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expt 1 - electrochemistry -...

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MAPUA INSTITUTE OF TECHNOLOGY School of Chemical Engineering and Chemistry TANGARA, Neil Patrick P. / CHM171L  /  A31 / Group No. 5 c/o Prof. Meynard Austria, B.S. ChE, B.S. Chm PHYSICAL CHEMISTRY LABORATORY 2 Experiment No. 1 ELECTROCHEMISTRY: DETERMINATION OF FARADAY’S CONSTANT ABSTRACT This experiment intends to determine the Faraday’s constant through electrolysis using copper sulfate solution as the anode. The Faraday’s constant was determined by measuring the amount of copper metal that has deposited on the cathode at specific current levels which varied from 4-5.5 amperes. The average value of the Faraday’s constant obtained was 119,112.37 which has a 23% error versus the theoretical value of 96,485 C/mole. This report will discuss why such a phenomenon occurs. INTRODUCTION Electrochemistry studies the reactions which take place at the interface of an electronic conductor (metal electrodes) and an ionic conductor (Copper sulfate solution). In this experiment, we shall investigate the Faraday’s law and determine the Faraday’s constant through electrolysis. Electrolysis, a topic under electrochemistry, covers the Faraday’s Laws. The first law states that “The mass of any element deposited during electrolysis is directly proportional to the number of coulombs of electricity passed” while the second law states that
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