...rest is made of many different ingredients. -Actual start of trimyristin in the Nutmeg was 1.6 grams and we extracted .320 grams of the Trimyristin. -As a result, the percent Recovery of trimyristin from nutmeg was 20 percent. -Melting Point was 52.3 degrees Celsius of the substance we isolated (trimyristin) -When measuring the melting point of the trimyristin we took three temperatures and averaged them (51.3 degrees Celsius, 52.2 degrees Celsius, 53.4 degrees Celsius) Discussion: a.) Questions: 1. After recovering our sample of trimyristin, we tested to see what the melting point of our product would be. According to chem-info.com, the melting point for trimyristin is between 56 and 57 degrees Celsius. However, our product melted at a temperature of about 52.3 degrees Celsius, which is five degrees lower than the expected melting point of trimyristin. One of the reasons why our trimyristin melted at a lower temperature than expected may be to the fact that our extracted product was not in the purest form it could be in. The trimyristin we extracted from the nutmeg may have had some impurities which may have lowered the melting point temperature to 52.3 degrees Celsius. 2. Our experimentally determined melting point range for our...
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...Magic Salt, Melting Snow. On this experiment, it’ shows how will acquire some basic and some practical information on the chemistry and physics of water, it’s melting a freezing points and how various differing chemical compounds are utilized to promote a change of state. For example, just plain salt can be used to raise the melting point of water or lower the freezing point. Salt lowers the temperature at which water freezes. Salt absorbs moisture and forms ions when dissolved in water. In the case of snow or ice, when salt lowers the melting or freezing point of water, it serves as a freezing point depressor. Other substances that dissolve in water also lower the freezing point of the solution. The amount by which the freezing point is lowered depends only on the number of molecules dissolved, not on their chemical nature. This so called freezing point depression is described as a colligative property of water. This property is one that depends on the number of ions that a substance produces when placed in solution. The more ions a substance produces when in solution in water, the more effective it is in lowering the freezing point of water. Salts such as sodium chloride and calcium chloride which ionize are useful in de-icing. However there are other variables to be considered such as the effects of these salts on grass, pavements, cars, concrete and living animals in the area. As for the methodology of this project, this science fair experiment also serves to acquaint...
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...crystallization. The recrystallizing solvent was chosen among ethanol, water and hexane. The acetanilide was synthesized and formed by acetylation of aniline and acetic anhydride, and it was then cooled to hasten the formation of crystals. After cooling, the mixture was filtered and dried to obtain the crude acetanilide. The crude acetanilide and the chosen recrystallizing solvent was mixed and heated in the water bath until the solid dissolved. The solution was filtered while hot and its filtrate was cooled in an ice bath. The filtrate was then filtered to collect the crystal residue formed. The crystals were washed with distilled water and allowed to dry to obtain the pure acetanilide. The weight of pure acetanilide was measured and the melting point of the pure acetanilide was determined. Based on the results obtained, water is the best recrystallizing solvent among the three given solvents and the limiting reagent in synthesis of acetanilide is aniline. Introduction Purification of a solid by recrystallization from a solvent depends on the fact that different substances are soluble to different solvents. The impurities are much more...
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...examples of physical changes. Explain that chemical changes form new substances. Observe signs of chemical change in an experiment. 2.1 Section Investigation — What are some signs of a chemical change? Internet Investigation — IPPEX: Volume and Density Chapter 2 Additional Investigation: Chapter 2 Math Support & Practice: Measuring Density Solving Proportions 2.1 Reading Study Guide A 2.1 Quiz — True/False Section 2.2 -- Changes of state are physical changes. By the end of Section 2.2 the student should… Describe how liquids can become solids, and solids can become liquids. Explain how liquids can become gases, and gases can become liquids. Determine how energy is related to changes of state. Chapter 2 Investigation — Freezing Point 2.2 Reading Study Guide A 2.2 Quiz — Completion Section 2.3 -- Properties are used to identify substances. By the end of Section 2.3 the student should… Describe how properties can help you identify substances. Explain how properties of substances can be used to separate substances. Design an experiment to separate a mixture. 2.3 Explore — How can properties help you identify a substance? 2.3 Section Investigation — How can a mixture of sand, salt, and pepper be separated? 2.3 Reading Study Guide A 2.3 Quiz — True/False Chapter Review and Test Chapter 2 Vocabulary ClassZone.Com — Review concepts & vocabulary Chapter 2 Review: Textbook p. 65: 8-15, 17;...
