of moles of toluene = Mass/Mr = 43.35g/(92.15g/mol) = 0.470428648 moles ≈ 0.470 moles Volume of Sulphuric acid = 10mL (10cm3) Density of Sulphuric acid = 1.84g/cm3 Mass of Sulphuric acid = Density x Volume = 1.84g/cm3 x 10cm3 = 18.4g Mr of Sulphuric acid = 98.09g/mol No. of moles of Sulphuric acid = Mass/Mr = 18.4g/(98.09g/mol) = 0.187582832 moles ≈ 0.188 moles Limiting reagent: Sulphuric acid No. of moles of p-Toluenesulphonic acid = 0.188 moles Mr of p-Toluenesulphonic
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Mole Conversion Web Quest EO 103 What the heck is a mole? We have Avagadro ( and others) to thank for this…….. 6.02 x 1023 is the number of “things” per mole of the substance. Here is a tutorial for an over view and for a reference as you work through these problems http://www.wiley.com/college/chem/spencer053872/tutorial/gramsmoles/gramsmoles1.html We can use this to do mathematical conversions to determine mass‚ volume‚ and number of atoms or molecules in a given substance. For example let’s
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38 grams | Mass of hydrated MgSO4 | 3.00 grams | Mass of crucible‚ lid‚ and anhydrous MgS04 | 12.82 grams | Mass of anhydrous MgSO4 | 1.45 grams | Mass of water in hydrated MgSO4 | 1.55 grams | Moles of anhydrous MgSO4 | 0.0120 moles | Moles of water in hydrated MgSO4 | 0.0860 moles | Observation of anhydrous MgSO4 | Different shade of white‚ more thicker and solid; powder-like | 3. To obtain the mass of water‚ first measure the mass of the crucible with the lid and anhydrous MgSO4
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Marie Alessandra T. Reyes Group 4 18L Quantitative Determination of the Acidity of Soft Drinks I. Introduction Soft drinks are well known beverages among the young that are consumed mostly for pleasure. These beverages normally contain flavoring‚ sweeteners coloring‚ carbonic acid and acids. Carbonic acid and acids play an important part in the formulation of soft drinks. They enhance the flavor and give a pleasant refreshing ’lift ’ to the drink. The type of acid used can even affect the palatability
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The senses and understanding when mammals[] the senses. Adopt the mammals different senses make it interacts with what is happening in the surrounding environment. The main and senses in mammals are: 1. smell 2. Tastefully decorated 3. Hearing 4. eyesight 5. The touchscreen. These senses does not equal in all species of mammals‚ and that some of these animals may not have all the senses. Smell sense of smell of more than senses the importance in most species of mammals. Species cubicle cavity large
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contains equal numbers of Na‚ O‚ and H atoms. Since this is the case‚ the atom ratio Na:O:H is 1:1:1‚ and so the simplest formula is NaOH. In terms of moles‚ we have one mole of Na‚ 23 grams‚ one mole of O‚ 16 grams‚ and one more of H‚ 1 gram. From this kind of argument we can conclude that the atom ratio in a compound is equal to the mole ratio. We get the mole ratio from chemical analysis‚ and from that the formula of the compound. In this experiment‚ we will use these principles to find the formula
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is known as reaction stoichiometry. In the example above‚ reaction stoichiometry describes the 1:3:2 ratio of molecules of nitrogen‚ hydrogen‚ and ammonia. Stoichiometry can be used to determine quantities such as the amount of products (in mass‚ moles‚ volume‚ etc.) that can be produced with given reactants and percent yield (the percentage of the given reactant that is made into the product). Stoichiometry calculations can predict how elements and components diluted in a standard solution react
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AP Chemistry Analysis of Alum * Purpose: * In this lab we performed several tests to determine if our crystals were actually aluminum potassium sulfate. * Procedures: * Materials: * Chemicals: * Aluminum potassium sulfate‚ 2.5 g * Equipment – Part 1: * 150 mL beaker * Bunsen burner * 2 capillary tubes * Mortar and pestle * Notched stopper to hold thermometer *
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Quantities The Mole General‚ Organic‚ and Biological Chemistry Copyright © 2010 Pearson Education‚ Inc. 1 Collection Terms A collection term states a specific number of items. 1 dozen donuts = 12 donuts 1 ream of paper = 500 sheets 1 case = 24 cans General‚ Organic‚ and Biological Chemistry 2 A Mole of Atoms A mole is a collection that contains the same number of particles as there are carbon atoms in 12.0 g of carbon 12C 6.02 x 1023 atoms of an element (Avogadro’s number) 1 mole of Element
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60108 x 68.92558amu .39892 x 70.9247005 average atomic mass = 69.723amu The Mole (Section 3.2) In chemistry‚ we use the counting unit of a mole (mol). This is defined as the amount of particles that are in exactly 12.00 g of the isotope 12C. This number is 6.022 x 1023. Using this same relationship‚ it can be reasoned that 6.022 x 10 23 amu = 1.000 g. Therefore‚ the average mass of one mole of any element in grams is equal to the average atomic weight‚ also called the average
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