CHEM 1127Q Lecture Notes - Lecture 5: Molar Mass, Namm Show, Empirical Formula

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11 Oct 2018
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CHEM 1127Q Full Course Notes
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CHEM 1127Q Full Course Notes
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Moles and # of atoms are the key to relating products to reactants. Mm = molar mass (g/mole) n = # of moles. Number of moles -(multiply by molar mass, mm)-> mass. Number of moles -(multiply by avogadro"s number)-> number of particles. Formula mass = (# atoms x atomic mass of atom) + (# atoms x atomic mass of atom) For every one molecule of fe2o3 there are 3 oxygen atoms. Just like a car has 4 tires or a chair has 4 legs. Sometimes you want to know what percent of your sample is a certain element. Take the % directly from the chemical formula. Mass of a/x atoms -(divide by molar mass)-> moles of a/x atoms -(divide by lowest number of moles)-> a to x mole ratio -(convert ratio to lowest whole numbers)-> empirical formula. The empirical formula of a compound can be derived from the masses of all elements in the sample.

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