Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg. 862-865 # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg. 862-865.

Slides:



Advertisements
Similar presentations
Redox potentials Electrochemistry ICS.
Advertisements

Electrochemistry Applications of Redox.
1 Suppose we had a 0.3A current producing 15mL of hydrogen gas in 6 min and 30 seconds. How much charge did we have per one mole of electrons? We need.
Electrochemistry.
Electrochemistry Quizzle Define the cathode. Where reduction occurs.
1 © 2006 Brooks/Cole - Thomson Balancing Equations for Redox Reactions Some redox reactions have equations that must be balanced by special techniques.
Electrochemistry Chapter 19
Chapter 20: Electrochemistry
Electrochemical Cells. Definitions Voltaic cell (battery): An electrochemical cell or group of cells in which a product-favored redox reaction is used.
19.2 Galvanic Cells 19.3 Standard Reduction Potentials 19.4 Spontaneity of Redox Reactions 19.5 The Effect of Concentration on Emf 19.8 Electrolysis Chapter.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electrochemistry The study of the interchange of chemical and electrical energy.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electrochemistry The study of the interchange of chemical and electrical energy.
Chapter 14 Electrochemistry. Basic Concepts Chemical Reaction that involves the transfer of electrons. A Redox reaction. Loss of electrons – oxidation.
Electrochemistry Part 1 Ch. 20 in Text (Omit Sections 20.7 and 20.8) redoxmusic.com.
Electrochemical Reactions
Electrochemistry Chapter 4.4 and Chapter 20. Electrochemical Reactions In electrochemical reactions, electrons are transferred from one species to another.
Electrochemistry. 17.1/17.2 GALVANIC CELLS AND STANDARD REDUCTION POTENTIALS Day 1.
Predicting Spontaneous Reactions
The End is in Site! Nernst and Electrolysis. Electrochemistry.
Chapter 17 Electrochemistry  Redox review (4.9)   
Electrochemistry Chapter 19.
Electrochemistry Chapter 19 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Redox Reactions and Electrochemistry
Chapter Oxidation states 20.2 half reactions.
Calculation of the standard emf of an electrochemical cell The procedure is simple: 1.Arrange the two half reactions placing the one with.
Electrochemistry Chapter 20 Electrochemistry. Electrochemistry Electrochemical Reactions In electrochemical reactions, electrons are transferred from.
Electrochemistry Chapter 19 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chapter 21: Electrochemistry II
Electrochemistry The study of the interchange of chemical and electrical energy. Sample electrochemical processes: 1) Corrosion 4 Fe (s) + 3 O 2(g) ⇌
Chapter 20 Electrochemistry Lecture Presentation © 2012 Pearson Education, Inc.
ELECTROCHEMISTRY Chap 20. Electrochemistry Sample Exercise 20.6 Calculating E° cell from E° red Using the standard reduction potentials listed in Table.
1 Electrochemistry. 2 Oxidation-Reduction Rxns Oxidation-reduction rxns, called redox rxns, are electron-transfer rxns. So the oxidation states of 1 or.
Redox Reactions and Electrochemistry Chapter 19. Voltaic Cells In spontaneous oxidation-reduction (redox) reactions, electrons are transferred and energy.
Electrochemistry Electrochemical Cells –Galvanic cells –Voltaic cells –Nernst Equation –Free Energy.
19.4 Spontaneity of Redox Reactions  G = -nFE cell  G 0 = -nFE cell 0 n = number of moles of electrons in reaction F = 96,500 J V mol = 96,500 C/mol.
Chapter 20 Electrochemistry. © 2009, Prentice-Hall, Inc. Oxidation Numbers In order to keep track of what loses electrons and what gains them, we assign.
The Nernst Equation Standard potentials assume a concentration of 1 M. The Nernst equation allows us to calculate potential when the two cells are not.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electrochemistry The study of the interchange of chemical and electrical energy.
Copyright © Houghton Mifflin Company. All rights reserved.17a–1.
Electrochemistry Chapter 19 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Nernst Equation Walther Nernst
Electrochemistry Combining the Half-Reactions 5 C 2 O 4 2−  10 CO e − 10 e − + 16 H MnO 4 −  2 Mn H 2 O When we add these together,
Electrochemistry © 2009, Prentice-Hall, Inc. Electrochemical Reactions In electrochemical reactions, electrons are transferred from one species to another.
Cell EMF Eocell = Eored(cathode) - Eored(anode)
Inorganic chemistry Assistance Lecturer Amjad Ahmed Jumaa  Predicting whether a (redox) reaction is spontaneous.  Calculating (ΔG°)
 Anything that uses batteries: › Cell phones › Game boys › Flash lights › Cars  Jewelry—electroplating.
Redox Reactions and Electrochemistry Chapter 19. Cell Potentials E cell  = E red  (cathode) − E red  (anode) = V − (−0.76 V) = V.
Electrochemistry Part Four. CHEMICAL CHANGE  ELECTRIC CURRENT To obtain a useful current, we separate the oxidizing and reducing agents so that electron.
CHAPTER 17 ELECTROCHEMISTRY. Oxidation and Reduction (Redox) Electrons are transferred Spontaneous redox rxns can transfer energy Electrons (electricity)
Chapter 20: Electrochemistry. © 2009, Prentice-Hall, Inc. Electrochemical Reactions In electrochemical reactions, electrons are transferred from one species.
Electrochemistry Hope you get a charge out of this one!!!!
Electrochemistry Terminology  Oxidation  Oxidation – A process in which an element attains a more positive oxidation state Na(s)  Na + + e -  Reduction.
Electrochemistry. Voltaic Cell (or Galvanic Cell) The energy released in a spontaneous redox reaction can be used to perform electrical work. A voltaic.
Electrochemistry.
Dr. Aisha Moubaraki CHEM 202
Electrochemistry the study of the interchange of chemical and electrical energy.
Chapter 19 Electrochemistry Semester 1/2009 Ref: 19.2 Galvanic Cells
Electrochemistry.
Electrochemistry.
Electrochemistry.
Electrochemistry Chapter 17.
From Voltage Cells to Nernst Equation
Electrochemistry.
Ch. 17 Electrochemistry.
Galvanic Cells Assignment # 17.1.
Presentation transcript:

