online classes)

(for tutoring, homework help, or help with online classes) www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 20.4-3 In a voltaic cell electrons flow from the anode to the cathode. Value 2. chem10b 20.1-35 How many grams

More information

Electrochemical Cells

Electrochemical Cells Electrochemical Cells There are two types: Galvanic and Electrolytic Galvanic Cell: a cell in which a is used to produce electrical energy, i.e., Chemical energy is transformed into Electrical energy.

More information

Solutions for Assignment-6

Solutions for Assignment-6 Solutions for Assignment-6 Q1. What is the aim of thin film deposition? [1] (a) To maintain surface uniformity (b) To reduce the amount (or mass) of light absorbing materials (c) To decrease the weight

More information

The first three categories are considered a bottom-up approach while lithography is a topdown

The first three categories are considered a bottom-up approach while lithography is a topdown Nanowires and Nanorods One-dimensional structures have been called in different ways: nanowires, nanorod, fibers of fibrils, whiskers, etc. The common characteristic of these structures is that all they

More information

Electrochemical Cells

Electrochemical Cells Electrochemistry Electrochemical Cells The Voltaic Cell Electrochemical Cell = device that generates electricity through redox rxns 1 Voltaic (Galvanic) Cell An electrochemical cell that produces an electrical

More information

18.2 Voltaic Cell. Generating Voltage (Potential) Dr. Fred Omega Garces. Chemistry 201. Miramar College. 1 Voltaic Cell.

18.2 Voltaic Cell. Generating Voltage (Potential) Dr. Fred Omega Garces. Chemistry 201. Miramar College. 1 Voltaic Cell. 18.2 Voltaic Cell Generating Voltage (Potential) Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Voltaic Cell Redox Between If Zn (s) and Cu 2+ (aq) is in the same solution, then the electrons transfer

More information

Section Electrochemistry represents the interconversion of chemical energy and electrical energy.

Section Electrochemistry represents the interconversion of chemical energy and electrical energy. Chapter 21 Electrochemistry Section 21.1. Electrochemistry represents the interconversion of chemical energy and electrical energy. Electrochemistry involves redox (reduction-oxidation) reactions because

More information

ELECTROCHEMISTRY I. The science concerned with the study of electron transfer across phase boundary

ELECTROCHEMISTRY I. The science concerned with the study of electron transfer across phase boundary ELECTROCHEMISTRY I The science concerned with the study of electron transfer across phase boundary Electrode: Is a conducting material immersed in a media. Electrode potential: Is the potential difference

More information

Electrochemistry. The study of the interchange of chemical and electrical energy.

Electrochemistry. The study of the interchange of chemical and electrical energy. Electrochemistry The study of the interchange of chemical and electrical energy. Oxidation-reduction (redox) reaction: involves a transfer of electrons from the reducing agent to the oxidizing agent. oxidation:

More information

The goal of this project is to enhance the power density and lowtemperature efficiency of solid oxide fuel cells (SOFC) manufactured by atomic layer

The goal of this project is to enhance the power density and lowtemperature efficiency of solid oxide fuel cells (SOFC) manufactured by atomic layer Stanford University Michael Shandalov1, Shriram Ramanathan2, Changhyun Ko2 and Paul McIntyre1 1Department of Materials Science and Engineering, Stanford University 2Division of Engineering and Applied

More information

Chapter 19 ElectroChemistry

Chapter 19 ElectroChemistry Chem 1046 General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 11July2009 Chapter 19 ElectroChemistry These Notes are to SUPPLIMENT the Text,

More information

Ch 18 Electrochemistry OIL-RIG Reactions

Ch 18 Electrochemistry OIL-RIG Reactions Ch 18 Electrochemistry OIL-RIG Reactions Alessandro Volta s Invention Modified by Dr. Cheng-Yu Lai Daily Electrochemistry Appliactions Electrochemistry: The area of chemistry that examines the transformations

More information

Experiment 28 DIRECT METHANOL FUEL CELL

Experiment 28 DIRECT METHANOL FUEL CELL Experiment 28 Direct methanol fuel cell 1 Experiment 28 DIRECT METHANOL FUEL CELL Objective The purpose of this experiment is to learn the principle of direct methanol fuel cell (DMFC) and set up a simple

More information

Structural and Electronic properties of platinum nanoparticles studied by diffraction and absorption spectroscopy

