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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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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The Calorimeters Calorimeters are a device that can measure the heat that comes from burning an item. Simple Calorimeter A simple calorimeter is used to detect the enthalpy change when a fuel is burned. The fuel is burnt to heat a specific mass of water and then measure its rise in temperature. The word calorimeter comes from the Latin phrase calor which means heat. A simple calorimeter just consists of a thermometer attached to a metal container full of water suspended above a combustion chamber
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Introduction The experiment is testing for the formation of precipitates caused by different limiting reactants. A precipitate results in a solid formed by an ionic compound. Calcium nitrate and copper sulfate will be added to separate beakers with approximately half of the solutions from the Büchner funnel system of each trial to test for the formation of precipitates. The limiting reactant is the reactant that will run out first in the chemical reaction. It is important to recognize which chemical
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this experiment‚ you will observe the reaction of iron nails with a solution of copper (II) chloride and determine the number of moles involved in the reaction. You will determine the number of moles of copper produced in the reaction of iron and copper (II) chloride‚ determine the number of moles of iron used up in the reaction of iron and copper (II) chloride‚ determine the ratio of moles of iron to moles of copper‚ and determine the number of atoms and formula units involved in the reaction. Through
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exothermic B. is endothermic C. has H > 0 D. both a and c are correct E. both b and c are correct 4. Calculate the heat of vaporization of carbon tetrachloride given that the standard molar enthalpy of formation of liquid carbon tetrachloride is -135.4 kJ/mol and the standard molar enthalpy of formation of gaseous carbon tetrachloride is -102.9 kJ/mol. A. +102.9 kJ/mol B. -32.5 kJ/mol C. +238.2 kJ/mol D. +32.5 kJ/mol E. -238.2 kJ/mol 5. The complete combustion of 1 mole of propane
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