Electrochemistry Lesson 8 Electrochemical Cells. Electrochemical cells are Batteries.

Slides:

Advertisements

Similar presentations

Experiment #10 Electrochemical Cell.

Advertisements

Electricity from Chemical Reactions

Electrochemistry Chapter 20.

Unit 11- Redox and Electrochemistry

Topic: Electrochemical Cells Do Now: 5 color pencils.

Oxidation Reduction Reactions

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.

Electrolytic Cells Lesson 8 Electrolytic Cells ELECTROLYSIS Electrolysis is a method of using a direct electric current (DC) to drive an otherwise non-

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

Aim: What are electrochemical cells?

Electrochemistry Chapter 19.

Electrochemistry Lesson 6 Electrochemical Cells.

Electrochemistry Electrochemical Cell – an apparatus that uses redox reactions to produce electrical energy. Voltaic Cell – a type of electrochemical cell.

ELECTROCHEMICAL CELLS. TASK Sequence these elements starting from the most reactive to the least reactive: Na, Pt, Au, C, H, Sn, Pb, Al, C, Mg, Li, Ca,

Electrochemistry. Electrochemical Cells  Electrons are transferred between the particles being oxidized and reduced  Two types –Spontaneous = Voltaic.

Notes on Electrolytic Cells An electrolytic cell is a system of two inert (nonreactive) electrodes (C or Pt) and an electrolyte connected to a power supply.

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

An Introduction to Electroanalytical Chemistry Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of.

GALVANIC AND ELECTROLYTIC CELLS

ELECTROCHEMICAL CELLS

Electrochemistry.

Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.

JUST REMEMBER... “OIL RIG” (oxidation is losing, reduction is gaining)

Electrolytic Cells Lesson 9 Electrolytic Cells. Notes on Electrolytic Cells An electrolytic cell is a system of two inert (nonreactive) electrodes (C.

Unit 14: ElectrochemLPChem: Wz. Unit 14: Electrochemistry.

Chapter 26 – Electricity from Chemical Reactions.

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

ELECTROCHEMICAL CELLS In redox reactions, there is a chemical reaction and an exchange of electrons between the particles being oxidized and reduced. An.

REDOX Part 2 - Electrochemistry Text Ch. 9 and 10.

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

Electric energy Chemical energy Electrolysis Galvanic cell Chapter 8 Electrochemistry.

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

Voltaic Cells/Galvanic Cells and Batteries. Background Information Electricity is the movement of electrons, and batteries are an important source of.

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

In the previous videos, we looked at electrochemical cells with reactive metal electrodes and solutions containing their cations. However, some electrochemical.

Galvanic Cells ELECTROCHEMISTRY/CHEMICAL REACTIONS SCH4C/SCH3U.

Electrochemistry. Electrochemistry is the study of the relationship between the flow of electric current and chemical changes, including the conversion.

Title: Lesson 6 Electrolytic Cells Learning Objectives: – Describe electrolytic cells – Identify at which electrode oxidation and reduction takes place.

Electrochemical cells - batteries

Electrolytic Cells Section 9.2. Vocabulary Electrolysis: electrical energy used to bring about a non-spontaneous redox reaction Electrolyte: any substance.

9.2 Electrochemical cells. Two types of electrochemical cells Voltaic cell Spontaneous Chemical  Electrical Uses activity differences between two metals.

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

1 UNIT 7 Reduction / Oxidation Reactions “Redox” and Electrochemistry.

CE Chemistry Module 8. A. Involves electron changes (can tell by change in charge) Cl NaBr 2NaCl + Br 2 B. Oxidation 1. First used.

Chapter 20: Electrochemistry. © 2009, Prentice-Hall, Inc. Electrochemical Reactions In electrochemical reactions, electrons are transferred from one species.

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

Redox 21-3 Electrochemistry. 1.) Electrochemical Cells A.) Also called Galvanic Cells B.) Conservation of mass, charge and energy C.) Changes Chemical.

9.2 Electrochemical Cells

Chapter 21 Electrochemistry. Voltaic Cells  Electrochemical cells used to convert chemical energy into electrical energy  Produced by spontaneous redox.

ELECTROCHEMISTRY Presentation by: P.K. CHOURASIA K.V MANDLA, Jabalpur Region.

Electrochemistry Chapter 18. Electrochemistry –the branch of chemistry that studies the electricity- related application of oxidation-reduction reactions.

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.

General Chemistry Unit 14. A. Involves electron changes (can tell by change in charge) Cl NaBr 2NaCl + Br 2 B. Oxidation 1. First.

Notes on Electrolytic Cells

Chemistry AS – Redox reactions

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

Electrochemical cells

Electrochemistry / Redox

Harnessing the changes in oxidation and reduction

10.2 Electrochemistry Objectives S2

Unit 8: Electrochemistry Applications

An electrolytic cell uses electricity to do a chemical reaction.

Electrochemistry i.e. This is the End!.

Electrochemistry Oxidation-Reduction

Electrochemistry.

from a battery or other external energy source

Electrochemistry Kenneth E. Schnobrich.

What is a redox reaction?

Presentation transcript:

Electrochemistry Lesson 8 Electrochemical Cells

Electrochemical cells are Batteries

Alkaline Batteries KOH

Car Batteries Pb-Acid H 2 SO 4

Mitsubishi iMiEV - Pure Electric Car Powered by a 330 v Li-Ion Rechargeable battery Plugs into your house and takes 14 hours to charge -100 km for $ 0.60 $ 50,000 Can $ 36,000 US Top Speed 130 km/h 63 hp and 133 lb.-ft. of torque

Cell Phone batteries Lithium Ion Rechargeable battery

Lithium Coin Cell

Space Ship Batteries Powered by Radioisotopes

Ni-Metal Hydride

Notes on Electrochemical Cells An electrochemical cell – a system of electrodes, electrolytes, and salt bridge that allow oxidation and reduction reactions to occur and electrons to flow through an external circuit. The salt bridge allows ions to migrate from one half-cell to the other without allowing the solutions to mix. 1.Spontaneous redox reaction 2.Produces electricity from chemicals 3.Is commonly called a battery

Analyzing Electrochemical Cells The reaction that is higher on the reduction chart is the reduction and the lower is oxidation and is written in reverse.

For any cell Oxidation always occurs at the anode and reduction at the cathode Electrons flow through the wire and go from anode to cathode Anions (- ions) migrate to the anode and cations (+ions) migrate towards the cathode usually through the salt bridge

voltmeter 1. Draw and completely analyze a Cu/Sn electrochemical cell. Higher Greatest Electron Affinity Reduction Cathode Cu e - → Cu (s) 0.34 v Gains mass + Cu Sn Cu 2+ NO 3 - Sn 2+ NO 3 - Na -+ NO v Lower Oxidation Anode Sn (s) → Sn e v Loses mass - Overall Reaction: Cu 2+ + Sn → Sn 2+ + Cu (s) 0.48 v e-e- e-e-

The Hydrogen half cell involves a gas and requires an inert or nonreactive Pt electrode. H 2(g) in Wire to circuit Pt (s) 1 M HCl H + Cl -

1.0 M KNO v Ag H2H2 voltmeter 2e - H + Cl - Ag + NO 3 - NO 3 - K + 2Ag + + H 2 → 2Ag + 2H v Draw a H 2 /Ag electrochemical cell with a KNO 3 salt bridge. Higher Greater electron affinity Reduction Cathode + Ag + + 1e - → Ag (s) v Gains mass oxidation Anode - H 2 → 2H + + 2e v pH decreases 1 M HCl 1 M AgNO 3 Pt