Structural and Electronic properties of platinum nanoparticles studied by diffraction and absorption spectroscopy The 4 th SUNBEAM Workshop Structural and Electronic properties of platinum nanoparticles studied by in situ x-ray x diffraction and in situ x-ray x absorption spectroscopy Hideto Imai Fundamental and Environmental

More information

Section A: Summary Notes

Section A: Summary Notes ELECTROCHEMICAL CELLS 25 AUGUST 2015 Section A: Summary Notes Important definitions: Oxidation: the loss of electrons by a substance during a chemical reaction Reduction: the gain of electrons by a substance

More information

Chapter 18 problems (with solutions)

Chapter 18 problems (with solutions) Chapter 18 problems (with solutions) 1) Assign oxidation numbers for the following species (for review see section 9.4) a) H2SO3 H = +1 S = +4 O = -2 b) Ca(ClO3)2 Ca = +2 Cl = +5 O = -2 c) C2H4 C = -2

More information

Fernando O. Raineri. Office Hours: MWF 9:30-10:30 AM Room 519 Tue. 3:00-5:00 CLC (lobby).

Fernando O. Raineri. Office Hours: MWF 9:30-10:30 AM Room 519 Tue. 3:00-5:00 CLC (lobby). Fernando O. Raineri Office Hours: MWF 9:30-10:30 AM Room 519 Tue. 3:00-5:00 CLC (lobby). P1) What is the reduction potential of the hydrogen electrode g bar H O aq Pt(s) H,1 2 3 when the aqueous solution

More information

Supplementary Information. Seeding Approach to Noble Metal Decorated Conducting Polymer Nanofiber Network

Supplementary Information. Seeding Approach to Noble Metal Decorated Conducting Polymer Nanofiber Network Supplementary Information Seeding Approach to Noble Metal Decorated Conducting Polymer Nanofiber Network Zhen Liu, Selcuk Poyraz, Yang Liu, Xinyu Zhang* Department of Polymer and Fiber Engineering, Auburn

More information

Supplemental Information. Carbon Monoxide Gas Diffusion Electrolysis. that Produces Concentrated C 2 Products. with High Single-Pass Conversion

Supplemental Information. Carbon Monoxide Gas Diffusion Electrolysis. that Produces Concentrated C 2 Products. with High Single-Pass Conversion JOUL, Volume 3 Supplemental Information Carbon Monoxide Gas Diffusion Electrolysis that Produces Concentrated C 2 Products with High Single-Pass Conversion Donald S. Ripatti, Thomas R. Veltman, and Matthew

More information

Suppose, we want to measure the standard electrode potential for zinc electrode, then we construct the cell according to the following cell diagram

Suppose, we want to measure the standard electrode potential for zinc electrode, then we construct the cell according to the following cell diagram Standard Electrode Potential The galvanic cell has two electrode potentials; anode potential and cathode potential When the cell potential is measured with voltmeter, it gives the difference of both potentials

More information

Repetition: Ion Plating

Repetition: Ion Plating Repetition: Ion Plating Substrate HV (bis ca. 1kV) Optional ionization system Source Ionized filling gas Source material, ionized or neutral Repetition: Ion Plating Ion Species Separated ion source Ions

More information

Electrolysis and Faraday's laws of Electrolysis

Electrolysis and Faraday's laws of Electrolysis Electrolysis and Faraday's laws of Electrolysis Electrolysis is defined as the passage of an electric current through an electrolyte with subsequent migration of positively and negatively charged ions

More information

Chapter 20. Electrochemistry. Chapter 20 Problems. Electrochemistry 7/3/2012. Problems 15, 17, 19, 23, 27, 29, 33, 39, 59

Chapter 20. Electrochemistry. Chapter 20 Problems. Electrochemistry 7/3/2012. Problems 15, 17, 19, 23, 27, 29, 33, 39, 59 Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 20 John D. Bookstaver St. Charles Community College Cottleville, MO Chapter 20 Problems

More information

Electrochemistry : Electrochemistry is a branch of science which deals with the production of electricity from energy released during spontaneous

Electrochemistry : Electrochemistry is a branch of science which deals with the production of electricity from energy released during spontaneous Electrochemistry : Electrochemistry is a branch of science which deals with the production of electricity from energy released during spontaneous chemical reactions and the use of electric energy to bring

