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1	Chapter 6 Calculations: Formula Masses, Moles, and Chemical Equations
2	Diamond is a covalent compound with many carbon atoms
3	Molar mass: The mass units Fig. 6.1 Oranges may be bought in units of mass or units of amount.
4	First chemical compound need to be weighed Fig. 6.2 A basic process in chemical laboratory work is determining the mass of a substance.
5	Mole is a counting unit used by chemists Fig. 6.3 Everyday counting units.
6	Unlike a dozen Avogadro’s number is large: 6.0022 x 10²³ Fig. 6.4 Amadeo Avogadro was the first scientist to distinguish between atoms and molecules.
7	Formula Masses in grams gives a Mole of a chemical compound Fig. 6.5 The mass of a mole depends on the substance.
8	To get the Formula Masse first find the types of atoms in the compound Fig. 6.6 A computer-generated model of the molecular compound N₂O₄.
9	Moles multiplied by Avogadro's number gives number of atoms and molecules Fig. 6.7 In solving chemical-formula-based problems, the only “transitions” allowed are those between quantities (boxes) connected by arrows.
10	Law of conservation of mass/atoms Fig. 6.8 When 16.90g of the compound CaS is decomposed into its constituent elements, the Ca and S produced has an identical mass of 16.90g.
11	Conversion factors in chemical calculations: Stoichiometry
12	Mole conversion to grams and particles Fig. 6.9 In solving chemical-equation-based problems, the only “transitions” allowed are those between quantities (boxes) connected by arrows.
13	What does 16-20-0 means in fertilizer?
14	Air bag should have right amount reactants to produce gas or baby will crush. Fig. 6.10 Testing apparatus for measuring the effects of air bag deployment.