Experiment11

# Experiment11 - of 1.602X10-19(C/e We also weighed each electro prior and after the experiment to calculate the difference in mass which was then

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Experiment #11 Electroplating and the Measurement of Avogadro’s Number By: Garrett Lucas November 3, 2009 Summary: In this experiment, we started by obtaining a strip of copper and a strip of tin, from there we proceeded to clean each of the strips by scrubbing them down first with a piece of sandpaper. After scrubbing them down we dipped the Copper electrode in nitric acid to remove any copper oxides as well as tin deposits, furthermore; we dipped the Tin electrode in hydrochloric acid. Once the cleaning of the electrodes was completed we continued by setting up our controlled experiment, by attaching the positive terminal to the Tin, and the negative terminal to the copper. Once affixed to the current probe we place both electrodes in a tin two positive solution (Sn 2+ ). We then proceeded to collect the current produced at a constant voltage. With the numbers all collected we were able to then convert the Amps to Coulombs by multiplying by the time duration. Once we had our number in Coulombs we divided by the electron to coulomb constant
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Unformatted text preview: of 1.602X10-19 (C/e-). We also weighed each electro prior and after the experiment to calculate the difference in mass which was then converted to moles. With moles we were able to take the number of electrons divided by two and then divide by number of moles to arrive at a value in which should be similar to Avogadro’s. Results: See Attached Pages Calculations and Graphs: See Attached Pages Discussion: When both electrodes were placed in the Sn 2+ solution prior to adding charge, it appeared that the Tin particles were beginning to bind to the Copper strip. Due to the fall off of Tin into the solution my numbers did not match up. I found through Calculation, which can be seen on following pages that the number of electrons was 8.35X10 20 . The number obtained from the Tin gained was closer to the actual value of Avogadro’s number because the amount lost is not all from electrolysis. We would not know the atomic weight because it is derived from the basics of Avogadro....
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## This note was uploaded on 11/09/2011 for the course CVEN 489 taught by Professor Staff during the Spring '08 term at Texas A&M.

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