More information

Modeling of Electrochemical Cells: HYD Lecture 08. Composite Membranes

Modeling of Electrochemical Cells: HYD Lecture 08. Composite Membranes Modeling of Electrochemical Cells: Proton Exchange Membrane Fuel Cells HYD7007 01 Lecture 08. Composite Membranes Dept. of Chemical & Biomolecular Engineering Yonsei University Spring, 2011 Prof. David

More information

Technology for Micro- and Nanostructures Micro- and Nanotechnology

Technology for Micro- and Nanostructures Micro- and Nanotechnology Lecture 10: Deposition Technology for Micro- and Nanostructures Micro- and Nanotechnology Peter Unger mailto: peter.unger @ uni-ulm.de Institute of Optoelectronics University of Ulm http://www.uni-ulm.de/opto

More information

Topic 12 Redox Equilibria Revision Notes

Topic 12 Redox Equilibria Revision Notes 1) Redox Reactions Topic 12 Redox Equilibria Revision Notes Redox reactions involve the transfer of electrons e.g. in the reaction between zinc metal and copper (II) sulphate, electrons are transferred

More information

Chapter 20. Electrochemistry

Chapter 20. Electrochemistry Chapter 20. Electrochemistry 20.1 Oxidation-Reduction Reactions Oxidation-reduction reactions = chemical reactions in which the oxidation state of one or more substance changes (redox reactions). Recall:

More information

The Curious Case of Au Nanoparticles

The Curious Case of Au Nanoparticles The Curious Case of Au Nanoparticles Industrial reactions performed by metals 1 Low Au reactivity Predictions are typically based on d-band model Hold well for polycrystalline materials Coinage metals

More information

Oxidation & Reduction (Redox) Notes

Oxidation & Reduction (Redox) Notes Oxidation & Reduction (Redox) Notes Chemical Activity (or Chemical Reactivity) is the measure of the reactivity of elements. If an element has high activity, then it means that the element is willing to

More information

A voltaic cell using the following reaction is in operation: 2 Ag + (lm) + Cd(s) 2 Ag(s) + Cd 2+ (l M)

A voltaic cell using the following reaction is in operation: 2 Ag + (lm) + Cd(s) 2 Ag(s) + Cd 2+ (l M) 0. Cu (s) + 2Ag + Cu 2+ + 2Ag (s) If the equilibrium constant for the reaction above is 3.7x10 15, which of the following correctly describes the standard voltage, E o and the standard free energy change,

More information

3. Potentials and thermodynamics

3. Potentials and thermodynamics Electrochemical Energy Engineering, 2012 3. Potentials and thermodynamics Learning subject 1. Electrochemical reaction 2. Thermodynamics and potential 3. Nernst equation Learning objective 1. To set up

More information

Aim: What are electrochemical cells?

Aim: What are electrochemical cells? Aim: What are electrochemical cells? Electrochemistry Electrochemistry- involves a redox reaction and a flow of electrons TWO TYPES of ELECTROCHEMICAL CELLS 1.Voltaic (similar to a battery) 2.Electrolytic

More information

A + B C +D ΔG = ΔG + RTlnKp. Me n+ + ne - Me. Me n n

A + B C +D ΔG = ΔG + RTlnKp. Me n+ + ne - Me. Me n n A + B C +D ΔG = ΔG + RTlnKp Me n+ + ne - Me K p a a Me Me n a n e 1 mol madde 6.2 x 1 23 atom elektron yükü 1.62 x 1-19 C FARADAY SABİTİ: 6.2 x 1 23 x 1.62 x 1-19 = 96485 A.sn (= coulomb) 1 Faraday 965

More information

Electron Transfer Reactions

Electron Transfer Reactions ELECTROCHEMISTRY 1 Electron Transfer Reactions 2 Electron transfer reactions are oxidation- reduction or redox reactions. Results in the generation of an electric current (electricity) or be caused by

More information

What is a Voltaic Cell? Voltaic Cells a.k.a. Electrochemical cells. May 25, Voltaic Cells 2018.notebook

What is a Voltaic Cell? Voltaic Cells a.k.a. Electrochemical cells. May 25, Voltaic Cells 2018.notebook What is a? s a.k.a. Electrochemical cells Aim: To analyze the process of a spontaneous chemical reaction that produces electricity. Voltaic cell: an electrochemical cell where chemical energy is spontaneously

More information

ELECTROCHEMISTRY OXIDATION-REDUCTION

ELECTROCHEMISTRY OXIDATION-REDUCTION ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Can extract electrical energy from these.

