Lacey_Che131_S2012_Lect-5s

Lacey_Che131_S2012_Lect-5s - Lec5:TheMole&Compounds

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Lec 5: The Mole & Compounds 1 Roy A. Lacey, Stony Brook University; Che 131, Falll 2012 Chemical Equations Chemical equations describe the changes on the atomic level, but one cannot easily work with individual atoms in the lab. Æ We work with a macroscopic quantity called the mole Roy A. Lacey, Stony Brook University; Che 131, Falll 2012 2
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The Mole ` 1 mol = 6.02 × 10 23 items, ` Avogadro’s number (N A ) ¾ The mole is a unit like dozen (12) or gross (144). It denotes the quantity of items. ¾ A mole is Avogadro’s number of atoms in exactly 12 grams of carbon 12. The mole is a very large number!! Roy A. Lacey, Stony Brook University; Che 131, Falll 2012 3 How Large is the Mole? ± 1 mole of hockey pucks would equal the mass of the moon mass of the moon! ± 1 mole of basketballs would fill a bag the 1 mole of basketballs would fill a bag the size of the earth! ` 1 mole of pennies would cover the Earth 1/4 il d mile deep! Roy A. Lacey, Stony Brook University; Che 131, Falll 2012 4
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Mole Conversions
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This note was uploaded on 03/29/2012 for the course CHE 131 taught by Professor Kerber during the Spring '08 term at SUNY Stony Brook.

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Lacey_Che131_S2012_Lect-5s - Lec5:TheMole&Compounds

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