Using chemistry to generate electricity

Slides:



Advertisements
Similar presentations
Chapter 20 Electrochemistry
Advertisements

Electrochemistry Batteries. Batteries Lead-Acid Battery A 12 V car battery consists of 6 cathode/anode pairs each producing 2 V. Cathode: PbO 2 on a metal.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electrochemistry The study of the interchange of chemical and electrical energy.
Representing electrochemical cells The electrochemical cell established by the following half cells: Zn(s) --> Zn 2+ (aq) + 2 e - Cu 2+ (aq) + 2 e - -->
Predicting Spontaneous Reactions
20-2 Batteries A battery is a group of cells in a series...the total charge is the sum of the charges of the cells. D,C,AA, AAA and other similar products.
Section 18.1 Electron Transfer Reactions 1.To learn about metal-nonmetal oxidation–reduction reactions 2.To learn to assign oxidation states Objectives.
Electrochemistry is the chemistry of reactions which involve electron transfer. In spontaneous reactions electrons are released with energy which can.
Electrochemistry Chapter 19.
“minimal” galvanic cells
Electrochemistry. Electrochemical Cells  Electrons are transferred between the particles being oxidized and reduced  Two types –Spontaneous = Voltaic.
Chemistry 100 – Chapter 20 Electrochemistry. Voltaic Cells.
Batteries A galvanic cell or a group of galvanic cells connected in series Source of portable power Several types of battery in use today; we’ll look.
Inorganic chemistry Assistance Lecturer Amjad Ahmed Jumaa  Batteries and their application.  Primary (nonrecharge able) batteries. 
 Deals with the relation of the flow of electric current to chemical changes and the conversion of chemical to electrical energy (Electrochemical Cell)
Applications of Electrochemical Cells: (Batteries)
18.8 Electrolysis 2 Types of electrochemistry 1.Battery or Voltaic Cell – Purpose? 2.Electrolysis - forces a current through a cell to produce a chemical.
Oxidation-Reduction Dr. Ron Rusay Fall 2001 © Copyright 2001 R.J. Rusay.
 Conversion of chemical energy and electrical energy  All involve redox reactions  Electrochemical Cell: any device that converts chemical energy into.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.
Unit 16 Electrochemistry Oxidation & Reduction. Oxidation verses Reduction Gain oxygen atoms 2 Mg + O 2  2 MgO Lose electrons (e - ) Mg (s)  Mg + 2.
What exactly are batteries?. Batteries  Connects objects  Converts chemical---electrical energy  Two or more voltaic cells connected to each other.
Brain Warmup Half-Reaction ℰ ° (V) Ag + + e -  Ag 0.80 Cu e -  Cu 0.34 Zn e -  Zn-0.76 Al e -  Al-1.66 What is ℰ ° for each of the.
Prentice-Hall © 2007 General Chemistry: Chapter 20 Slide 1 of 54 Juana Mendenhall, Ph.D. Assistant Professor Lecture 4 March 22 Chapter 20: Electrochemistry.
OXIDATION ANY REACTION IN WHICH A SUBSTANCE LOSES ELECTRONS
Electrochemistry Part Four. CHEMICAL CHANGE  ELECTRIC CURRENT To obtain a useful current, we separate the oxidizing and reducing agents so that electron.
Electrochemistry.
Oxidation-Reduction Chemistry
Oxidation-Reduction Reactions
Chem. 1B – 11/8 Lecture.
Engineering Chemistry CHM 406
Electrochemistry Chapter 18.
Chapter 27 – Cells and Batteries
Chemsheets AS006 (Electron arrangement)
Introductory Chemistry, 3rd Edition Nivaldo Tro
Electrolytic Cells galvanic cell electrolytic cell 2 H2(g) + O2(g) 
CHAPTER 16 (pages ) Oxidation and Reduction
Electrochemistry and The Chemical Cells.
Photovoltaic Systems Engineering
“minimal” galvanic cells
Chapter 21: Electrochemistry
Cells & Batteries.
Redox Reactions and Electrochemistry
Batteries and Galvanic Cells
Electrochemistry the study of the interchange of chemical and electrical energy.
Chemsheets AS006 (Electron arrangement)
Electrochemistry Chapter 19
“minimal” galvanic cells
CHAPTER 15 Electro-chemistry 15.4 Electrochemical Cells.
Chapter 15 Oxidation and Reduction
Electrochemistry.
Electrochemistry.
Electrolytic Cells galvanic cell electrolytic cell 2 H2(g) + O2(g) 
Electrochemistry Oxidation & Reduction
Standard Reduction (Half-Cell) Potentials
Batteries and Galvanic Cells
ELECTROLYSIS.
Electrochemistry Chapter 19

Electrochemistry AP Chapter 20.
Photovoltaic Systems Engineering
Chapter 18 Electrochemistry Lesson 2
Electrochemistry Chapter 19
Chapter 21 Thanks to D Scoggin Cabrillo College
Section 1 Introduction to Electrochemistry
A. Oxidation-Reduction Reactions
Electrochemistry Chapter 19
ELECTROCHEMISTRY CHARGE (Q) – A property of matter which causes it to experience the electromagnetic force COULOMB (C) – The quantity of charge equal.
Redox in Electrochemistry
Presentation transcript:

Using chemistry to generate electricity Batteries Using chemistry to generate electricity

Dry Cell Batteries Common batteries (AA, AAA, 6V, 9V, etc.) Utilize electrolyte paste to minimize moisture content.

Dry Cell Batteries

Dry Cell Batteries Electron flow Zn (anode) is oxidized to lose 2 e- The NH4Cl paste gains to 2 e- to make NH3 and H2. MnO2 removes H2 and forms Mn2O3 and H2O.

Dry Cell Batteries More common alkaline batteries Use KOH as electrolyte paste to produce reaction under basic conditions. Have longer working life and longer shelf life Why? Zn anode corrodes less under basic conditions than acidic conditions.

Lead-Acid Storage Batteries Batteries used in automobiles

Lead Acid Batteries Consist of 6 cells in series (each produces 2V for a total of 12 V) Contains PbO2 cathode and Pb anode in sufuric acid solution. Pb(s) + PbO2(s) + HSO4-(aq) + 2H+(aq)  2PbSO4(s) + 2H2O(l) PbSO4 builds up on electrodes if run for too long without being charged (function of the alternator…) If too much builds up, battery goes dead.

Fuel Cells Reactants must be constantly replenished. Most common is Hydrogen-Oxygen fuel cell. H flows past anode (Pt catalyst) and undergoes oxidation O flows past cathode (similar catalyst) and undergoes reduction. Only product is water. Used in space shuttle program to provide drinking water for astronauts.

Other fuel cells Breathalyzers Measures ethanol content in bloodstream using redox reaction. Ethanol is oxidized to acetic acid Magnitude of electric current is directly proportional to alcohol content in bloodstream if calibrated correctly.

Rechargeable Batteries

Electrolytic Cells Electric current drives a nonspontaneous reaction through electrolysis. Eocell = negative since reaction is thermodynamically unfavored. Electrical force must be greater than cell potential.

Electrolytic vs. Galvanic Battery

Other uses Artifact restoration Electroplating Innovations in fuel cells For example: water + electricity  splits into H2(g) at the Cathode and O2(g) at the anode. If you could find a way to spontaneously use this method in conjunction with a fuel cell… that is the ultimate goal and will change the world.