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...| | Ice Melting Experiment and Analysis | INT1 Natural Science Task 3 | Ice Melting Experiment and Analysis ------------------------------------------------- Objective The objective of this experiment is to test the melting point of ice against different variables. I will use a control of ice against air and test this next to ice in water, sugar on ice, salt on ice and Baking Soda on ice. By measuring the melting time of each element on an ice cube I will be able to tell which element affects ice’s melting properties at what rate. Everyday we use chemical mixtures to melt ice that affects our roadways. A lot of these chemical mixtures are harmful to our waterways, and can pollute the environment. I believe its important to look for alternatives that can both help our roads from freezing in the winter while being kind to the environment. Industry Literature Review There are many different chemicals used in commercial ice melters that are made for our roads. Commercial companies tend to test for what elements melt ice the fastest, thus, producing a “best working” product. It is the pressure from consumers that encourages companies to test for possible harmful effects on the environment by these products, and what is most environmentally friendly. Ossain Inc. serves customers word wide with products designed around different needs for the type of ice melter needed. Their opinion on the ice melting industry is that the majority of ice melting companies have...
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...in all academic areas. Introduction: The physical properties of compounds are determined by a variety of factors, and one of the most important is the type of bond holding the molecules together. There are many tests that can be performed to determine whether a molecule contains covalent or ionic bonds, and three of these tests will be utilized in this lab. The compounds will be tested for their solubility and conductivity in water, and their melting points will also be determined. Covalent compounds usually do not conduct electricity in water and have relatively low melting points. Ionic compounds are usually conductive in water and have very high melting points. Using data collected from these tests, bonds can be classified as covalent or ionic. Guiding Questions: Please answer the following questions before beginning the lab. 1. A compound has a melting point of 92 oC, does not dissolve in water, and does not conduct electricity in water. What type of compound is this? 2. A compound has a very high melting point, does dissolve in water, and conducts electricity in water. What type of compound is this? Equipment/Materials: Acetylsalicylic acid Capillary tubes Calcium carbonate Conductivity apparatus Deionized water Dextrose Digital Thermometer Disposable pipet Dropping Tube Magnesium sulfate Mel-Temps Naphthalene Scoopula Sodium chloride Stirring rod Urea Wash bottle of DI water Well plate Zinc oxide Safety: Goggles should be...
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...reaction works best with dienes that are electron rich and dienophiles that are electron poor. For this experiment, our dicyclopentadiene is the diene and the maleic acid is our dienophile. In a Diels-Alder reaction, sigma bonds are formed from pi bonds. For this particular experiment, cyclopentadiene and maleic anhydride react via Diels-Alder in order to produce an endo-bicyclic product: cis-5-norbornene-endo-2,3-dicarboxylic anhydride. This product is a six-membered ring alkene with two sigma bonds. Materials and Methods Materials Used * 3 g maleic anhydride * 5 mL dicyclopentadiene * 8 mL ethyl acetate * 3 mL cyclopentadiene (from distillation) Method 1) A total of ____________ of maleic anhydride was measured out into a 125 mL Erlenmeyer flask 2) Approximately ____________ of ethyl acetate was measured out to dissolve the anhydride. This mixture was then placed on a hot plate. 3) Once heated, ____________ of hexanes was added to the mixture, and then allowed to cool in an ice bath. 4) A total of ____________ of distilled, dry cyclopentadiene was then added and mixed with the ice-cold maleic anhydride solution. 5) The mixture was then swirled in the ice bath until the exothermic reaction ended and we saw a white solid precipitate. 6) Recrystallization was then carried out to purify our final product (the cis-norbornene-5,6-endo-dicarboxylic anhydride). This was done by carrying out the steps entailed below: a. The...
