Sean Dowling Julia Phaltankar Mrs. Oakes Chemistry w/ Algebra 10/G February 18‚ 2015 Determining Empirical Formula Lab Introduction: One can find an empirical formula by taking a sample of a compound and dividing the number of moles of one element in the compound by the number of moles of another element in the compound to form a small wholenumber formula. For example‚ in a sample of a made up compound of oxygen and lead‚ one mole of lead has a molar mass of 207.2 g/mole‚ and oxygen
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Analysis of Alum The objective of this lab is to run tests on a compound and analyze the substance itself‚ and then determine whether or not the compound is actually alum. Jill Cline Period 3 November 19‚ 2013 Laurel Hergenroeder and Sarinah Martelli Introduction/Purpose The purpose of this experiment is to run various tests on the substance called alum. (AlK(SO4)2 ∙ 12H2O). These tests like the process of filtration heating the solution will reveal things
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The Empirical Formula of Magnesium Oxide. Focus Question – Can the mass of magnesium combusted in excess oxygen be used to determine the empirical formula of magnesium oxide? Hypothesis – Combustion of Magnesium will generate data which can be used to calculate the EF of Magnesium Oxide Experimental Report: Data Collection and Processing Qualitative Observations: * The Magnesium burnt with a very bright flame. (as seen in figure 2 below) * White smoke was formed and some
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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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Formal Lab Report #1 I. Basics Title of the Experiment: The Empirical Formula of an Oxide Authors: Section Number: Chemistry Location and Date II. Abstract The aim in this lab was to determine the empirical formula of an oxide of magnesium through combustion in air. This was achieved by heating an established mass of magnesium in air inside of a crucible‚ ultimately attaining a compound that contained Mg and O. The major result of the experiment was the empirical formula of the oxide of magnesium
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Chemistry SL Magnesium Oxide Lab Report Rashpreet Singh Date Performed: November 6‚ 2014 Research Question: To determine the empirical formula of the compound which forms between magnesium and oxygen. Design: The following figure represents the experiments lab setup‚ visualize the equipment used. Materials: Done 1. Ceramic evaporating dish 2. Electronic balance 3. Bunsen burner 4. Retort stand‚ ring clamp‚ clay triangle 5. Sand Paper 6. Tongs 7. Magnesium Ribbon Safety: Done 1. The duration
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The primary objective in the lab is to determine the molecular formula of Copper Oxide through synthesis of copper oxide. In the first procedure‚ an empty crucible‚ Bunsen Burner‚ and electronic scale were placed onto the workbench. The electronic scale was zeroed before the crucible was placed on it. The total mass of the empty crucible was 88.000g. Afterwards‚ 10 grams of copper powder was placed into the crucible and weighed to be 98.000 g. The crucible with the copper was placed onto the Bunsen
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Emission Spectroscopy Lab Introduction: According to the Bohr atomic model‚ electrons orbit the nucleus in fixed paths with specific energies. Each path is therefore often referred to as an “energy level”. Electrons possessing the lowest energy are found in the levels closest to the nucleus. Electrons of higher energy are located in progressively more distant energy levels. If an electron absorbs sufficient energy to bridge the “gap” between energy levels‚ the electron may jump to a higher
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Pre-Lab Discussion An empirical formula is a formula for a chemical compound found by direct laboratory examination. Laboratory procedures allow the chemist to find the simplest whole number ratio of elements within the compound. In order to find the true molecular formula‚ the chemist also needs to know the compound’s molecular mass. The general procedure is to use laboratory techniques to determine the mass of each element in the compound. In this lab‚ we will react a known quantity of magnesium
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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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