...Electrochemistry review: The Galvanic Cell Dion, D.A.,Franco, A.N., Jose, C.K., Jugno, C.A., Josol, S.G. Group 4-2B-Biochemistry, Department of Biochemistry, Faculty of Pharmacy, University of Sto. Tomas Abstract: In this experiment, we used dry cell battery. The two main objectives of the experiment are to (1) relate and apply the concepts of electrochemistry to actual experiments, (2) understand the processes and elements of an electrochemical cell and (3) determine the spontaneity of reduction-oxidation (redox) reactions based on standard reduction potential. Different half-cells were prepared and connected to copper, which served as the reference electrode, to set up a voltaic cell. The volt-meter readings of the set-ups were then used to calculate for the standard reduction potentials of the variable half-cells. The results obtained from the experiment indicated the spontaneity of the redox reactions investigated, showing that the least spontaneous system is that connected to another copper half- while the most spontaneous system is that connected to the Zinc half-cell. Introduction: Electrochemistry is the study of the relationships between chemical reactions and electricity. The functionality of every portable electronic device you own, whether it be your laptop, Ipod, or cell phone, is made possible by electrochemical reactions. Fundamental oxidation/reduction reactions occur inside the batteries of these devices. Chemists and engineers all over the world are...
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...By definition electrochemistry is the science that deals with the relation of electricity to chemical changes and with the inter-conversion of chemical and electrical energy (Definition of electrochemistry n.d.). The process of an electrochemical reaction is one which is either caused by the movement of current or a result of the movement of electrical current. This process is commonly known as a redox (oxidation-reduction) reaction (Conjecture Corporation 2014). In this process one atom/molecule gives off its electrons to another atom/molecule. The atoms/molecules reacting are relatively far from each other, this forces the electrons being transferred to move a larger distance thus producing and electrical current (Conjecture Corporation...
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...____________ [Chemistry 3] Experiment No 3.1 CORROSION K. M. U. AMANDORON, R. N. T. COLANAG, E. J. G. MERIN, F. T. OPADA, R. J. C. PARBA IV-Photon Philippine Science High School - Central Visayas Campus Talaytay, Argao, Cebu, Philippines Date performed: December _, 2013 Date submitted: January 6, 2013 ABSTRACT Corrosion is a process through which metals in manufactured states return to their natural oxidation states, a reduction-oxidation reaction in which the metal is being oxidized by its surroundings, often the oxygen in air [1]. The first part of the experiment involved the products of rusting. Certain amounts of 3% NaCl, 10% K3Fe(CN)6 and phenolphthalein were combined. A piece of paper was soaked in this mixture. 2 nails (one straight, one bent) were wrapped in the damp paper allowing space in between, then left for 10mins. After which, colors formed in the paper napkins were observed. The second part was the bimetallic corrosion. 2 iron nails were cleaned using sand paper. In one nail, copper wire was coiled around its tip. On the other, a zinc granule was attached to its tip. Another paper was soaked in the same mixture in which the nails were wrapped separately and were left for 10mins. The papers were opened and sites where pink and blue colors formed were examined. The results didn’t absolutely correspond to the objectives of this experiment due to the errors on the materials used; however, it was inferred that during the process...
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...Electrochemistry Electrochemistry is a branch of chemistry that studies chemical reactions which take place in a solution at the interface of an electron conductor (the electrode: a metal or a semiconductor) and an ionic conductor (the electrolyte). These reactions involve electron transfer between the electrode and the electrolyte or species in solution. If a chemical reaction is driven by an externally applied voltage, as in electrolysis, or if a voltage is created by a chemical reaction as in a battery, it is an electrochemical reaction. In contrast, chemical reactions where electrons are transferred between molecules are called oxidation-reduction (redox) reactions. In general, electrochemistry deals with situations where redox reactions are separated in space or time, connected by an external electric circuit. Principles Oxidation and reduction The term "redox" stands for reduction-oxidation. It refers to electrochemical processes involving electron transfer to or from a molecule or ion changing its oxidation state. This reaction can occur through the application of an external voltage or through the release of chemical energy. Oxidation and reduction describe the change of oxidation state that takes place in the atoms, ions or molecules involved in an electrochemical reaction. Formally, oxidation state is the hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic. An atom or ion that gives up an electron to another atom or...
