Chemistry Practical Report: Topic: Determining the Empirical Formula of Magnesium Oxide Patrick Doan 11 CHEM 11 26/9/08 Table of contents 1.0 Aim 1 2.0 Theory 2-3 3.0 Materials 4 4.0 Method 4 5.0 Results 4 - 5.1 Qualitative Observations 4 - 5.2 Example Calculations for each Calculated Value 5-7 -5.21 Experimental Values and Associated Errors 5-7 - 5.3 Accumulated Raw Data 8 - 5.4 Mean Experimental
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Shawn Dubbs Lab 1 The Mole Concept of and the Chemical Formula of a Hydrate Abstract: The objective of this lab was to conduct an experiment to analyze the molar components in alum. This was conducted by heating the alum till the water had evaporated and then determining the number of moles for each component. Then using the these amounts to figure out the empirical formula for alum. Results: In order to determine how much of each separate component a total mass was taken before hand for
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Analysis of a Copper Sulfate Sample Empirical Formula of Hydrous Copper Sulfate Joel Ramirez 9/25/2012 10/2/2012 The purpose of this experiment is to find the empirical formula of a hydrous copper sulfate sample and the amount of water in the sample. This whole process will be determined in three different experiments. Procedure: Experiment 1 – Percentage of water in sample. The percentage of water in hydrous copper sulfate was determined. Clean‚ dry and weight the crucible
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FORMAL LAB REPORT INTRODUCTION John Dalton’s atomic theory states that elements combine in simple numerical ratios to form compounds. A compound‚ no matter how it is formed‚ always contains the same elements in the same proportion by weight. The law of mass conservation states that mass can neither be created nor destroyed. In this experiment‚ the mass of the metal was not destroyed or created; the metal’s mass was simply changed into a compound form once the gas
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Formula of a Hydrate Lab Wednesday October 29‚ 2014 Chemistry Honors Purpose This lab was done to determine the percentage of water in a hydrate‚ which was CuSO4 ?H20. Not only the percentage of water can be found‚ the moles of water can be found per one mole of anhydrous salt. An anhydrous salt is a hydrate that lost its water. Using various lab equipment such as burners‚ crucible‚ and balance‚ and techniques such as the mass-to-mole ratio and mass to percentage‚ the percentage of water in a hydrate
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Experimental Determination of the Formula of Magnesium Oxide. Introduction: Magnesium is a mental‚ it is known to react with oxygen. Magnesium reacts vigorously when heated in the presence of air‚ which is why we have chosen high heat in our method to facilitate combustion. This oxidation reaction produces magnesium oxide gaining oxygen from the air. When sharing of electrons occur a chemical bond is made and the atoms combine to form a molecule. So‚ the predicted molecular formula:
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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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DETERMINATION OF THE CHEMICAL FORMULA FOR A HYDRATE USING MOLE RATIO OF WATER MASS AND MAGNESIUM SULPHATE INTRODUCTION Ionic (salt) compounds are able to hold loose bonds with water molecules. A hydrate is a compound that incorporates water molecules into its crystalline lattice structure (McGraw-Hill Ryerson‚ 2014). Identifying a compound as hydrated or anhydrous is important as the mass of the compound increases if it contains water molecules. In nature‚ hydrates exist with a fixed ratio
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CHM 3120L ANALYTICAL CHEMISTRY I LABORATORY REPORT EXPERIMENT: SPECTROPHOTOMETRIC DETERMINATION OF IRON IN DRINKING WATER Name: Steven Adrien Section: 3 Date Experiment Completed: Wednesday‚ July 17‚ 2013 1. Complete the following table Fe(II) stock solution | mass‚ g | 0.1756 | volume‚ mL | 500.0 | MW(Fe(NH4)2(SO4)2 x 6H2O)‚ g/mol | 392.14 | AW(Fe)‚ g/mol | 55.85 | conc. Fe(II)‚ ppm | 50.0 | Use Equation Editor to show how you calculated the concentration of Fe(II)
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Chemistry 2 Jorge Nuñez Ms. Principe / Period 2 February 8th‚ 2011 Aim: How are we going to determine the empirical formula of a compound? Do Now: 1) What is the percent by mass of oxygen in H2C2O4? H2 = 2(1) = 2 ; C2 = 2(12) = 24 ; O4 = 4(16) = 96 Gram Formula Mass = 90 Percentage of Oxygen = 6490 x 100 = 71% 2) Calculate the percentage of water: -Mass of empty crucible and cover = 11.7g -Mass of crucible‚ cover‚ and hydrate before heating = 14.9g -Mass of crucible
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