"Magnesium oxide" Essays and Research Papers

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    CHEMISTRY REVISION GUIDE for IGCSE Coordinated Science This revision guide is designed to help you study for the chemistry part of the IGCSE Coordinated Science course. The guide contains everything that the syllabus says you need you need to know‚ and nothing extra. The material that is only covered in the supplementary part of the course (which can be ignored by core candidates) is highlighted in dashed boxes: Some very useful websites to help you further your understanding include: •http://www

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    Lead (II) nitrate and potassium iodide solutions  6. Pour about 2.0 mL of lead (II) nitrate into the test tube. Add 5 to 10 drops of potassium  iodide solution to the test tube and record your observations of the reaction.  7.   8.   9. Magnesium metal and hydrochloric acid solution  10. Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid  slowly and observe the reaction. Next‚ place a burning splint near the mouth of the test  tube to test for the presence of hydrogen gas.  11.   12.   13. Electrolysis of water 

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    Milk of Magnesia

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    magnesia was invented in 1817 by the Irish pharmacist Sir James Murray (1788–1871). Murray built a plant to produce a mixture of magnesium hydroxide in water that he sold for the treatment of a variety of disorders‚ including heartburn‚ stomach acidity‚ bladder and bowel problems‚ and "female problems." He said that the liquid mixture was much more effective than powdery magnesium hydroxide which had previously been used for the same purposes. In 1880‚ New York chemist Charles Henry Phillips (1820–1882)

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    Limiting Reagents and Percentage Yield Worksheet 1.      Consider the reaction              I2O5(g) + 5 CO(g) ------->  5 CO2(g) + I2(g) a)   80.0 grams of iodine(V) oxide‚ I2O5‚ reacts with 28.0 grams of carbon monoxide‚ CO.       Determine the mass of iodine I2‚ which could be produced? 80 g I2O5 1 mol I2O5 1 mol I2 1 333.8 g I2O5 1 mol I2O5 28 g CO 1 mol CO 1 mol I2 253.8 g I2 1 28 g CO 5 mol CO 1 mol I2 b)   If‚ in the above situation‚ only 0.160 moles‚ of iodine‚ I2 was produced

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    reactive the metal‚ the more difficult it is to extract. Thus electrolysis would be used more the more reactive and the “Blast Furnace” for the less: Metal Method of Extraction Potassium Electrolysis Sodium Electrolysis Calcium Electrolysis Magnesium Electrolysis Aluminium Electrolysis Zinc Heat with C or CO Iron Heat with C or CO Lead Heat with C or CO Copper Roasting in air Silver Occur naturally Gold Occur naturally Out of all the methods‚ native metals are the easiest

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    H2 Unit 3 Lab Report

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    Unit 3 – Virtual Labs Letizia Schianodicola Lab #1 – Atomic Weight of Magnesium 1. Moles of hydrogen evolved‚ from chemical property dialog for beaker: a. 0.000411 mol H2 2. Calculate the atomic weight of Magnesium. Atomic weight of Mg = weight of Magnesium/moles of H2. b. 59‚136.253 g/mol Mg (24.305 - weight of Mg / 0.000411 mol H2) 3. Calculate the # of molecules of H2 that were produced in the reaction – use Avagadro’s number –

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    * Assorted measuring cylinders * Stopwatch * Thermometer * 0.1g of magnesium powder * 10cm3 of sulphuric acid Method: First‚ I will measure the correct amount of magnesium I need‚ which is 0.1g. Then I will measure out 10cm3 of the sulphuric acid into the measuring cylinder. Next‚ before I start the experiment‚ I will measure the starting temperature of the acid. Then I will place the magnesium and sulphuric acid in a beaker. I will measure the temperature every twenty seconds

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    Investigating Acid Rain

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    acidic presents two different problems for crops. First‚ the amount of necessary minerals in the soil such as potassium and calcium decreases. Second‚ aluminum and manganese levels increase to potentially toxic levels below a pH of roughly 5.5.Calcium oxide‚ addresses the problem. It reacts in water to release calcium ions and hydroxide ions‚ which raise the pH of the soil.The soil which is too acidic will be neutralised by the lime which is alkaline. H2O + CO2 -> H2CO3 2SO2 + H2O + O2 -> 2H2SO4

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    essential to human dietary needs. c. To facilitate the secondary use of the desalinated water‚ for example‚ irrigation. Dosages of 60 to 120 mg/L as CaCO3 of calcium containing chemicals like lime‚ calcite‚ calcium‚ hypochlorite‚ or calcium and magnesium containing chemicals like dolomite are added to the desalinated water. this is important for the water distribution

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    experiment‚ phenylmagnesium bromide‚ a Grignard reagent was synthesized from bromobenzene and magnesium strips in a diethyl ether solvent. The Grignard reagent was then converted to triphenylmethanol‚ a tertiary alcohol with HCl. The reaction for phenylmagnesium bromide was: The reaction for Grignard to triphenylmethanol was: In the formation of the Grignard reagent‚ the limited reagent‚ magnesium was determined and 0.00617mol was calculated. In the second part of the experiment‚ a yield

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