Electrochemistry - redox reaction 7 Each corresponding...

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Electrochemistry April 15 th , 2008 Lab Section 2107 Course Number 4103 Simon Duri Amanda Quella
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Part One Metal Solution Observations Cu Zn (NO 3 ) 2 Nothing Zn MgSO 4 Nothing Pb Cu(NO 3 ) 2 Solution turned green/turquoise Ag Pb(NO 3 ) 2 Nothing Part Two Cathode Anode Volts Cu Zn -0.873 Zn Mg -0.852 Pb Cu 0.488 Ag Pb -0.933 Purpose : To observe and determine whether redox equations occur between electron donors and electron acceptors. Procedure : 1. Copper and Zinc Nitrate, Zinc and Magnesium Sulfate, Lead and Copper Nitrate, and Silver and Lead Nitrate were all chosen combinations for the redox cells 2. 4 small test tubes were labeled with the names of the electron donors and acceptors 3. A small amount of the appropriate solid metal was added to the appropriate labeled test tube 4. 1 mL of the appropriate electron acceptor was added to the appropriate test tube 5. After 5-10 minutes, the changes, if any, were recorded 6. The same combinations used in the first part of the lab were used to construct redox cells for each
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Unformatted text preview: redox reaction 7. Each corresponding solution to the metal used were put into wells of a dish and the corresponding solid metals were then placed into the solutions with a salt bridge 8. The salt bridge was a piece of filter paper soaked in Potassium Nitrate 9. The metals were then connected to a milivolt reader Data : Discussion DS1 : In the solutions and metals combined, only one will proceed spontaneously, the Lead and the Copper. This was expected because only in that combination a reaction occurs when the lead is the cathode and the copper is the anode. DS2 : The three combinations were correct because when the table in Appendix E was used, their E o were negative. In the combination of lead and copper, the E o was positive. Conclusion : In this lab, redox reactions were observed and only the combination of lead and copper produced a redox reaction....
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