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...written permission of the Publisher, or authorization through payment of the appropriate per-copy fee to the Copyright Clearance Center, 222 Rosewood Drive, Danvers, MA 01923, (978) 750-8400, fax (978) 750-4470. Requests to the Publisher for permission should be addressed to the Permissions Department, John Wiley & Sons, Inc., 605 Third Avenue, New York, NY 10158-0012, (212) 850-6011, fax (212) 850-6008, E-Mail: PERMREQ@WILEY.COM. To order books or for customer service, call 1 (800)-CALL-WILEY (225-5945). Library of Congress Cataloging in Publication Data: Bard, Allen J. Electrochemical methods : fundamentals and applications / Allen J. Bard, Larry R. Faulkner.— 2nd ed. p. cm. Includes index. ISBN 0-471-04372-9 (cloth : alk. paper) 1. Electrochemistry. I. Faulkner, Larry R., 1944- II. Title. QD553.B37 2000 541.3'7_dc21 00-038210 Printed in the United States of America 10 9 8 7 6 5 4 3 2 1 PREFACE In the twenty...
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...(A) Write a précis of the science article you have been assigned (150 words maximum) Eley’s article “Synthesis by Sunlight” (2013) asserts that US scientists would like both the organic and electrochemistry fields to work together to produce more sustainable and environmentally friendly reactions which are powered by sunlight. Scientists from Washington University are setting out to prove that chemical oxidations can be powered by sunlight with the aid of electrochemistry. In order to do this reaction, they connected a reaction flask and a photovoltaic cell together. When visible to sunbeams, the electricity produced allows the chemical oxidant to be regenerated at the positively charged electrode (anode). As a result, the scientists have...
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...Science fair during activity week Introduction This report investigates an activity done during the activity week which took place during the third week in June 2014. The science fair was held during the fourth day and this programme was initiated to demonstrate science related experiments to the students. The experiments were based on form 5 and form 4 practical books. The science fair was conducted by teachers from science department and was divided into three different subjects; physics, chemistry and biology. The objectives of the science fair are; 1. One of the programme during the activity week. 2. As a teaching platform to introduce physics, chemistry, and biology subject to lower secondary and for further understanding in the science subjects for upper secondary. 3. Demonstrate science related experiments based on practical books to students. 4. Introduction to laboratory rules and regulations, apparatus and materials. 5. Help students to relate and understand the science concept learned during class by observing and participating in the experiments Content 1.0 Physics 1.1 Topics 1.1.1 Introduction to physics In the experiments, students were introduced to several apparatus like Vernier caliper and Micrometer for measuring purposes. Students were showed on how to properly use the measuring instruments and how to take a measure using these instruments. 1.1.2 Force and Pressure The experiments were conducted for better understanding...
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...Application Assignment #3 – Equilibrium and Electrochemistry According to Chemicool chelation is the “formation or presence of bonds between two or more separate binding sites within the same ligand and a single central atom” (chemicool). Chelation therapy is a process in which reduction of toxic effects of metals within the human body take place. The agents often bind to the toxic ions and form structures that are then easily excreted. Most agents are made up of atoms like Sulphur, Nitrogen and Oxygen functioning as ligand atoms. As metals release toxic substances into the human body the need for an agent to try and reduce the toxicity for our well being is necessary. Most of the heavy are toxic such as lead, copper and zinc which accumulate in the human body. The process of chelation causes a chemical reaction involving a shift of equilibrium to remove the metals before the organs get permanently damaged. The shift in equilibrium occurs because when the agent is introduced to the body to try and reduce the effects, with the body being the system it tries to re-establish equilibrium by shifting from left to right. Barium sulphate is usually made by a combination of a solution of the ions and salts of barium and sulphate. Barium being a heavy metal is highly toxic. In colour it is a white solid with a crystal structure. The reason that Barium sulphate salt is used is that the ions of Barium are opaque to x-rays and can absorb the rays much better than other compounds. Without...
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...was of animal origin and could be found only in living tissues. A few years later, in 1800 Alessandro Volta discovered that electricity could be produced through inorganic means. In fact, by using small sheets of copper and zinc and cloth spacers soaked in an acid solution, he built a battery - the first apparatus capable of producing electricity. Naysayers were quick to predict that electricity would never serve a useful purpose. Obviously they were very wrong. Electricity has a central role in our lives and to this day Electrochemistry is a standard course of study. While listening to lessons on Electrochemistry, many students may wonder why it was ever invented, if it was really ever necessary to invent it and if the world would be better off without it. With the small experiments that follow, we hope to make peace between these students and the study of Electrochemistry. These fun and simple experiments can teach the fundamental concepts of Electrochemistry without asking much of the student. As you will see, many of these demonstrations are easily adapted to various configurations and each can be done independently or as part of the full curriculum. POROUS VASE - An actual porous vase made for the purpose may be difficult to acquire. It is used to prevent the quick mixing of various solutions, while permitting the exchange of ions. For our purposes you can adapt a terracotta pot of the type used in gardening simply by plugging the hole in the bottom with molten wax and...
