9-12 Unit 7 II: Unit Title: Mole Concept III. Unit Length: 7 days (on a 90 min. per day block schedule) IV. Major Learning Outcomes: Students should be able to: Mole Concept • Calculate formula mass. • Convert representative particles to moles and moles to representative particles. (Representative particles are atoms‚ molecules‚ formula units‚ and ions.) • Convert mass of atoms‚ molecules‚ and compounds to moles and moles of atoms‚ molecules‚ and compounds
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One can find an empirical formula by taking a sample of a compound and dividing the number of moles of one element in the compound by the number of moles of another element in the compound to form a small wholenumber formula. For example‚ in a sample of a made up compound of oxygen and lead‚ one mole of lead has a molar mass of 207.2 g/mole‚ and oxygen has a molar mass of 16 g/mole. If this compound forms in a one to one atom ratio‚ then the ratio of moles will be 13 moles of oxygen to 1 mole of lead. In the experiment‚ the students
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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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neutralization reaction is caused by the combination of H3O+ and OH- ions. In order to determine the concentration of an unknown acid and base‚ a method called acid-base titration is used. The end of the titration has been reached when the moles of acid equals the moles of base. This is called the equivalent point. However‚ end point os the actual point that is reached in neutralization reaction. End point is signalled by the change in color of the solution because of the presence of pH indicator. The
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below. 1. Calculate the number of moles of CaCl2·2H2O from the mass you weighed out and record in the table below. Have Factor (molar mass) Want _____ g CaCl2·2H2O ___ moles CaCl2·2H2O Note: CaCl2·2H2O is an example of a hydrate‚ the 2 water molecules are attached to the crystal structure of the compound. When determining the molar mass‚ add the mass of 2 water molecules to the mass of the CaCl2. 2. From the balanced equation calculate the number of moles of Na2CO3 required to react completely
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ANALYSIS OF ASPIRIN TABLETS The aim of this investigation is to determine the percentage by mass of aspirin aspirin present in different commercial preparations and to find out‚ which the best value is‚ using a neutralization reaction followed by a direct titration with NaOH. Chemicals Used: 100 ml of distilled water in a wash bottle 50 ml of 0.100 M NaOH 40 mL of 96% ethanol phenolphthalein as an indicator (3 drops per titration) 325 mg non buffered aspirin tablets Materials Used: One
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For as long as humans have occupied this planet some form of religion has seem to accompany them. Curiosity of the unknown and explanations for things that seem difficult to explain have seemed to spark these ideas of religion. Emile Durkheim sets to explain how society’s infatuation with religion. The explanation of different forms of symbols‚ such as sacred and profane. With these explanations from Durkheim and how he sets to describe the idea of religion‚ it is relatively safe to say religion
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in the Spec 20. Data Calculations: To find the molarity of the stock solution: *Note: Molarity is moles/ Liters so in the equation below the first half is finding the number of moles of KMnO4 and the second half is dividing the moles by the liters of the solution. Grams of KMnO4 x (1 mole / molar mass (158.04g)) / Liters of stock solution = molarity of Stock Solution 0.570g KMnO4 x (1 mole / 158.04g) / 0.500 Liters = 0.00721 M To find the molarity of solution #1: *Note: To find the molarity
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Producing Isoamyl Acetate from Isoamyl Alcohol and Acetic Anhydride through Esterification Racquel Erica D.G. Isada‚ Jannah B. Juan*‚ Moses Isaiah L. Koh and Hedder A. Lim Department of Biology‚ College of Science University of Santo Tomas‚ España Street‚ Manila 1051 Date Submitted: August 13‚ 2014 Abstract: In this experiment‚ the synthesis of Isoamyl acetate from Isoamyl alcohol and Acetic anhydride was prepared with the process of Esterification. By using the reflux technique‚ extraction
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in a solution to its pure vapour pressure p∗ by its mole fraction in solution χa . a pa = χa p∗ a This allows us to calculate the mole fraction of 2-propanol χp (in the solution with the dissolved unknown) to the solutions vapour pressure pp and the vapour pressure of pure 2-propanol p∗ . p χp = pp /p∗ p 1 CHEM 3411‚ Fall 2010 Solution Set 5 Additionally‚ we know the solution only contains 2-propanol and the unknown with moles fraction of χp and χu respectively‚ and therefore χp
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