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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Heat of Combustion of Magnesium Background: The students were given full instructions on how to experimentally determine the enthalpy of reaction (ΔHrxn) for the combustion of magnesium ribbon‚ using Hess’s Law. Data Collection: | |Reaction 1 |Reaction 2 | | |(MgO) |(Mg)
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Empirical Formula Lab Class: Chemistry 1405 Fall 2013 Aim: The aim of this Lab Exercise is to use the mass of a chemical and use that mass to find the amount of moles of the final product you can get using the empirical formula. Introduction: The empirical formula of a compound is the simplest whole-number ratio of the elements in the compound‚ which as you will discover‚ is a ratio of the moles of those elements. “Empirical” also means “experimentally determined”. In this experiment
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0.1 g of ammonium dichromate phenolphthalein tongs strip of magnesium spatula NaOH HCl sodium nitrate potassium chloride. magnesium sulfate calcium nitrate sodium carbonate. Safety notes: 1. Wear aprons and
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Empirical Formula of Copper (II) Chloride Gabriella Jane Lukas B1401404 HELP University Empirical Formula of Copper (II) Chloride Objectives 1. To validate that the empirical formula of copper (II) chloride is . 2. To calculate the percent composition of copper in copper (II) chloride. 3. To illustrate the Law of Constant Composition in copper (II) chloride. 4. To study the reaction between copper (II) chloride solution and aluminium metal. Introduction One of the most fundamental statements
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heat evolved when magnesium reacts with dilute acids. Planning What I am going to do I am going to find out how much heat is given out when magnesium reacts with a variety of dilute acids. In order to make comparisons between the acids‚ I shall use my results to work out how much heat would be given out if 1 mole of magnesium reacted with an excess of each acid. The acids I shall use are hydrochloric acid‚ sulphuric acid‚ nitric acid and ethanoic acid. What I already know Magnesium reacts with most
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Magnesium Mg(Z=12) in Group 2 Alkaline Earth Metals The structure of the element: Giant lattice metallic structure of immobile positive metal ions surrounded by a ’sea’ of freely moving mobile electrons (so-called delocalised electrons). Physical properties: A moderately hard silvery-white solid; mpt 649oC; bpt 1090oC; good conductor of heat/electricity. Group‚ electron configuration (and oxidation states): Gp2 Alkaline Earth Metal; e.c. 2‚8‚2 or 1s2 2s2 2p6 3s2; (+2 only) e.g. MgCl2
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Purpose: To determine the percent magnesium by mass in magnesium oxide and to observe if the percentage composition is constant by comparing class results. Hypothesis/Prediction: The percent composition by mass of magnesium in magnesium oxide will not change significantly with each group that conducted the experiment. The composition of each substance should stay the same and any differences must be due to some error. Materials:Magnesium stripCrucibleCrucible coverClay triangleIron ringRetort standTongsBalanceBunsen
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Beryllium and magnesium These are just like the reactions with dilute hydrochloric acid‚ and you have probably been familiar with the reaction between magnesium and dilute sulphuric acid almost since you started doing chemistry. Bubbles of hydrogen are formed‚ together with colourless solutions of beryllium or magnesium sulphate. For example: Calcium‚ strontium and barium Calcium sulphate is sparingly soluble‚ and you can think of strontium and barium sulphates as being insoluble
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Zinc oxide in a mixture with a about 0.5% iron(III) oxide (Fe2O3) is called calamine and is used in calamine lotion. There are also two minerals‚ smithsonite and hemimorphite‚ which have been called calamine historically (see: calamine (mineral). Zinc peroxide‚ ZnO2 .½ H2O‚ is a white to yellow powder that is used in antiseptic ointments. Zinc white is used as a pigment in paints and is more opaque than lithopone‚ but less opaque than titanium dioxide. It is also used in coatings for paper
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