applied electrochemistry ppt
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Slide 6. 7. Electrolysis To determine the moles of electrons passed we measure the current and time that the current flows Charge (C) = Current (A) x Time (s) Because the charge on 1 mol of e- is 96 500 C the number of moles of e- passed through the cell is
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· Electrochemistry is the study of reactions in which charged particles (ions or electrons) cross the interface between two phases of matter typically a metallic phase (the electrode) and a conductive solution or electrolyte. A process of this kind can always be represented as a chemical reaction and is known generally as an electrode
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· Electrochemistry The study of the interchange of chemical and electrical energy Oxidation is the loss of electrons (Increase in charge). Reduction is the gain of electrons (Decrease in charge) Electrochemical Cells Galvanic Cells Produces electrical current spontaneous chemical reactions Battery 2. Electrolytic Cells Consumes electrical current
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· difference must be applied for the half cell reactions to occur. Two questions therefore arise • What is the voltage that we can obtain from a galvanic cell given specific anode and cathode materials • What is the voltage that needs to be applied in an electrowinning cell There are two approaches for determining the cell voltage.
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Slide 6. 7. Electrolysis To determine the moles of electrons passed we measure the current and time that the current flows Charge (C) = Current (A) x Time (s) Because the charge on 1 mol of e- is 96 500 C the number of moles of e- passed through the cell is
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· Electrochemistry Electrochemistry is that branch of chemistry which deals with the study of production of electricity from energy released during spontaneous chemical reactions and the use of electrical energy to bring about non-spontaneous chemical transformations. Importance of Electrochemistry 1. Production of metals like Na Mg. Ca and Al. 2.
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· • The greater the applied voltage the larger the resulting current flow and the greater the rate of the chemical reaction. ne-Q Oxidation or de-electronation. P = reductant (electron donor) Q = Product ne-B Reduction or electronation. A = oxidant (electron acceptor) B = Product In electrolysis we use an applied voltage • The rate at which
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· Occurs at both electrodes making oxidations more The reaction requiring the smallest applied Lets look at an example to determine if a Can Pb2 be quantitatively be separated from Cu2 Assume that our solution starts with 0.1M of Well define quantitative as only 1 part in 10. Chem 340 Fall 2013Lecture Notes 12- Electrochemistry (Chap.
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Electrochemistry. P. Madkour. SS902 ADVANCED ELECTROCHEMISTRY Murali Rangarajan Department of Chemical Engineering Amrita Vishwa Vidyapeetham Ettimadai 1 fELECTRODICS 2 f FARADAIC PROCESSES • Two types of processes take place at electrodeFaradaic ProcessesNon-Faradaic Processes • Faradaic processes involve electrochemical redox
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· Dr. Sapna Gupta/ElectrochemistryApplications 3. BATTERIES •A battery is a galvanic cell or a series of cells connected that can be used to deliver a self-contained source of direct electric current. •Dry Cells and Alkaline Batteries •no fluid components
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· Electrochemistry is the study of reactions in which charged particles (ions or electrons) cross the interface between two phases of matter typically a metallic phase (the electrode) and a conductive solution or electrolyte. A process of this kind can always be represented as a chemical reaction and is known generally as an electrode
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· Electrochemistry The study of the interchange of chemical and electrical energy Oxidation is the loss of electrons (Increase in charge). Reduction is the gain of electrons (Decrease in charge) Electrochemical Cells Galvanic Cells Produces electrical current spontaneous chemical reactions Battery 2. Electrolytic Cells Consumes electrical current
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· 5. Tying Electrochemistry to Thermodynamics. In electrochemistry the quantity in which we are most interested is E the potential energy of the system. It is the value you see on a new E = 1.5V or E = 6 V battery. We can relate this idea of work done in electrochemistry to the thermodynamic concept of work free energy through the equation
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Fundamentals of Electrochemistry CHEM 7234 / CHEM 720 Lecture 1 Course Overview Date Thurs 8 Fri 9 Mon 12 Tues 13 Wed 14 Thurs 15 Fri 16 Mon 19 Tues 20 Wed 21 Thurs A free PowerPoint PPT presentation (displayed as a Flash slide show) on PowerShowid 4d64f0-NGU0Z
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· now being applied throughout the field. The impact on industry of these developments has been impressive. Beneficial cross fertilization of ideas has occurred recently at an explosive rate. For example ion exchange membranes originally developed for fuel cells in space capsules have revolutionized chlor-alkali production. These same
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This presentation is all about acid base and salt of class 7 from cbse science book have the detailed explanation about concept of acid that is definition of acid types of acid and various examples of acid from day to day life.these concepts are very well explained with adequate examples and animated images. the examples are very well explained for each individual illustration.
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· Occurs at both electrodes making oxidations more The reaction requiring the smallest applied Lets look at an example to determine if a Can Pb2 be quantitatively be separated from Cu2 Assume that our solution starts with 0.1M of Well define quantitative as only 1 part in 10. Chem 340 Fall 2013Lecture Notes 12- Electrochemistry (Chap.
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View Electrochemistry2015.ppt from APPLIED SC MF101 at UCSI University Cheras. Electrochemistry Electrolysis Decomposition of substances by electrical current at the electrode. 1 Faraday (F) is the
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· Electrochemistry Notes Example Problems 1. Consider the galvanic cell based on the reaction Al3 Mg Al Mg2 The half reactions are Al e Al E V303 1.66 Mg e Mg E V202 2.37 Give the balanced cell reaction and calculate E0 for the cell. (See work on page 845) Solution 0.71 V 2. Using the data in Table 17.1 calculate the G for the reaction
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· Electrochemistry Electrochemistry is that branch of chemistry which deals with the study of production of electricity from energy released during spontaneous chemical reactions and the use of electrical energy to bring about non-spontaneous chemical transformations. Importance of Electrochemistry 1. Production of metals like Na Mg. Ca and Al. 2.
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· difference must be applied for the half cell reactions to occur. Two questions therefore arise • What is the voltage that we can obtain from a galvanic cell given specific anode and cathode materials • What is the voltage that needs to be applied in an electrowinning cell There are two approaches for determining the cell voltage.
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· Electrochemistry 2 • If we place MnO4-and Fe2 in the same container the electrons are transferred directly when the reactants collide. No useful work is obtained from the chemical energy involved which is instead released as heat
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· Occurs at both electrodes making oxidations more The reaction requiring the smallest applied Lets look at an example to determine if a Can Pb2 be quantitatively be separated from Cu2 Assume that our solution starts with 0.1M of Well define quantitative as only 1 part in 10. Chem 340 Fall 2013Lecture Notes 12- Electrochemistry (Chap.
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· Electrochemistry is the study of reactions in which charged particles (ions or electrons) cross the interface between two phases of matter typically a metallic phase (the electrode) and a conductive solution or electrolyte.
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