Formula and Percent Composition of the Compound Magnesium Oxide (MgO) Nice sounding title Date Performed Lab: 8/31/06 Purpose: The purpose of this lab was to confirm the chemical formula of magnesium oxide by comparing the masses of pure magnesium solid prior to any reaction and magnesium oxide solid after a reaction between all of the magnesium and oxygen from the air when heated from a Bunsen burner in a crucible. Using molar masses of both magnesium and oxygen‚ an expected percent composition
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addition of Grignard reagents to three different carbonyl groups: a ketone‚ an ester‚ and a carbonate. Grignard reagents are organometallic compounds that have a carbon-metal bond‚ such as carbon-magnesium. Grignard reagents are formed from the reaction of an alkyl‚ cycloalkyl‚ or aryl halide and magnesium metal in dry ether. The reaction is shown below in figure 1. Figure 1: Formation of a Grignard reagent The Carbon bonded to the metal is both a strong nucleophile and base. The Carbon
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A) January 18‚ 2011B) Empirical Formula C) The purpose is to determine the empirical formula of a metallic oxide. D) Pre Lab Questions: After heating the metal‚ the crucible and contents should mass less than it did before it was heated. This is because heating the crucible may rid of other residue that was left in it; bringing it a to a constant mass. A yellow flame will deposit soot on the crucible. This would be a problem because the soot left on the crucible would vary from our constant
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CHEMISTRY EXPERIMENTAL REPORT SALLY LI INTRODUCTION: In chemistry‚ compounds can be distinguished by using the empirical formula. The formula provides the simplest positive integer ratio of elements in a compound. The empirical formula is largely useful in determining the ratio of elements within ionic compounds where the structure is of a non-directional nature of bonding where any ion at any time could be surrounded
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Lab of Determining an Empirical Formula B2 Honors 12/18/13 Abstract In this lab‚ to help better understand the concepts of gram atomic masses and empirical formulas‚ we found the gram atomic masses and empirical formula of a binary compound. The two compounds should form a definite whole number ratio by mass. This ratio will also help determine the subscripts of the elements in the empirical formula. Errors in this experiment can stem from measuring wrong or doing equations incorrectly.
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Grignard Synthesis of Tirphenylmethanol David Szuminsky Organic Chemistry Lab II Shaopeng Zhang Monday 1PM 2/10/14 & 2/24/14 - Abstract A sample of triphenylmethanol was prepared using Grignard synthesis techniques. Reflux was used in order to speed up the reaction and the final product was purified using recrystallization methods. The percent recovery and percent yield were 80.46% and 47.526%‚ respectively. A melting point range of 85-87oC was obtained from
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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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Massing Magnesium Lab Research Question/Aim To understand the change in mass after burning magnesium and to also determine the chemical formula of magnesium oxide Hypothesis Burning the magnesium will result in an increase in mass because the magnesium will react with oxygen in the air to make magnesium oxide Variables Independent- Initial mass of magnesium (Mg) Dependent- Mass of the burnt magnesium (MgO) Controlled: Intensity of flame Apparatus used (same crucible‚ Bunsen burner
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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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04.05 Chemical Reactions: Combustion: Lab Worksheet and Rubric Before You Begin: You may either copy and paste this document into a word processing program of your choice or print this page. Procedure: 1. Iron (III) and copper (II) sulfate solution 2. Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction. 3. 4. 5. Lead (II) nitrate and potassium iodide solutions 6. Pour about 2.0 mL of lead (II) nitrate into the test tube
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