Aim # 36: What is the difference between a

Slides:

Advertisements

Similar presentations

Created by C. Ippolito March 2007 Updated March 2007 Chapter 22 Electrochemistry Objectives: 1.describe how an electrolytic cell works 2.describe how galvanic.

Advertisements

(c) 2006, Mark Rosengarten Voltaic Cells  Produce electrical current using a spontaneous redox reaction  Used to make batteries!batteries  Materials.

Cells and Voltage.

Oxidation-Reduction Reactions

Oxidation-Reduction Reactions LEO SAYS GER. Oxidation and Reduction (Redox)  Electrons are transferred  Spontaneous redox rxns can transfer energy 

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

Electrolytic Cell and Electroplating Chapter 19 Page Chem 12.

What does this?. Have to do with this? NOTHING!!!

ELECTROLYSIS. Compare and contrast voltaic (galvanic) and electrolytic cells Explain the operation of an electrolytic cell at the visual, particulate.

Redox: Oxidation and Reduction Definitions Oxidation: loss of e- in an atom increase in oxidation number (ex: -1  0 or +1  +2)  Reduction: gain of.

Aim Redox 1 – Why is redox so important in your life?

Topic: Electrolytic Cell Do now: p.19 in packet, cross out # 19 and do # 20 and #21. must label anode/cathode.

Chapter 22 REDOX.

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.

Explain the process of electrolysis and its uses

ELECTROCHEMICAL CELLS

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)

Electrochemical & Electrolytic Cells Using Redox Reactions in everyday life.

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

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.

Chapter  Electrochemistry occurs through the use of spontaneous redox reactions.

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

Corrosion of Iron Since E  red (Fe 2+ ) < E  red (O 2 ) iron can be oxidized by oxygen. Cathode: O 2 (g) + 4H + (aq) + 4e -  2H 2 O(l). Anode: Fe(s)

Electrolytic Cells Chemistry Chapter 19 E.

Electrolytic Cells. An electrolytic cell is an electrochemical cell that undergoes a redox reaction when electrical energy is applied. It is most often.

Electrolytic Cells utilizes electrical energy to create chemical energy.

Topic 19 Oxidation and Reduction. 1)What is the oxidation number of P in PO 4 -3 ? 2)If Cu and Zn and connected, which is the anode? 3)What reaction (oxidation.

Electrochemistry f.

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

Electrolysis 2 Types of electrochemistry 1. Battery or Voltaic Cell – Purpose? 2. Electrolysis - forces a current through a cell to produce a chemical.

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.

Chapter  The electrochemical cells require the INPUT of energy rather than creating energy.

ELECTROCHEMISTRY Voltaic and Electrolytic Cells

Electrochemistry.

Oxidation-Reduction Reactions

Redox in Action: Voltaic cells

CHEMISTRY CHAPTER 19 LEO SAYS GER

Chapter 10.7 Electrolysis.

Electrolytic Cells.

Electrochemistry and The Chemical Cells.

Chapter A2 A2.5 – Electrolytic Cells.

H.W. # 24 Study pp (sec ) Ans. ques. p. 883 # 93a,95c,97,104,105,

Chemistry AS – Redox reactions

Standard Cells & Cell Potential

Chapter 21: Electrochemistry

Oxidation-Reduction Reactions

Electrochemistry the study of the interchange of chemical and electrical energy.

Corrosion Corrosion of Iron

Electrolytic Cells Aim: Write half reactions for electrolysis of a salt and electroplating.

Chapter 10 Electrolytic Cells 10.7.

1. Introduction to Electrochemical Cells

10.2 Electrochemistry Objectives S2

Chemistry 21.3.

Electrochemistry.

Reduction - Oxidation Chapters

Chapter 10 ELECTROLYTIC CELLS 10.7.

Chemistry/Physical Setting

Electrolytic Cell Involves non spontaneous redox reactions

An electrolytic cell uses electricity to do a chemical reaction.

Redox & Electrochemistry.

Oxidation-Reduction Reactions

Electrochemistry.

from a battery or other external energy source

A. Oxidation-Reduction Reactions

Today’s assignment is: Quiz/ test is on Tuesday!!!

Redox in Electrochemistry

Presentation transcript:

Aim # 36: What is the difference between a Aim # 36: What is the difference between a voltaic cell and an electrolytic cell? H. W. # 36 Study class notes Study pp. 599-600 Ans. ques. p. 604 # 39-42

I Electrolytic Cell- a device used to produce a redox reaction by supplying an electric current to an aqueous solution of an electrolyte. An electrolytic cell has 3 essential parts: A source of direct current that provides the energy that causes the reaction to occur- a battery or a dry cell. Two electrodes- an anode(+) and a cathode(-). An electrolyte- a substance dissolved in water that provides ions, thus balancing the flow of electrons in the external circuit.

The process by which an electric current At the Ag electrode (anode) Ag(s) → Ag+(aq) + e- At the Mg electrode (cathode) Ag+(aq) + e- → Ag(s) The process by which an electric current causes a redox reaction in the water solution of an electrolyte is called electrolysis.

II A. Electroplating- the use of electrolysis to coat a material with a layer of metal. For electroplating to occur, the object to be plated must be a conductor.

B. Electrolysis– the production of hydrogen and oxygen from water.

III Practical applications of electrolysis Electroplating Recovery of active nonmetals (O2, H2, Cl2) Recharging a battery