Introduction: The purpose of this experiment is to study a set of metals and their reactions reactions using different metals in an ordered activity series‚ the goal is to find the relative reactivity of them.Discovering why metals react with certain cations and solutions is the main point of this lab. This has many real life applications. When creating buildings‚ or bridges it is important to understand and counter-act the rusting of iron. You can do that by using the activity series. For any industry
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Purpose: To find out the percent yield of copper in the reaction between copper sulfate (CuSO4) and Iron (Fe). Materials: Balance 100-mL beaker 250-mL beaker Bunsen burner Copper sulfate crystals Glass stirring rod 100-mL graduated cylinder Iron filings Ring stand and ring Wire gauze Procedure: 1. Record mass of clean 100-mL beaker. 2. Add 8.0 grams of copper sulfate crystals to beaker. 3. Add 50.0 milliliters of distilled water to the crystals. 4. Put wire gauze on ring on ring
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ABSTRACT By calculating the difference in the mass of the hydrate copper (II) sulfate and the anhydride we were able to determine the mass of water in the hydrate. This information was then used to determine the empirical formula of the hydrate‚ defined as a compound formed by the addition of water to another molecule. In the first trial‚ the mass of water in the hydrate was determined to be 0.41 g‚ while in the second trial the mass of water was 0.52 g. Moles of water associated with a single
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subject than any other. Recently‚ I was assigned a lab. The purpose was to let Copper Sulfate react with Aluminum and obtain Copper. Before the experiment‚ I set up the stoichiometric equation carefully‚ predicting the production of Copper using my assigned mass of Copper Sulfate. Additionally‚ I intentionally made Copper Sulfate an excess in my equation‚ since it would be dissolved in water and I would only have to collect Copper at the end‚ to get the highest percent yield. Unfortunately‚ I did not obtain
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cylinder X Water ¡V deionizer (distilled water) X 0.1M cobalt (II) chloride hexahydrate X 95% ethanol X 0.1M cobalt (II) chloride hexahydrate dissolved in 95% ethanol X zinc X 1M hydrochloric acid solution X 0.1M copper (II) sulfate solution X 0.5M sodium hydrogen carbonate solution X 1M ammonia solution X magnesium X 1M sodium hydroxide solution X ammonium chloride Procedure: A. Be sure to always start with clean‚ dry test tubes‚ equipment‚ and
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different chemicals and what chemical has more reactivity series then other Hypothesis: Iron + Copper Sulfate: Iron will displace copper because it is more reactive and it is going to end up as Iron Sulphide + Copper Copper + Silver Nitrate: Copper will displace Silver because it is more reactive and it is going to end up as Copper Nitride + Magnesium + Copper oxide: Magnesium will displace Copper because it is more reactive. Aluminum + Iron Oxide: Aluminum will displace Iron because it is more
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Writing Practical Reports Aim: To observe what happens during and after a chemical reaction. Equipment: Concentrated nitric acid in a glass dropping bottle Small pieces of Copper 250ml Beaker 2 M Lead nitrate in a dropping bottle 2 M Potassium iodide in a dropping bottle 2 M Copper sulfate in a dropping bottle 2 M Sodium hydroxide in a dropping bottle 2 M Hydrochloric acid in a dropping bottle 4 Pyrex test tubes Test tube rack Spatula Bunsen burner‚ gauze
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materials using cheesecloth. A clean‚ cotton cloth was then subjected to a series of procedures from pretreatment and mordanting down to dyeing with the rnangosteen extract. Alum and copper sulfate were used as mordants. Results revealed that the mangosteen extract was stabilized by both mordants‚ but copper sulfate was a better fixing agent than alum‚ because it intensified the color of the extract. It can be concluded that the mangosteen husk extract can effectively be used as an alternative‚ environment-friendly
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If there are more ions available‚ then the appropriate oxidation or reduction reaction would have more chance of occurring. Apparatus * Iron electrode‚ 3cm x 2cm * Copper electrode‚ 3cm x 2cm * Iron (II) Sulfate solution - 0.2 mol dm-3‚ 400ml * Copper (II) Sulfate solution - 0.2 mol dm-3‚ 400ml * Zinc Sulfate solution - 0.2 mol dm-3‚ 400 ml * Electronic voltmeter * Connecting wires with alligator clips x 2
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Richmonde Zegbe CHM111 Anita Mohan 03-11-2013 Experiment: Chemical reactions‚ and Equations Materials: 3 mL of copper(II) sulfate solution. 5 mL of 6 M HCl piece of zinc wooden splint test tube Bunsen burner 3 mL of zinc chloride solution. pentahydrate distill water
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