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# 5-3 Balancing Moles

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### 5-3 Balancing Moles

1. 1. 5-3 Balancing with Moles<br />Objectives:<br />Define mole.<br />Explain how moles are used in chemical reaction<br />
2. 2. Counting with Moles<br />Chemists need a practical unit to count things.<br />The mole is chemist practical counting unit.<br />1 mole of matter = 6.022 x 1023 particles<br />This number is known as Avagadro’s number.<br />1 mole of Fe = 6.022 x 1023 iron atoms<br />1 mole of Cl- = 6.022 x 1023 Chlorine ions.<br />Moles of different substances have different masses.<br />
3. 3. Are there the same number of balls?<br />
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6. 6. Molar mass<br />The mass of one mole of substance.<br />Carbon has a atomic mass of 12 amu.<br />One mole of carbon has a mass of 12 g.<br />One mole of any element equal to the mass number of grams.<br />One mole of carbon does not equal one mole of oxygen.<br />
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8. 8. Converting Mass to Moles<br />
9. 9. Converting Mass to Moles<br />
10. 10. Converting Mass to Moles<br />
11. 11. Converting Mass to Moles<br />
12. 12. Converting Mass to Moles<br />
13. 13. Converting Mass to Moles<br />Each line shows the conservation of mass.<br />There is no law that states conservation of molecules.<br />The mass numbers can be express in g/mol.<br />
14. 14. 5-3Summary<br />The law of conservation of mass says that mass can not come from nowhere or simply disappear.<br />To show mass is conserved during reaction, chemical equations must be balanced.<br />Instead of number of particles, moles are used because chemical reactions involve very large numbers of particles.<br />The mass of a reactant or product can be calculated by using chemical equations and molar mass.<br />