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Quantitative Chemistry Block 6 Zachary Baillie Ryan Gerhart Patrick McGay Sheel Patel

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Summary Quantitative chemistry is based on the Law of Conservation of Mass.

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Formula Mass Is the atomic weight in grams Is also called the “relative atomic mass” and “molecular mass” Examples: Hydrogen Gas H2, the formula mass is 2.0158 g=(2*1.0079) Mass of O2 is about 32 g=(2*15.9994)

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Formula Mass of Compounds The formula mass of a compound equals the sum of the formula masses of it’s components For CaCl2- Ca=40.08 g Cl=2*43.35=90.870 g Total=130.95 g For glucose(C6H12O6)- C=6*12.0107=72.0642 g H=12*1.00794=12.09528 g O=6*15.9994=95.9964 g Total=72.0642+12.09528+95.9964=80.1559

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Mass of Molecule The molecular mass is the standard unit for measuring chemicals Chemists call this a “mole” One mole of a substance contains about 6.02x10^23 This is Avogadro’s Number, L

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Calculating the Number of Moles Moles= measured mass/formula mass If we have 458.325 g. of CaCl(2), how many moles do we have? Moles= 458.325/(130.95 g/mole)= 3.5 moles

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