Lecture 243/14/06. Balancing Redox reactions H 2 C 2 O 4 (aq) + MnO 4 -  Mn 2+ + CO 2 (g) oxalic acid permanganate 1. Break into half-reactions 2. Balance.

Slides:

Advertisements

Similar presentations

MS FARZANA MEHBOOB D.A.NEELUM HIGH SCHOOL

Advertisements

Chapter 20 Electrochemistry

Galvanic (= voltaic) Cells Redox reactions which occur spontaneously are called galvanic reactions. Zn will dissolve in a solution of copper(II) sulfate.

Electrochemical Cells

Cells and Voltage.

Cells and Voltage.

Galvanic Cells What will happen if a piece of Zn metal is immersed in a CuSO 4 solution? A spontaneous redox reaction occurs: Zn (s) + Cu 2 + (aq) Zn 2.

Electrochemical Cells. Definitions Voltaic cell (battery): An electrochemical cell or group of cells in which a product-favored redox reaction is used.

Electrochemistry I. Electrochemistry Half-Reactions and Electrochemical Cells Voltaic Cells: Using Spontaneous Reactions to Generate ElectricalEnergy.

Lecture 253/27/06 Bottle and Can drive today 11-3 Hagan Info Booth Seminar today at 4 pm.

Chapter 18 Electrochemistry. Redox Reaction Elements change oxidation number  e.g., single displacement, and combustion, some synthesis and decomposition.

Lecture 263/30/07. E° F 2 (g) + 2e - ↔ 2F Ag + + e - ↔ Ag (s)+0.80 Cu e - ↔ Cu (s)+0.34 Zn e - ↔ Zn (s)-0.76 Quiz 1. Consider these.

Lecture 233/12/06. What is a REDOX reaction? OXIDATION: Ca(s)  Ca 2+ REDUCTION: 2H +  H 2 (g) OIL RIG Combined (net): REDOX REACTIONS Oxidation-Reduction.

Prentice Hall © 2003Chapter 20 Zn added to HCl yields the spontaneous reaction Zn(s) + 2H + (aq)  Zn 2+ (aq) + H 2 (g). The oxidation number of Zn has.

Lecture 223/19/07. Displacement reactions Some metals react with acids to produce salts and H 2 gas Balance the following displacement reaction: Zn (s)

Electrochemistry Use of spontaneous chemical reactions to produce electricity; use of electricity to drive non-spontaneous reactions. Zn(s) + Cu 2+ (aq)

Chapter 20 Electrochemistry

Lecture 11: Electrochemistry Introduction

Lecture 233/30/05. Redox example: respiration/combustion Balance redox reaction for glucose (C 6 H 12 O 6 ) respiration (same as combustion reaction)

Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Electrochemistry TEXT REFERENCE Masterton and Hurley Chapter 18.

Electrochemistry Chapter 19.

Section 18.1 Electron Transfer Reactions 1.To learn about metal-nonmetal oxidation–reduction reactions 2.To learn to assign oxidation states Objectives.

Electrochemistry Chapter 21. Electrochemistry and Redox Oxidation-reduction:“Redox” Electrochemistry: study of the interchange between chemical change.

Chapter 21: Electrochemistry I Chemical Change and Electrical Work 21.1 Half-Reactions and Electrochemical Cells 21.2 Voltaic Cells: Using Spontaneous.

Oxidation and Reduction

Electrochemistry Experiment 12. Oxidation – Reduction Reactions Consider the reaction of Copper wire and AgNO 3 (aq) AgNO 3 (aq) Ag(s) Cu(s)

Principles of Reactivity: Electron Transfer Reactions Chapter 20.

Redox Reactions Year 11 Chemistry ~ Unit 2.

Electrochemistry Chapter 20 Brown-LeMay. Review of Redox Reactions Oxidation - refers to the loss of electrons by a molecule, atom or ion - LEO goes Reduction.

17-Nov-97Electrochemistry (Ch. 21)1 ELECTROCHEMISTRY Chapter 21 Electric automobile redox reactions electrochemical cells electrode processes construction.

Oxidation & Reduction Electrochemistry BLB 11 th Chapters 4, 20.

14.2a Voltaic Cells Basic Function. Voltaic Cell Basics Electrodes and electrolytes chemically react to form ions that move in or out of solution. Anode.

CHM 112 Summer 2007 M. Prushan Chapter 18 Electrochemistry.

1 ELECTROCHEMISTRYELECTROCHEMISTRY Redox reactions results in the generation of an electric current (electricity).Redox reactions results in the generation.

Electrochemistry. Electron Transfer Reactions Electron transfer reactions are oxidation- reduction or redox reactions. Electron transfer reactions are.