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...REDUCTION REACTION Reduction is chemical reaction that involves the gaining of electrons. It refers to the side that accepts electrons. When iron reacts with oxygen it forms a chemical called rust. In that example, the iron is oxidized and the oxygen is reduced. Reduction is the opposite of oxidation. A reduction reaction always comes together with an oxidation reaction. Oxidation and reduction together are called redox. Oxidation is a gain of oxygen. Reduction is a loss of oxygen. For example: * Fe2O3 + 3CO → 2Fe + 3CO2 Both reduction and oxidation go on at the same time which is a redox-reaction. The gain of Hydrogen-atoms; and, the simultaneously loss of oxygen-atoms, is known as reduction. Oxidising agent is a chemical that releases oxygen atoms. For example, potassium chlorate has a chemical formula of KClO3. When it oxidizes a reducing agent, such as powdered aluminium metal, it loses its oxygen to the aluminium and becomes potassium chloride, KCl. It is also referred to as a chemical that accepts electrons from a reducing agent. For example, potassium permanganate has an oxidation state of +7. In acid solution, it gains 5 electrons (e-), becoming a manganese compound with an oxidation state of +2. Most oxidizing agents of the second (electron-accepting) definition have oxygen, but not all. For example, fluorine (F2), the most powerful oxidizing agent, does not have any oxygen in it. When it acts as an oxidizing agent, it gains an electron to...
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...CEM334: ELECTROCHEMISTRY Tutorial / Tutoriaal Summary of selected formulas from CEM334 electrochemistry. / Opsomming van geselekteerde formules van CEM334 elektrochemie Ecell = Ereduction potential of reduction halfreaction – Ereduction potential of oxidation halfreaction RT a (products) RT ln = E 0 (T ) − ln Q nF a (reactants) nF E (T ) = E 0 (T ) − ∆G = -nFEcell E 0 cell = RT ln K a nF ∂∆G ∂E ∆S = − = nF ∂T P ∂T P E − E1 ∆S = nF 2 T −T 1 P 2 E − E1 − E1 ∆H (T1 ) = ∆G + T1∆S = nF T1 2 T2 − T1 P ∂E ∆H = ∆G + T∆S = nF T − E ∂T P NOTE from above: R = gas constant, 8.314 J mol-1 K-1 F = Faraday constant, 96485 C ekw-1 ∂E ∆G = ∆H − T∆S = ∆H − nFT ∂T P YOU MUST KNOW THEM AND HOW TO USE THEM – NO FORMULA SHEET WILL BE PROVIDED IN TESTS OR EXAMS! / U MOET HULLE KEN EN KAN GEBRUIK. GEEN FORMULEBLAD WORD IN TOETSE OF EKSAMENS VOORSIEN NIE! 1 Selected problems on Electrochemistry 1) Nernst equation Determine the following cell potential of the cell at 25°C (298K): CuCu2+(2.00 M) Ag+(0.500 M) Ag From the table of standard electrode potentials at 25°C Cathode (Reduction) Half-Reaction Cu2+(aq) + 2e- -> Cu(s) Ag+(aq) + e- -> Ag(s) Standard Potential E° (volts) 0.337 0.7991 ANSWER: Cell reaction: Cu(s) + 2 Ag+(0.500 M) → Cu2+(2.00 M) + 2Ag(s) E0cell(298K) = E0reduction(298K) - E0oxidation(298K) = 0.799 V - 0.337 V = +0.46 V (standard cell potential)...
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...Exercise 12: Some Investigations on Corrosion of Iron I. Introduction Corrosion can be defined as the degradation of a material due to a reaction with its environment. Although this definition is applicable to any type of material, it is usually reserved for metallic alloys, in which the oxidation process M → M+ + e– is facilitated by the presence of suitable electron acceptor. The chemical reactions that take place in corrosion processes are reduction-oxidation (redox) reactions. Such reactions require a species of material that is oxidized (the metal), and another that is reduced (the oxidizing agent). In oxidation, the metal loses electrons. The zone in which this happens is known as the anode. In the reduction reaction, the oxidizing agent gains the electrons that have been shed by the metal, and the zone in which this happens is known as the cathode. (Brown, 2000) The presence of water is necessary in order to transport ions to and from the metal, but a thin film of adsorbed moisture can be sufficient. A corrosion system can be regarded as a short-circuited electrochemical cell in which the anodic process is something like Fe(s) → Fe2+(aq) + 2 e– and the cathodic steps can be any of O2 + 2 H2O + 4e– → 4 OH– H+ + e– → ½ H2(g) M2+ + 2e– → M(s) where M is a metal. (Brown, 2000) Which parts of the metal serve as anodes and cathodes can depend on many factors. In this report, the effects of the following factors on the corrosion of...
