Experiment 4 (Galvanic Cells).docx - CM011L CHEMISTRY FOR ENGINEERS(LABORATORY 1ST Quarter SY 2018-2019 Galvanic Cells the Nernst Equation(Experiment 4

Experiment 4 (Galvanic Cells).docx - CM011L CHEMISTRY FOR...

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CM011L: CHEMISTRY FOR ENGINEERS (LABORATORY) 1 ST Quarter SY 2018-2019 Galvanic Cells, the Nernst Equation (Experiment 4) Manguiam, Von Louie R. 1 , Sario, Kachel Joy, S. 2 1 Professor, School of Chemical, Biological, and Materials Engineering and Sciences, Mapúa University; 2 Student, CM011L/GEOA9, Mapúa University ABSTRACT An electrochemical cell is a device that utilizes electrochemical processes, particularly the conversion of chemical energy into electrical energy and vice versa; these processes employ redox reactions which involves the oxidation, the loss of electron(s) of a compound or element, and the reduction, the gain of electron(s) of a compound or element, thus an exchange of electrons happens. A galvanic cell is made up of two electrodes and solutions. It consists of two half-cells housing the redox couple in each of their compartments in which either oxidation or reduction occurs, separated by a porous partition called a salt bridge. Adapted from J.A. Beran’s Tenth Edition of Laboratory Manual for Principles of General Chemistry, the experiment involved the measure of reduction potentials in the setups of copper-zinc, zinc-iron, and copper iron cells, identification of factors affecting cell potentials of CuSO4 concentration, and calculation of four concentrations of Cu(NO3)2 solution. Identification of the anode and cathode allowed for the writing of half- reactions and balanced reactions; reduction potential of a cathode determined by using the reduction potential of the anode zinc and the formula for standard cell potentials; the electromotive force of concentrations of Cu(NO3)2 solution calculated using the Nernst equation. Employment of these satisfied the objectives of the experiment to measure relative reduction potentials for a number of redox couples, develop an understanding of the movement of electrons, anions, and cations in a galvanic cell, study factors affecting cell potentials, and estimate the concentration of ions in solution using the Nernst equation. Keywords : galvanic cell, redox reaction, cell potential, Nernst equation, electrochemistry INTRODUCTION An electrochemical cell is a device that utilizes electrochemical processes, particularly the conversion of chemical energy into electrical energy and vice versa; these processes employ redox reactions which involves the oxidation, the loss of electron(s) of a compound or element, and the reduction, the gain of electron(s) of a compound or element, thus an exchange of electrons happens. The first electrochemical cell was invented by Italian physicist Alessandro Volta (1745- 1827). He designed a cell that can be used for the generation of a direct electric current (DC). These are called voltaic cells which are electrochemical cells that are used for the conversion of chemical energy into electrical energy (Addison-Wesley, 1997). This energy is produced by the spontaneous redox reactions occurring within the cell thus generating an electric current – the flow of electrons through a circuit. These voltaic cells are commonly known as galvanic cells.
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