'Standard cell potential' diaporamas de présentation

Electrochemistry

Electrochemistry. Unit 14. Overview. Oxidation States Oxidation versus Reduction Redox reactions Identifying Half Reactions Balancing Voltaic (Galvanic) Cells Cell potential Standard reduction potentials Standard hydrogen electrode. Strength of Agents Nernst Equation Calculations

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Chemistry 232

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Introduction to Electrochemistry

CHAPTER. 18. Introduction to Electrochemistry. Oxidation ????? Reduction ????? Reducing agent : ??? ??????????????? Oxidizing agent ???? ???????????????.

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RedOx Chemistry

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RedOx Chemistry

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Some more advanced redox problems

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Some more advanced redox problems

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Electrochemical Equilibria

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Electrochemistry

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Electrochemical Cells

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Electrochemistry Lesson 7 The Standard Hydrogen Cell

Electrochemistry Lesson 7 The Standard Hydrogen Cell. The Standard Hydrogen Half Cell The zero point of the reduction chart is the hydrogen half-cell. E is the cell potential or voltage E 0 is the standard cell potential @ 25 o C solutions are 1.0 M gases are 101 KPa.

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ELECTROCHEMISTRY

ELECTROCHEMISTRY. Electrical and Chemical Energy Interconversion. REDOX REACTION. Reduction Oxidation Reducing Agent Oxidizing Agent. ELECTRICAL CONDUCTION. Electrons Conducting medium e lectron transfer (flow) conductance (mho) Resistance (ohm). Electrochemical Cell. e -. V. Zn.

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Electrochemistry

Electrochemistry. Redox reactions. Write the balanced equation for the reaction of permanganate and oxalate in acidic solution. MnO 4 - + C 2 O 4 2- ? Mn 2+ + CO 2 1. Find oxidation numbers. Permanganate & oxalate. Separate into half reactions

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Midterm Exam 1: Feb. 2, 1:00-2:10 PM at Toldo building, Room 100

Midterm Exam 1: Feb. 2, 1:00-2:10 PM at Toldo building, Room 100. Example: Calculate emf of the cell : Mn(s)|Mn +2 ||Fe +3 , Fe +2 |Pt(s) Solution: The two reduction half reactions Right (cathode): Fe +3 (aq) + e - ? Fe +2 (aq) Left (anode): Mn +2 (aq) + 2e - ? Mn(s)

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Potentiometry and the Detection of Fluoride

Potentiometry and the Detection of Fluoride . pH Meter. pH meters use a ion selective glass electrode: Thin glass membrane connects sample with a reference solution Glass membrane typically made of silica Potential difference builds across membrane

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Electrochemistry

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Voltaic Cells

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Electrochemistry

Electrochemistry. Kristin Shepard Brooke Petersen. Electrochemical Cells- Terms. Electrode - Any cell that is used to conduct electricity; Where the reaction actually takes place- Solid Part Anode - Solid where the oxidizing happens Cathode - Solid where the reduction occurs

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Electrochemical Cells (continued):

Standard cell potential. Standard oxidation potential. Standard reduction potential. = +. Electrochemical Cells (continued):. Calculating Cell Voltages.

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