Presentation8_061011

Presentation8_061011 - Chem 6A Presentation #8 Overview...

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Chem 6A Presentation #8 2006-10-11 1 Overview Fundamentals F: Determination of chemical formulas Mass-percent composition Determining empirical and molecular formulas Fundamentals G: Mixtures and solutions Preparing solutions of definite concentration Separating mixtures
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2 Empirical vs molecular formulas Empirical formula indicates relative number of atoms in the compound: The empirical formula CH could be benzene or acetylene ...or something else Molecular formula indicates number of atoms in a molecule of the compound: benzene: C 6 H 6 ethyne: C 2 H 2
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3 Mass-percent composition Mass-percent composition = mass of element in sample total mass of sample When considering the mass-percent of an element in a compound, you can think of the masses in terms of: atomic mass units (amu) at the microscopic scale; or grams at the macroscopic scale. At the microscopic scale, it's often convenient to work with 1 formula unit of the compound. At the macroscopic scale, it's often convenient to work with 1 mole or 100 g of the compound.
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4 Mass-percent composition What is the mass percent of nitrogen in ammonium nitrate, NH 4 NO 3 ?
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5 Mass-percent composition What is the mass percent of nitrogen in ammonium nitrate, NH 4 NO 3 ? Consider the ratio of N to NH
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This note was uploaded on 01/31/2010 for the course CHEM CHEM 6A taught by Professor Czarkowski during the Fall '07 term at UCSD.

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Presentation8_061011 - Chem 6A Presentation #8 Overview...

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