Formal Lab Report- making a battery.docx - LAB 8: MAKING A...

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Rebeka[COMPANY NAME][Company address]LAB 8: MAKING A BATTERYREBEKA GONZALESCHEM 1008-601INSTRUCOR: MAJI
AbstractIn this experiment we determined the oxidation reduction reactions between different elements.Using an electrochemical, or battery, we determined which elements would create the mostefficient batter. To do this, we had to understand the composition of a battery and learn how toachieve the largest possible potential with different concentrations and elements. The mostefficient battery for me was silver and lead because it was .89V and the cost was $1.375 V/$.IntroductionBatteries are a great example of putting chemical reactions to use in the everyday world.In this experiment, we used an oxidation reduction reaction to produce voltage. The transfer ofelectrons is the focal point of how a battery works. In a chemical reaction of batteries, reductionand oxidation occurs. During oxidation, the reagent loses electrons and becomes the reducingagent. During reduction, the reagent gains electrons and becomes the oxidizing agent. Potentialenergy (E) is the driving force of a reaction and is represented by ΔG=-nFE. When the oxidizingand reducing agent comes in contact with each other, a spontaneous reaction occurs.The equations used for this experiment:1.ΔG=ΔG˚+ RT lnQ2.ΔG=-RT ln K3.E=E˚-(RT/nF) lnQ4.E=E˚- (0.059/n) log Q at 25˚ExperimentThis experiment consisted of 3 parts and was broken down over 2 labs periods. For each part ofthe experiment goggles, latex gloves, and knowledge of all lab equipment was used to ensuresafety.The main redox equation used:Cu2+(aq) = Zn(s) → Cu(s) + Zn2-(aq)The materials used throughout the experiment were as followed:-2 24-cell plates-Salt bridges-Electrode-Voltage meter-Alligator-clip jumper-Pipettes-50ml Beakers-100ml beakers-50ml volumetric flasks
-100ml volumetric flaskPart 1 of lab:For the first part of the lab, we needed to construct a battery. To do this, the voltage meterand alligator-clip jumpers were connected and calibrated.We then got the copper and zincsolutions and copper and zinc metals. I poured 25ml of the 1 M zinc solution into a 50ml beakersand did the same with the 1 M copper solution in a separate beaker. Next I pipetted eachsolutions into a cell in the cell-plate. The copper and zinc metals were attached to each of thealligator clips and then placed into the opposing cells that contained their solutions.Using Kimwipes, I tore off a piece and twisted it in a rope-like manner, therefore creating the salt bridgeconnecting the solutions and metals to make a battery. Once everything was set up properly, thevoltage of the reaction was recorded.Part 2 of lab:The next part of the lab was to construct more batteries with copper and zinc like in part1. The only difference is that the concentration of the solutions are different. The firstconcentration was 1.0 M Cu2+and 1.0 M Zn2-. The second concentration was 1.0 M Cu2+and0.10 M Zn2-. The third concentration was 0.10 M Cu2+and 1.0 M Zn2-. The fourth concentrationwas 0.10 M Cu2+and 0.10 M Zn2-. The 5thconcentration was 0.50 M Cu2+and 0.50 M Zn2-. The6thconcentration was 0.010 M Cu2+and 1.0 M Zn2-. The 7thand final concentration was 1.0 MCu2+and 0.010 M Zn2-. Each concentration was kept in a volumetric flask and saved to makeeach of the other concentrations. After calculating the predicted potentials, an apparatus was usedto find the observed potential. Both the predicted and observed potentials for each concentrationis recorded on table 1.

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Term
Fall
Professor
Pheobe Zito

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