'Cell potential' diaporamas de présentation

Electrochemistry

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Electrochemistry

Electrochemistry. Lincoln High School. Version 1.04 Updated February 27, 2009. 1. Electrochemistry. Electrochemistry is the study of chemical reactions that generate electrical effects and of the chemical reactions that are caused by the action of an electrical current or applied potential.

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Electrochemistry

Electrochemistry. KC. Version 1.04 Updated February 27, 2009. 1. Electrochemistry. Electrochemistry is the study of chemical reactions that generate electrical effects and of the chemical reactions that are caused by the action of an electrical current or applied potential. 2.

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Chemistry 142 Chapter 18: Electrochemistry

Chemistry 142 Chapter 18: Electrochemistry. Outline Oxidation-Reduction Reactions Voltaic (or Galvanic) Cells Electrolysis Corrosion. Electric Current Flowing Directly Between Atoms. Electric Current Flowing Indirectly Between Atoms.

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ELECTROCHEMISTRY Chapter 18

ELECTROCHEMISTRY Chapter 18. Introduction. * Electrochemistry : the study of the relationship between electron flow and redox reactions. Significance and Applications?

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HCM INTERNATIONAL UNIVERSITY SCHOOL OF BIOTECHNOLOGY

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Chemistry 232

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Electrochemistry

Electrochemistry. Chapter 17. Electron Transfer Reactions. Electron transfer reactions are oxidation-reduction or redox reactions. Results in the generation of an electric current (electricity) or be caused by imposing an electric current.

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CELL POTENTIAL, E

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A.P. Chemistry

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Oxidation-Reduction

Oxidation-Reduction. Larry J. Scheffler Lincoln High School. LEO . LEO says. GER!. GER!. LEO says. L oss of Electrons = Oxidation Gain of Electrons = R eduction. Oxidation Numbers. Oxidation is the loss of electrons; Reduction is the gain of electrons

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Electrochemistry Generating Voltage (Potential)

Electrochemistry Generating Voltage (Potential). Historically. Historically oxidation involved reaction with O 2 . i.e., Rusting 4 Fe (s) + 3O 2 (g) ?? Fe 2 O 3 (s) Other example Zn (s) + Cu 2+ (aq) g Zn 2+ (aq) + Cu (s) In this reaction:

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Electrochemistry

Electrochemistry. Chapter 18, 19-20. Electrochemical processes are oxidation-reduction reactions in which: the energy released by a spontaneous reaction is converted to electricity or electrical energy is used to cause a nonspontaneous reaction to occur.

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Electrolytic Cells

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ELECTROCHEMISTRY

ELECTROCHEMISTRY. Prepared by: Mr.P.L.Meena. What is electrochemistry ?.

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Electrochemistry

Electrochemistry. Terminology. You may have noticed oxygen never gets oxidized, it always gets reduced. The reason for this is because oxygen is an oxidizing agent . An oxidizing agent is something that causes something else to be oxidized.

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Dependence of cell potential on concentrations

Dependence of cell potential on concentrations. Lab 10. Outline. Purpose Electrochemistry Galvanic Cells Cell Potentials Standard Reduction Potentials The Nernst Equation Graphical Nernstian Response Procedure Safety Concerns Waste Next Lab Reminder. Purpose .

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Standard Reference Electrode Standard Hydrogen Electrode (SHE)

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ELECTROCHEMISTRY Chap 20

ELECTROCHEMISTRY Chap 20. Nernst Equation for a Complete Reaction. E cell = E + − E − = E cathode − E anode. Only valid when both ½-rxns written as reductions. Given: Cd ( s ) │ Cd(NO 3 ) 2 ( aq ); M A ║ FeCl 2 (aq); M C │ Fe ( s)

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1 st you need the BALANCED EQUATION

1 st you need the BALANCED EQUATION. Pb 2+ + 2 e- ?Pb (s) E 0 red = -0.13 V Cu 2+ + 2 e- ?Cu (s) E 0 red = 0.34 V You need an OXIDATION and a REDUCTION. E 0 cell >0 or nothing happens!. 1 st you need the BALANCED EQUATION. Pb (s) ? Pb 2+ + 2 e- E 0 ox = + 0.13 V

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