Chemistry 107 Lab Report 11

# Chemistry 107 Lab Report 11 - 118.71g 2e-Na of Sn 1 mol Sn...

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Summary In this experiment we deposit tin onto a piece of cooper by the electrolysis of a tin (II) solution. By measuring the electric current that flows through the solution, we were able to calculate Avogadro’s number. The first thing we had to do was clean off each metal in an acid solution. Once our electrodes were clean we measure each one on an analytical balance. Finally, we let the electrodes sit in a 40 mL Sn 2+ solution for a few minutes and to record observations. As the electrodes set in the solution, data was also imputed to the computer. 1. ( Tin) .7294g – .5725g = .157g lost (Copper) 1.1226 g – 1.1842g = .062g gained Convert mass to moles: Tin .157g / 118. 7 = .0013 mol Copper .062g / 63.54 = .0011 mol 2. Calculate total charge: 144.3 / 1.602E-19 = 9E+20 3. Avogadro’s number 144.3 Sn (S) 1 mol Sn
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Unformatted text preview: 118.71g 2e-Na of Sn 1 mol Sn = 6.02E23 Discussion For some odd reason the Copper gained weight in the solution. The only explanation could be is that the Copper reacts in the Sn more solution than the Tin. What I also lean is not all metals react to electricity. The Sn look it like a crystal like structure while the Cu just deteriorate. Our value came out to be Avogadros number. Even though the electrodes were different the value was very close. The only difference that I seen that could of play a factor is that one metal gain mass and the other loss some. Tin didnt represent a flaw in our method. Avogadros number is best on the elements so we would know the atomic weight of Tin with Avogadros number. 1mol of Sn = 6.02*10^23) In conclusion, we calculated Avogadros number at an accepted value....
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## This note was uploaded on 11/10/2009 for the course CHEM 107 taught by Professor Generalchemforeng during the Spring '07 term at Texas A&M.

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