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...By: Aymen Syed 12/20/15 Table of Contents Testable question and background research……………………………….page 3 Hypothesis, variables, material, procedure…………..…………………….page 4 Data………………………………………………………………………...page 5 Conclusion………………………………………………………………....page 6 Bibliography……………………………………………………………….page 7 Testable Question: Can an ice cube be lifted from a glass of water using a string? Background Research: Ice is frozen water. The state of matter ice is at in room temperature is liquid. When the temperature of water comes below a certain point, called the freezing point, it starts to solidify. The freezing point of pure water is 32 degrees Fahrenheit, but when water comes into contact with different substances the freezing point can sometimes move up or down. Salt is a white crystalline substance that gives seawater its characteristic taste. The chemical formula for table salt is sodium chloride. Salt has many uses in day to day life, and is used as a preservative, seasoning, and as a preventative measure for icing over on bridges. The reason for it being used to prevent ice forming on bridges is that it lowers the freezing point of water to slightly below 0 degrees. What is supposed to happen in this experiment is that the salt, thrown in a thin layer on top of the ice cube, should lower the melting point of the ice and melt a thin layer. The water should then cool down a bit further, and then refreeze around...
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...of solid salol, two magnifying glasses, and a match book. 2) Use a magnifying glass to look at the crystal and describe what you see. 3) Scratch off some of the crystal from the smaller side and save it on your desk. 4) Light a match and heat the bigger crystal side and time how many seconds it takes for the crystal to reach its melting point. 5) Let the melted crystal cool to room temperature and see if it has solidified. 6) Add a small piece of the crystal you previously scratch off onto the desk, and put it into the cooled crystal. 7) After you watch the crystal solidify again, heat the crystal up again. 8) This time, add a piece of lead, paper, or a piece of the match, and see if the solution solidifies. Observation: The crystal is flaky, shiny, and white. It is lumpy in some parts and flat in others. The crystals are in a shape of a rhombus. It took about 7 seconds for the crystal to melt. After adding the lead to the crystal, the lead did nothing. It did not re-solidify the crystal. Conclusions: After melting the crystal, the crystal does not solidify at room temperature. It does, however, re-solidify when solid crystal is added to it. We can conclude that this crystal remains melted at room temperature and does not re-solidify. I think that the room temperature keeps the crystal at a liquid point because it is too warm to solidify the...
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...Chemistry laboratory Pr. Zineb EDFOUF 3- Compound types CH 1213 Chemistry I Name: …………………………. Group: ….......................... Purpose: To examine the difference between ionic and covalent compounds and understand how their properties give rise to this categorization Introduction: It is amazing what early chemists accomplished even without an understanding of atomic make-up. Reading old chemistry textbooks shows how they justified some of their conclusions, which, with a few exceptions, were right on target. Some discussed the octet rule in terms of “valencies”, and they have it exactly right. What is interesting about this is that at that time they talked about this new sub-atomic particle that they were tentatively calling the “electron”. Another thing they had correct was the categorization of compounds into “covalent” and “ionic”. In class, you have discussed these compounds in terms of electrons, wherein ionic compounds transfer electrons and covalent compounds share electrons. How did the early chemists classify compounds, though, when they did not know what electrons were? They used properties, such as solubilities, melting points, and conduction. Solubility helps us to classify compounds as polar or non-polar, because, as a general rule, polar solutes dissolve in polar solvents (like water), while non-polar solutes dissolve in non-polar solvents (like oils). Conductivity means whether or not a compound will conduct electricity when it is dissolved...
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...Melting Range Report Name: Date: Lab Section: |Selected Known Compounds | |Name |Structural Formula |Literature Melting Point | |Acetanilide |[pic] |114.3°C | | |C8H9NO | | |Fluorene |[pic] |116.5°C | | |C13H10 | | |Experimental Data | |Sample Composition | |1. |2. |3. |4. |5. |6. |7. | |100% |10% |25% |50% |75% |90% |100% | |...
