Experiment 16_ Electrolysis, the Faraday Constant, and Avogadro’s Number.pdf

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Student Name: Mina NakhlaExperiment Name: Experiment 16: Electrolysis, the Faraday Constant, and Avogadro’s NumberSubmission Date: 04-18-2021Lab Partners:Report ElementPoints EarnedMaximum ValueAbstract__________10Introduction__________15Experimental__________15Results__________25Discussion and post labquestions___________30References___________5Late Penalty__________–10 pts/calendar day lateFinal Report GRADE100
Experiment 16: Electrolysis, the Faraday Constant, and Avogadro’s NumberMina Nakhla, 04-21-2022General Chemistry II CHEM 1204Justin BogartDepartment of Chemistry and Biochemistry Maxwell Becton College of Arts and SciencesFairleigh Dickinson UniversityAbstract:Experiment 16's goal was to use electrolysis to determine the Faraday constant and Avogadro'snumber. To perform electrolysis and create hydrogen gas, a sulfuric acid solution was made anda DC source was employed. The calculated Faraday constant, according to the findings of thisexperiment was 94,300 C/mol electrons and the calculated Avogadro's number wasdeterminedto be. The accepted value for Faraday constant is 96,500 C/mol5. 783 * 1026?????????/???electrons and accepted value for Avogadro's number is. This leaves6. 02 * 1023?????????/???the % error for faraday’s constant to be 2.2% and % error for Avogadro's number to be− 1 * 10−23
IntroductionElectrolysis was the focus of this lab's experimentation. Electrolysis is defined as the act ofpassing an electric current through a material to cause a chemical change at the electrodes. Theanode undergoes oxidation, whereas the cathode undergoes reduction. The quantity of electronstransmitted is directly proportional to the amount of reaction that occurs at the electrodes. TheFaraday constant and Avogadro's number were calculated using experimental data in thisexperiment. The Faraday constant is defined as the total charge carried by Avogadro's number ofelectrons, or the charge on 1 mol of electrons. Avogadro's number is known as the number ofmoles of a reaction. The Faraday constant was found in this experiment by measuring the amountof charge necessary to reduce 1 mol ofions via the reaction 1?+[1]2?+(??) + 2?→ ?2(?)The quantity of electrical charge that travels through a location in a circuit when a currentrunsfor a certain amount of time is measured in coulombs using equation2[2]?=? * ?

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Term
Fall
Professor
Dr. Murphy
Tags
Chemistry, Faraday, Elementary charge, Avogadro constant, Faraday Constant

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