Unit 10 - Chpt 18 - Electrochemistry Balance Redox equations HW set1: Chpt 18 - pg # 30, 32 - Due Tues. Apr 20 HW set2: Chpt 18 - pg # 40, 44, 50, 54, 60, 65, 74 - Due Fri. Apr 23

Workbook Lesson pkt Lesson 13 - Formal Oxidation number assignments - with examples and homework Lesson 28 - Balancing Redox Reactions with examples and homework

Sect (slides provided)

Galvanic Cell schematic Oxidation occurs at anode (vowels) Reduction occurs at cathode (consonants) Oxidation produces electrons, so current flows from anode to cathode.

Types of cells Standard Hydrogen cell platinum electrode metal electrodes

Cell Potential & Nernst Equation Galvanic Cell Potentials - free energy G o = -nFE o F is Faraday constant C/mol e- n = moles of e- from balanced Redox eqn Concentration Cell Potentials G = G o + RTlnQ or K if E cell = 0

Cell Potential & Nernst Equation G = G o + RT ln Q -nFE = -nFE o +RT ln Q E = E o - RT/nF ln Q E = E o /n log Q So E of a cell with concentrations not equal to 1 M is the std cell potential with the correction remember to know electrons transferred in Redox

Equilibrium, K constant E = E o - RT/nF log Q At equilibrium E cell = 0 and Q = K 0 = E o /n log K log K = nE o /

K example Example pg 841

Battery - Dry Cell

Feedback: Privacy Policy Feedback
Do Not Sell My Personal Information
About project: SlidePlayer Terms of Service

© 2025 SlidePlayer.com. Inc. All rights reserved.