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...Materials and Processes Homework, Chapter 8 Review Questions Deborah Williams 10052014 1. Die casting needs more machining, 2 types, less likely are the shell process and the Shaw Process. 2. Wax and plaster of paris, jelly, sand. Shell molds use sand and plastic resin. Polystyrene in evaporative casting process. 3. Draft or taper 4. When metal solidifies from liquid it shrinks in inches/feet depending on metal. You have to leave enough extra metal to allow for shrinkage and machining. 5. Cores are the center (void) of a part. Used to produce a desired cavity. Mostly by compacting a sand mixture into the core box and curing it. 6. A crane hook needs to be able to safely handle a lot of weight, so I would use steel because it is stronger than cast iron and cast iron is a lot more brittle. 7. I would choose grey cast iron because the housing is a non-weight bearing part, it just needs to keep grease in and dirt out. The cast iron would be much cheaper to make and it doesn’t need to be remachined after either. Reducing production and labor cost. 8. I would use the shell process of sand casting. It will be much less expensive to make the molds, they can be re-used, and there would be no machining afterwards providing labor savings. 9. Used with permanent molds to make a shell of metal in the mold. Metal is poured in and allowed to solidify for a certain amount of time, used for hollow parts, not necessarily for strength. 10. Centrifugal...
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...Introduction: The melting point of a pure substance is a characteristic that is physically consistent with each specific substance. When a substance is impure, it causes the melting point to decrease and the range of the melting point to increase. In order to identify a pure substance, it must be purified in order to get an accurate melting point estimation. Purification can be done through crystallization. Crystallization is one of the simplest and most effecting ways to purify a solid. The procedure involves dissolving the impure solid, gravity filtering the hot solution through fluted filter paper to remove impurities and then cooling the filtrate to effect recovery of the material as a solid and then filtered again by suction filtration....
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...may rotate around a single bond, but dienes locked in the s-trans conformation do not react. [pic] The purpose of this experiment is to form 9,10-dihydroanthracene-9,10-α,β-succinic anhydride by way of a Diels Alder reaction between anthracene and maleic anhydride, as shown in the reaction below. Anthracene acts as the diene and maleic anhydride functions as the dienophile. Xylene (dimethylbenzene) is used as a high boiling temperature solvent so that the reaction will proceed quickly. Melting temperature analysis will be used to characterize the product. Anthracene Maleic anhydride 9,10-dihydroanthracene- 9,10-α,β-succinic anhydride OBJECTIVES IN THIS EXPERIMENT, YOU WILL • Synthesize 9,10-dihydroanthracene-9,10-α,β-succinic anhydride. • Isolate the product. • Measure the melting temperature of your product. MATERIALS PART I SYNTHESIS |50 mL round bottom flask |anthracene...
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...INT Task 3 Does Salt make Ice melt Faster? Project Plan Salt is known to be used on icy roads in certain areas of the country in the winter season to help clear roadways to make them safer for travel. Salt causes a reaction that lowers the freezing point of water. In this experiment we will test this method of applying salt to ice to see if for certain this is true, and how much faster the salt melts if so. In this experiment, the Independent Variable will be adding Salt to the ice and the Dependent variable will be the time it takes the ice to melt. The Plan is to use two ice cubes in separate containers, and add ice to only one of these. Each will be timed and observed for the duration it takes both to melt, and data will be collected throughout. At the end of the experiment, enough information will be gathered to confirm whether adding salt to ice in turn makes it melt faster, and how much faster this occurs versus adding nothing to ice. This will prove or disprove the benefit of using salt on roads to help make ice melt faster. Literature Review Many experiments have been done to test what makes Ice melt faster. Some of these included one or many different additives such as: Table Salt, Sugar, Pepper, Rock Salt. In these studies Salt prevailed as the one ingredient that would speed the melting time of Ice significantly versus adding nothing, or another substance such as sugar. (Nina DeSales, 2014). In one study Salt was added to ice water. This was done to show...
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