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