More information

Electrochemistry Worksheets

Electrochemistry Worksheets Electrochemistry Worksheets Donald Calbreath, Ph.D. Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other interactive

More information

Chemistry 30 Review Test 3 Redox and Electrochemistry /55

Chemistry 30 Review Test 3 Redox and Electrochemistry /55 Chemistry 30 Review Test 3 Redox and Electrochemistry /55 Part I Multiple choice / Numerical Response Answer the following multiple choice questions on the scantron sheet. Answer the numerical response

More information

Introduction to Electrochemical reactions. Schweitzer

Introduction to Electrochemical reactions. Schweitzer Introduction to Electrochemical reactions Schweitzer Electrochemistry Create and or store electricity chemically. Use electricity to drive a reaction that normally would not run. Plating metal onto a metal

More information

Unit - 3 ELECTROCHEMISTRY VSA QUESTIONS (1 - MARK QUESTIONS) 3. Mention the purpose of salt-bridge placed between two half-cells of a galvanic cell?

Unit - 3 ELECTROCHEMISTRY VSA QUESTIONS (1 - MARK QUESTIONS) 3. Mention the purpose of salt-bridge placed between two half-cells of a galvanic cell? Unit - 3 ELECTROCHEMISTRY 1. What is a galvanic cell? VSA QUESTIONS (1 - MARK QUESTIONS) 2. Give the cell representation for Daniell Cell. 3. Mention the purpose of salt-bridge placed between two half-cells

More information

Exam3Fall2009thermoelectro

Exam3Fall2009thermoelectro Exam3Fall2009thermoelectro Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Thermodynamics can be used to determine all of the following EXCEPT

More information

Electrochemistry. Electrochemistry. Preliminary Concepts. More Preliminary Concepts. Daniell Cell. Electrochemical Cells

Electrochemistry. Electrochemistry. Preliminary Concepts. More Preliminary Concepts. Daniell Cell. Electrochemical Cells Electrochemistry Electrochemistry CHEM 102 T. Hughbanks Applications: Batteries Corrosion Industrial production of chemicals such as Cl 2, NaOH, F 2 and Al Biological electron transfer reactions Preliminary

More information

Electrochemistry and battery technology Contents

Electrochemistry and battery technology Contents Electrochemistry and battery technology Contents Introduction Redox overview voltaic cells, electrolytic cells, fuel cells, Primary and secondary batteries. Other batteries; Construction, working and applications

More information

AP Questions: Electrochemistry

AP Questions: Electrochemistry AP Questions: Electrochemistry I 2 + 2 S 2O 2-3 2 I - + S 4O 2-6 How many moles of I 2 was produced during the electrolysis? The hydrogen gas produced at the cathode during the electrolysis was collected

More information

Wksht 4.2 Aqueous Equilibria II

Wksht 4.2 Aqueous Equilibria II Wksht 4.2 Aqueous Equilibria II Date: 10/16/17 1. Label the type of titration each graph represents and whether their equivalence point ph values would be greater than, equal to, or less than 7. WA being

More information

CHEMISTRY 13 Electrochemistry Supplementary Problems

CHEMISTRY 13 Electrochemistry Supplementary Problems 1. When the redox equation CHEMISTRY 13 Electrochemistry Supplementary Problems MnO 4 (aq) + H + (aq) + H 3 AsO 3 (aq) Mn 2+ (aq) + H 3 AsO 4 (aq) + H 2 O(l) is properly balanced, the coefficients will

More information

Oxidation Numbers, ox #

Oxidation Numbers, ox # Oxidation Numbers, ox # are or numbers assigned to each or assuming that the are transferred from the electronegative element to the electronegative element. now mimic systems. ox # are written followed

More information

Electro Chemistry Part-II 1. Faraday s laws of electrolysis are related to the 1) Molar mass of the electrolyte 2) Equivalent weight of the cation or anion 3) Molecular mass of the electrolyte 4) Atomic

More information

Electrochemistry C020. Electrochemistry is the study of the interconversion of electrical and chemical energy