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...N. Boyd, S.K.Bhattacharjee, Organic Chemistry, 7th Edition, Pearson Other Reading Sr No Jouranls atricles as compulsary readings (specific articles, Complete reference) 4 http://onlinelibrary.wiley.com/journal/10.1002/(ISSN)1097-4601 5 http://www.springer.com/chemistry/electrochemistry/journal/10800 6 http://www.sciencedirect.com/science/journal/13882481 7 http://www.springerlink.com/content/100224/ 8 http://www.sciencedirect.com/science/journal/00108545 9 http://pubs.acs.org/journal/joceah 10 http://www.sciencedirect.com/science/journal/00323861 Relevant Websites Sr. No. (Web adress) (only if relevant to the courses) 11 http://www.klte.hu/~lenteg/animate.html 12 http://dwb4.unl.edu/chemAnime/atomic_orbits.htm Salient Features Chemistry animation and videos Atomic orbital animations 13 http://www.mhhe.com/physsci/chemistry/essentialchemistry/fla Hybridization animation sh/hybrv18.swf 1 Approved for Spring Session 2011-12 14 http://www.mhhe.com/physsci/chemistry/animations/chang_7e VSEPR animation _esp/bom3s2_7.swf 15 http://jchemed.chem.wisc.edu/JCEDLib/WebWare/collection/o Molecular orbital theory animations pen/JCEWWOR019/momovies.html 16 http://dwb4.unl.edu/chemAnime/Electro.htm Electrochemistry animations 17 http://www.mhhe.com/physsci/chemistry/essentialchemistry/fla Galvanic Cell animation sh/galvan5.swf 18...
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...an unknown solution using cyclic voltammetry and analyzing the current vs potential graphs Apparatus Required: Potentiostat and electrodes Nitrogen gas for mixing Test tubes Standard flask Reagents required: KNO3 solution 10mM K3Fe(CN)6 solution Theory: Cyclic Voltammetry: Cyclic Voltammetry (CV) is an electrochemical technique which measures the current that develops in an electrochemical cell under conditions where voltage is in excess of that predicted by the Nernst equation. Cyclic voltammetry (CV) is perhaps the most versatile electro-analytical technique for the study of electroactive species. Its versatility dined with ease of measurement has resulted in extensive use of CV in the fields of electrochemistry, inorganic chemistry, organic chemistry and biochemistry. Cyclic voltammetry is often the first experiment performed in an electrochemical study of a compound, biological material, or an electrode surface. The effectiveness of CV results from its capability for rapidly observing the redox behavior over a wide potential range. The resulting voltammogram is analogous to a conventional spectrum in that it conveys information as a function of an energy scan. Instrumentation: The main components of a Cyclic Voltammeter are the Reference electrode, Auxillary electrode, Working electrode and Potentiostat. The Potentiostat is an instrument that controls the potential of the working electrode with respect to the reference electrode while also...
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...Vinegar as a battery of Calculator Uba, Terrence L. Navarro, Loyd V. Ebabacol, Ruben S. Baa, Margaux Eve P. Ompoc, Shamira Jasmine C. Submitted in partial fulfillment of the requirements in Research 1 Alubijid National Comprehensive High School Special Science Class Alubijid, Misamis Oriental January 8, 2014 Mrs. Ma. Romila D. Uy Research Adviser Abstract Battery is a device used to store electrical energy. Battery can also be called a cell in which the reaction between two different substances can be made to occur in such a way that some of the chemical energy is converted into a useful electricity. Since its invention and inception, battery has become the most common power source for many household and industries. The vinegar battery is constructed out from simple components or materials. Adding an amount of vinegar to a strip of different metals like copper, from copper wires and zinc, from nails can form a simple battery. This battery has a low amperage output which can supply power on a low amperage/low voltage device like a calculator. It is easy to construct. The following steps should be followed in constructing the vinegar battery: 1. Prepare all the materials needed like: * Vinegar * Strip of Zinc from nails * Strip of copper from copper wire * Vinegar container (non-metallic) * Multi-tester 2. Place the vinegar inside the container. Make sure that it is deep enough to suspend the two different metals on it. 3. Cut a piece of copper...
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