Electrochemical Cells - producing an electric current with a redox reaction.

Chapter 18 Notes1 Chapter 18 Electrochemistry 1. review of terms; balancing redox equations 2. galvanic cell notation, relationships 3. standard reduction.

 Learners must be able to define galvanic cell in terms of electrode reaction. e.g. salt bridge.(N.B. anode and cathode)  Learners must be able to do.

Electrochemical Cells (Galvanic, Voltaic, Electric)

1 AnodeCathode Basic Concepts of Electrochemical Cells.

Electrochemistry - Section 1 Voltaic Cells

Electrochemistry ZnSO4(aq) CuSO4(aq) Cu Zn Zn

Chapter 20 Electrochemistry West Valley High School General Chemistry Mr. Mata.

Electrochemistry Ch.19 & 20 Using chemical reactions to produce electricity.

Reduction- Oxidation Reactions (1) 213 PHC 9 th lecture Dr. mona alshehri (1) Gary D. Christian, Analytical Chemistry, 6 th edition. 1.

Electrochemical cells - batteries

Chem Catalyst Determine what is being oxidized and what is being reduced in the following reaction: CuO + H 2  Cu + H 2 O.

ELECTROCHEMICAL CELLS. ELECTROCHEMISTRY The reason Redox reactions are so important is because they involve an exchange of electrons If we can find a.

10.3 Half-reactions and electrodes

Electrochemistry Ch. 18 Electrochemistry 18.1 Voltaic Cells.

Electrochemistry Introduction Voltaic Cells. Electrochemical Cell  Electrochemical device with 2 half-cells with electrodes and solutions  Electrode—metal.

Balancing Redox Equations – Voltaic (Galvanic) Cells.

Chapter 18 Electrochemistry Lesson 1. Electrochemistry 18.1Balancing Oxidation–Reduction Reactions 18.2 Galvanic Cells 18.3 Standard Reduction Potentials.

Electrochemistry Is the study of the interchange of chemical and electrical energy HW: Read CH 8 and 18 3 min

Redox Review. Create a Venn Diagram for Voltaic and Electrolytic cells.

Electrochemistry. To obtain a useful current, we separate the oxidation and reduction half-reactions so that electron transfer occurs thru an external.

Zn (s) + Cu2+ (aq)  Zn2+ (aq) + Cu (s)

Chapter 20 Electrochemistry

Ch. 19 Oxidation and Reduction

Electrochemical cells

14.2a Voltaic Cells Basic Function.

Electrochemistry / Redox

Electrochemistry.

HELP Balancing Redox Reactions 3 I2 (s) + Al (s)  2 2 AlI

Introduction to Electrochemistry

January 2018 Electrochemistry Chemistry 30.

Voltaic (Galvanic)Cells

HELP Balancing Redox Reactions 3 I2 (s) + Al (s)  2 2 AlI

Zn (s) + Cu2+ (aq)  Zn2+ (aq) + Cu (s)

Galvanic Cells Assignment # 17.1.

Presentation transcript:

Lecture 243/14/06

Balancing Redox reactions H 2 C 2 O 4 (aq) + MnO 4 -  Mn 2+ + CO 2 (g) oxalic acid permanganate 1. Break into half-reactions 2. Balance the atoms 3. Combine the half-reactions 4. Check for mass and charge balance

Redox example: respiration/combustion Balance redox reaction for glucose (C 6 H 12 O 6 ) respiration (same as combustion reaction) How do the oxidation numbers of carbon and oxygen change? What is being oxidized? What is being reduced? What is the oxidizing agent? The reducing agent?

Acid Mine Drainage FeS 2 (pyrite)

Redox under basic conditions: Balance the following redox reaction in a basic solution CrO SO 3 2-  Cr(OH) 3 + SO 4 2-

Displacement reactions Some metals react with acids to produce salts and H 2 gas Balance the following displacement reaction: Zn (s) + HBr (aq)  ZnBr 2 (aq) + H 2 (g)

Apparatus with oxidation and reduction reactions in different compartments Apparatus with oxidation and reduction reactions in different compartments redox reaction occurs by transferring electrons through an external connector redox reaction occurs by transferring electrons through an external connector voltaic or galvanic cell product favored reaction product favored reaction produces electric current produces electric current electrolytic cell reactant favored reaction reactant favored reaction external electric current used to drive reaction external electric current used to drive reaction Electrochemical cells

Voltaic (Galvanic) Cells Redox reaction must favor products Electrodes Anode: where oxidation occurs Cathode: where reduction occurs Salt bridge Need salt bridge or porous barrier in order to maintain charge balance in each compartment External circuit Wire to allow electrons to flow between electrodes