Ch 10 Notes - Honors Chemistry

12/1/2011Summary• Use Avogadro’s Number to convert◦ # of particles # of moles• Use Molar Mass to convert◦ # of moles mass (in grams)• Use both Avogadro’s Number & Molar Mass toconvert◦ # of particles mass (in grams)19Homework• All “Practice Problems” in 10.1 & 10.2 (1-6, 15-21)◦ p323 1-4◦ p324 5-6◦ p328 15-16◦ p329 17-18◦ p331 19-21• SHOW ALL WORK AND INCLUDE UNITS!!20Ch 10 - The MoleCh 10 - The MoleMoles of CompoundsMoles of Compounds21S E C T I O N 1 0 . 3• How many atoms are there in 1 mol of C atoms?• What is the mass of 1 mol of C atoms?22T H E M O L A R M A S S O F A C O M P O U N D C A N B EC A L C U L A T E D F R O M I T S C H E M I C A L F O R M U L AA N D C A N B E U S E D T O C O N V E R T F R O M M A S ST O M O L E S O F T H A T C O M P O U N D .• How many atoms is 1 g of C atoms?• What’s the mass of 1 mol of CO 2 molecules?Ch 10 - The MoleCh 10 - The MoleFormulas and Moles• The formula of a compound represents the numberof atoms of each element in one molecule/formulaunit.◦ Therefore, the formula of a compound also represents thenumber of moles of atoms of each element in one mole of thecompound.23Calculating Molar Mass24• The molar mass (molecular weight) of acompound equals the molar mass of each elementmultiplied by the number of moles of that element inthe compound, added together• 1 mol of CO 2 contains◦ 1 mol of C atoms◦ 2 moles of O atomsCh 10 - The MoleCh 10 - The Mole4