Making Galvanic Cells Lab 3)The salt bridge allows the cell to continue to function. K + or NO 3 – can move into one of the half cells to balance the charge.

Slides:

Advertisements

Similar presentations

Types of cells – – – Overview Cells are containers of liquid with electrodes: In electrolytic cells, electricity is used to force chemicals to.

Advertisements

Electrochemical & Voltaic Cells

Electrochemistry. Remember… Anode: electrode in the half-cell where oxidation takes place Metal electrode atoms are oxidized and become aqueous ions Anions.

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.

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)

Lecture 11: Electrochemistry Introduction

Electrochemical Cells (Batteries) Chemical reaction produces electricity. Called “voltaic cells” Happens SPONTANEOUSLY.

Electrochemistry The study of chemical reactions that produce electrical current or are driven to occur by applying an electrical current. Chemical potential.

Electrolytic cell: Converts electrical energy to chemical energy. Electrolysis – Electrolytic Cell Copper chloride CuCl Cu 2+ Cl - Cu 2+ (aq) +

Redox Half Reactions What is the purpose of creating a half reaction? How to balance a half reaction?

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

Electrochemistry A lemon can power a small light bulb. Where does the energy come from? RedOx reactions move electrons from one element to another.

 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.

III.Electrochemical Cells: (ie: Batteries or Galvanic Cells)  Redox reactions that take place in such a way that electrical energy (or voltage) is produced,

CONTENT OBJECTIVE make qualitative or quantitative predictions about galvanic (voltaic) cells based on half-cell reactions and potentials and analyze these.

Voltaic/Galvanic Cells. Voltaic Cells In spontaneous oxidation-reduction (redox) reactions, electrons are transferred and energy is released.

Presented by Azra Goher

Electrochemistry - Section 1 Voltaic Cells

Topic: Redox Aim: What are electrochemical cells? Do Now: Which of the following ions is most easily reduced? 1)Li+ 2) K+ 3) Ca 2+ 4) Na+ HW:

5.7 Galvanic Cell Leo Ger “Lose electron  oxidation” Zn  2e - + Zn 2+ “Gain electron  reduction” 2e - + Cu 2+  Cu My name is Leo. Grr-rrrr…

Electrolysis Chapter 17 Section 7 Electrochemistry e-

Electrolysis. In a galvanic cell, a redox reaction occurs to produce electricity. In an electrolytic cell, electricity is used to produce a redox reaction.

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

Batteries Electrochemical cells  Terms to know Anode Cathode Oxidation Reduction Salt Bridge Half cell Cell potential Electron flow Voltage.

Oxidation and Reduction Chapters 20 & 21. Oxidation vs Reduction.

Chapter 19 Redox Reactions.

Galvanic Cells ELECTROCHEMISTRY/CHEMICAL REACTIONS SCH4C/SCH3U.

Principles and application

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

 Anything that uses batteries: › Cell phones › Game boys › Flash lights › Cars  Jewelry—electroplating.

Electrochemistry Ch. 18 Electrochemistry 18.1 Voltaic Cells.

1 © 2006 Brooks/Cole - Thomson OXIDATION-REDUCTION REACTIONS Indirect Redox Reaction A battery functions by transferring electrons through an external.

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

1 REVERSIBLE ELECTROCHEMISTRY 1. Voltaic Or Galvanic Cells Voltaic or Galvanic cells are electrochemical cells in which spontaneous oxidation- reduction.

Oxidation-Reduction (aka Redox) Reactions These are electron- transfer reactions! om/ICT/rr/redox1.html.

Voltaic Cells Notes A.) Spontaneous reaction 1.) In Voltaic Cells (Batteries), when the circuit is closed (turned on) electrons will move from anode.

Electro-chemistry: Batteries and plating Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of electrons.

Electrolysis 3.7 Electrolysis…. Electrolysis Use of electrical energy to produce chemical change...forcing a current through a cell to produce a chemical.

ELECTROCHEMISTRY is the branch of chemistry which deals with…

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

You will have to completely label a diagram to look like this

Chapter 20 Electrochemistry

To be viewed with PowerPoint. Animation doesn’t work otherwise.

Electrochemistry The batteries we use to power portable computers and other electronic devices all rely on redox reactions to generate an electric current.

Voltaic Cells Aim: To identify the components and explain the functions of an electrochemical (voltaic) cell.

Chp 17 Electrochemistry.

14.2a Voltaic Cells Basic Function.

Types of cells.

Electrochemistry / Redox

Harnessing the changes in oxidation and reduction

10.2 Electrochemistry Objectives S2

Reduction - Oxidation Chapters

Making Galvanic Cells Lab

You will have to completely label a diagram to look like this

Introduction to Electrochemistry

Types of cells.

Electrochemistry Lesson 3

Electrochemical Cells (Batteries)

AP Chem Get HW checked Work on oxidation # review

Chapter 21: Electrochemistry

AP Chem Get HW checked Take out laptops and go to bit.ly/GalCell

Write the oxidation half reaction for lithium oxidizing

Redox and Electrochemistry

Redox and Electrochemistry

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

Electrochemistry Kenneth E. Schnobrich.

Electrochemistry Lesson 1 Introduction.

Presentation transcript:

Making Galvanic Cells Lab 3)The salt bridge allows the cell to continue to function. K + or NO 3 – can move into one of the half cells to balance the charge created by + metal ions forming or leaving solution. 4)No. We did not get the same values in the lab No bridgeVoltagePoints toDeposit Cu – Al 0 V2.0 VCu Cu – Zn 0 V1.1 VCu Al – Zn 0 V0.9 VZn

Cu – Zn cell Zn Zn e – (oxidation - LEO) Cu e – Cu (reduction - GER) Cu 2+ + Zn Cu + Zn 2+ Electron flow Salt bridgeCu (+) Zn (–) Cu 2+ Zn 2+

Al – Zn cell Zn e – Zn (reduction - GER) Al Al e – (oxidation - LEO) 2Al + 3Zn 2+ 2Al Zn Electron flow Salt bridgeZn (+) Al (–) Zn 2+ Al 3+

Making Galvanic Cells Lab AlDepositCuDeposit AlPoints toCuPoints to sec sec sec sec 0No bridge0 voltageAl-ZnvoltageCu-Zn 3)The salt bridge allows the cell to continue to function. K + or NO 3 – can move into one of the half cells to balance the charge created by + metal ions forming or leaving solution. 4)No. We did not get the same values in the lab For more lessons, visit