Electrochemistry C020. Electrochemistry is the study of the interconversion of electrical and chemical energy Electrochemistry C020 Electrochemistry is the study of the interconversion of electrical and chemical energy Using chemistry to generate electricity involves using a Voltaic Cell or Galvanic Cell (battery)

More information

CHEM J-8 June /01(a)

CHEM J-8 June /01(a) CHEM1001 2012-J-8 June 2012 22/01(a) A galvanic cell has the following cell reaction: D(s) + 2Zn 2+ (aq) 2Zn(s) + D 4+ (aq) Write the overall cell reaction in shorthand cell notation. E = 0.18 V 8 D(s)

More information

Chemistry Standard level Paper 1

Chemistry Standard level Paper 1 M15/4/CHEMI/SPM/ENG/TZ1/XX Chemistry Standard level Paper 1 Thursday 14 May 2015 (afternoon) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all

More information

CHAPTER 10 ELECTROCHEMISTRY TEXT BOOK EXERCISE Q1. Multiple choice questions. (i) The cathode reaction in the electrolysis of dill. H2SO4 with Pt electrode is (a) Reduction (b) Oxidation (c) Both oxidation

More information

Today. Electrochemistry in the World Batteries Fuel Cells Corrosion

Today. Electrochemistry in the World Batteries Fuel Cells Corrosion Today Electrochemistry in the World Batteries Fuel Cells Corrosion This is the most impractical 1.1 V battery X 1.1 V volt meter How can we get rid of the beaker and salt bridge? Can we use this to make

More information

Chemistry 1011 TOPIC TEXT REFERENCE. Electrochemistry. Masterton and Hurley Chapter 18. Chemistry 1011 Slot 5 1

Chemistry 1011 TOPIC TEXT REFERENCE. Electrochemistry. Masterton and Hurley Chapter 18. Chemistry 1011 Slot 5 1 Chemistry 1011 TOPIC Electrochemistry TEXT REFERENCE Masterton and Hurley Chapter 18 Chemistry 1011 Slot 5 1 18.5 Electrolytic Cells YOU ARE EXPECTED TO BE ABLE TO: Construct a labelled diagram to show

More information

EE C245 ME C218 Introduction to MEMS Design Fall 2007

EE C245 ME C218 Introduction to MEMS Design Fall 2007 EE C245 ME C218 Introduction to MEMS Design Fall 2007 Prof. Clark T.-C. Nguyen Dept. of Electrical Engineering & Computer Sciences University of California at Berkeley Berkeley, CA 94720 Lecture 5: ALD,

More information

Oxidation (oxidized): the loss of one or more electrons. Reduction (reduced): the gain of one or more electrons

Oxidation (oxidized): the loss of one or more electrons. Reduction (reduced): the gain of one or more electrons 1 of 13 interesting links: Battery Chemistry Tutorial at http://www.powerstream.com/batteryfaq.html Duracell Procell: Battery Chemistry at http://www.duracell.com/procell/chemistries /default.asp I. Oxidation

More information

Batteries (Electrochemical Power Sources)

Batteries (Electrochemical Power Sources) Batteries (Electrochemical Power Sources) 1. Primary (single-discharge) batteries. => finite quantity of the reactants 2. Secondary or rechargeable batteries => regeneration of the original reactants by

More information

Chapter 22. Bulk Electrolysis: Electrogravimetry and Coulometry. Definition. Features of Bulk Electrolysis Cells

Chapter 22. Bulk Electrolysis: Electrogravimetry and Coulometry. Definition. Features of Bulk Electrolysis Cells Chapter 22 Bulk Electrolysis: Electrogravimetry and Coulometry Definition Bulk Electrolysis deals with methods that involve electrolysis producing a quantitative change in oxidation state Example: In a

More information

Ch. 13 Fundamentals of Electrochemistry

Ch. 13 Fundamentals of Electrochemistry Ch. 13 Fundamentals of Electrochemistry 13.1 13-1. Basic Concepts of electrochemistry redox reaction : reactions with electron transfer oxidized : loses electrons reduced : gains electrons Fe 3+ + V 2+

More information

CHAPTER 6: Etching. Chapter 6 1

CHAPTER 6: Etching. Chapter 6 1 Chapter 6 1 CHAPTER 6: Etching Different etching processes are selected depending upon the particular material to be removed. As shown in Figure 6.1, wet chemical processes result in isotropic etching

More information