Edexcel Level 3 BTEC Nationals in Applied Science (Forensic Science) Unit 01 – Fundamentals of Science Assignment 01-01‚ Volumetric Analysis Date set: Sept 2010 Date due: Oct 2010 This assignment addresses the following Criteria… Unit 1 – Fundamentals of Science Assessment and grading criteria To achieve a pass grade the evidence must show that the learner is able to: To achieve a merit grade the evidence must show that‚ in addition to the pass criteria‚ the learner is able to: To
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of iron to convert the mass of iron to moles. 85.65g/55.9g 1.534 moles of Iron were used 2. According to the law of conservation of mass‚ what is the mass of oxygen that reacts with the iron? 118.37g – 85.65g = 32.72 grams of Oxygen reacted with Iron 3. Calculate the number of moles of oxygen in the product. 32.72g/15.99g = 2.045 moles is the amount of moles of Oxygen produced 4. Use the ratio between the number of moles of iron and the number of moles of oxygen to calculate the empirical formula
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of the dehydrated compound from the mass of the hydrate to determine the mass of water that was present in the hydrate. -20.03 grams 5. Convert the mass of water to moles of water. -0.1281 moles 6. Convert the mass of dehydrated compound to moles of the compound. -1.113 7. Divide by the lowest mole value to get a whole number mole ratio. -0.007 Discussion and Conclusion: 1. How would you expect the final measured mass of the anhydrate to change if the hydrate was not heated for a sufficient length
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Deborah Bell April 17‚ 2012 Chemistry 1212K Lab Synthesis Report Introduction In this Chemistry Lab the main objective is to perform accurate chemical analysis for the quantity of elements and compounds in a sample. There will be a compound made then synthesized. The methods used were acid-base titrations‚ redox titrations‚ gravity filtration‚ and distillation. General conclusions included Procedures Weight of Crucibles 1. The first experiment is Preparation of a Cobalt Amine
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by the addition of water to another molecule. In the first trial‚ the mass of water in the hydrate was determined to be 0.41 g‚ while in the second trial the mass of water was 0.52 g. Moles of water associated with a single mole of anhydride were then calculated for both trials‚ giving the values of 4.7 and 4.5 moles of water‚ respectively. This indicated that the empirical formula of the hydrate might be copper (II) sulfate pentahydrate – CuSO4·5H2O. I. INTRODUCTION Hydrates are chemical
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00 g of sodium sulfate decahydrate (Na2SO4.10 H2O). Hydrates Analysis Objective: The formula for an unknown hydrate is quantitatively determined by heating the unknown hydrate to constant mass and calculating the ratio of the moles of water to the moles of anhydrous material. Observations will be made of any color changes during heating and re-hydration of the compound as well as heat effects during the re-hydration. A hydrate is a compound that is associated with a definite number
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* Introduction The melting point is defined as the temperature at which the solid is in equilibrium with its liquid‚ and this characteristic is very unique‚ so a substance can be determined by the melting point. Determination of the melting point is very important technique in many areas of chemistry especially‚ in organic chemistry area because the melting point is really significant in order to identify the purity and the identity of a substance. Measuring the melting point is a fast and
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Experiment 9 and 10: Volumetric/Vinegar Analysis Abstract: The goal of the experiment that was conducted was to figure out both the molar concentration of NaOH and the standard mole ratio of the NaOH solution. In order to find the concentration of the NaOH solution‚ volumetric analysis was used. In volumetric analysis‚ a titration mechanism was utilized in order to find the reaction that the base will end up having with KHC8H4O4
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masses and volumes as Trial 1. Calculations: 1. Determining the volume of 6 M CH3COOH (acetic acid) required to completely react with the mass of NaHCO3 NaHCO3 (s) + CH3COOH (aq) CO2 (g) + CH3COONa (aq) + H2O (l) Given 0.8023 g of NaHCO3 (Trial 1) Mole ratio 1 mol of NaHCO3 : 1 mol of CH3COOH Molar
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the formula molality = moles solute/kg solvent to find the number of moles in 10% antifreeze solution. 3. Using the formula molar mass = grams/moles calculate the molecular mass of antifreeze in the 10% solution. 4. Using the equation ΔT = Kf m¸calculate the molality of the 20% antifreeze solution. 5. Use the formula molality = moles solute/kg solvent to find the number of moles in 20% antifreeze solution. 6. Using the formula molar mass = grams/moles calculate the molecular
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