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Chapter 10 Chemical Quantities 10.1 The Mole Chemistry Today we are learning to:1. Understand the relationship between moles, Avogadro’s number and gram formula mass 2. Use gram formula mass to convert grams of a substance into moles 3. Use gram formula mass to convert moles of a substance into grams 17.1 The Mole Exothermic and Endothermic Processes 1 mole is defined a the number of atoms of carbon present in exactly 12g of carbon-12. This number of atoms is called Avogadro’s number and is equal to 6.022x1023 atoms. It follows that: 1 mole of any element = 6.022x1023 atoms = atomic mass of element 1 mole of any compound = 6.022x1023 formula units/molecular formula = gram formula mass of compound The mole can be abbreviated to mol 17.1 Converting Exothermic and GramsEndothermic to Moles Processes To convert from grams to moles use the formula: 1 mol moles = number of grams x -------------------------------Gram formula mass Converting Moles to Grams To convert from moles to grams use the formula: Gram formula mass grams = number of moles x -------------------------------1 mol 17.1 Converting Exothermic and MolesEndothermic to Grams Processes Sulfuric acid Ex.1 how many grams are present in 40.5 mol of H2SO4? 1. Identify the knowns and unknowns moles of H2SO4 = 40.5 mass of H2SO4 = ? 2. Calculate gram formula mass. For H 2 x 1.0 amu = 2.0 amu For S 1 x 32.1 amu = 32.1 amu For O 4 x 16.0 amu = 64.0 amu formula mass = 98.1 amu 3. Plug in the numbers and solve equation Gram formula mass Mass g = number of moles x ---------------------------1 mol 98.1 g Mass g = 40.5 mol x ----------1 mol Mass g = 3970 g Try question 27-50 on page 50-51 of review book END OF SHOW