chem notes 9-19 - Dr Stevens Gen Chem 1 Notes-3.1 due Fri...

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September 19, 2007 Dr. Stevens Gen. Chem. 1 Notes: -3.1 due Fri. 9pm -Exam 1 next Wed. -Review next Tuesday 9pm -Practice Exam on Bb Chapter 3 Objectives: -Determine mass of a mole in amu or of a mol in grams -Use Avogadro’s # to determine # of particles present -Interconvert between % composition and formula of a mole -balance chemical equations -use stoichiometry to determine masses of substances in a reaction Molar Mass (MM) -1 mol X = __ g X -__ g X/1 mol X = MM -Molar Mass of Compound: addition of all elements in the formula -MM(CH4) = 1xMM(C) + 4xMM(H) = 1(12.01) + 4(1.0079) = MM(CH4) = 16.04 g/mol -Can relate to # particles (mole) by Avogadro’s # mass <-> mol (varies) -through PT mol <-> particles (always the same) -Avogadro’s #: 6.022x10^23 -How many molecules are in 10.0 g CH4? -10.0g CH4 x 1 mol/16.04g x 6.022x10^23 mole/1 mol = 3.75x10^23 -If you have 10.0g Fe that rusts to form 0.0895 mol of Fe2O3, calculate total m of Fe2O3. -10.0g Fe + O2 = Fe2O3 -MM(Fe2O3) = 2Fe+3O = 2(55.847) + 3(15.9994) = 159.6922g/mol Fe2O3 -mol Fe=mol Fe2O3 -0.0895 mol Fe2O3 x 159.6922g/mol Fe2O3 = 14.292g =
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