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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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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LEARNING TASK NO. 4B Composition Stoichiometry Problems Mole Relationship from Chemical Formulas: a) Determine the number of moles of chloride ions in 2.53 mol ZnCl2. b) Calculate the number of moles of each element in 1.25 mol glucose (C6H12O6). c) How many molecules of oxygen atoms are present in 5.00 mol diphosphorus pentoxide? d) Calculate the number of moles of hydrogen atoms in 11.5 mol water. e) A sample of ethanol (C2H5OH) has a mass of 45.6 g.How many carbon atoms does the sample
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involved in burning magnesium metal. Materials Stirring rod Retort stand Ring clamp Clay triangle Crucible and lid Bunsen burner Flint lighter Balance Crucible tongs 40 cm of magnesium ribbon Method 1. Find the mass of a clean crucible and lid. USE THE SAME BALANCE DURING THE ENTIRE EXPERIMENT. 2. Curl the magnesium ribbon around a pencil to make a size that just fits inside the crucible. Do not curl the ribbon too tightly. 3. Describe the magnesium ribbon. 4. Find
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Determining the Chemical Formula of a Hydrate Chemistry 11 3/5/2013 Purpose: To determine the percent by mass of water in a hydrate of copper (II) sulfate hydrate. Hypothesis: I hypothesize that when the solution is heated the hydrate will convert to an anhydrous ionic compound. Then the percentage composition will be determined by weighing the mass of the white crystals. Materials: 400ml beaker‚ hot plate‚ tongs‚ scoopula‚ electronic balance‚ glass rod‚ hot pad‚ and 4g of hydrated
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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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3/4/14 Determining The Formula of a Complex Ion Luqman Khan Contents: Aim………………………………………………………………………………………………………………….……2 Results……………………………………………………………………………………….………………………2-6 - Raw Data………………………….………….……………………………………………………..…..2 - Qualitative Analysis………………………………………………………………………………….2 - Data Processing……………………………..……………………………………………………..3-5 - Graphical Results……………………………..…………………………………………….…….5-6 Conclusion…………………………………………………………………………………………………………6-7 Evaluation……………………………………………………………………………………………………………
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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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Mass of Magnesium(Mg) (g) | Volume of Hydrogen (H₂) (cm³) | 1st trial | 0.040 | 39.9 | 2nd trial | 0.040 | 40.3 | 3rd trial | 0.035 | 36.5 | Quantitative data: The Magnesium was silvery-white‚ lustrous and relatively flexible before being placed in the burette. Whilst reacting with the hydrochloric acid‚ it dissolved and bubbles were visible. The hydrochloric acid slowly diffused downwards. Calculations: Volume of un-diffused hydrochloric acid = 25 cm³ Average mass of magnesium = 0.038
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