Empirical Formulas from Analyses

Empirical Formulas from Analyses - Empirical Formulas from...

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Empirical Formulas from Analyses An empirical formula tells us the relative ratios of different atoms in a compound. The ratios hold true on the molar level as well. Thus, H 2 O is composed of two atoms of hydrogen and 1 atom of oxygen. Likewise, 1.0 mole of H 2 O is composed of 2.0 moles of hydrogen and 1.0 mole of oxygen . We can also work backwards from molar ratios: if we know the molar amounts of each element in a compound we can determine the empirical formula . Mercury forms a compound with chlorine that is 73.9% mercury and 26.1% chlorine by mass. What is the empirical formula? Let's say we had a 100 gram sample of this compound. The sample would therefore contain 73.9 grams of mercury and 26.1 grams of chlorine. How many moles of each atom do the individual masses represent? For Mercury: (73.9 g)*(1 mol/200.59 g) = 0.368 moles For Chlorine: (26.1 g)*(1 mol/35.45 g) = 0.736 mol What is the molar ratio between the two elements? ( 0.736 mol Cl/0.368 mol Hg) = 2.0
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This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

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Empirical Formulas from Analyses - Empirical Formulas from...

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