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Mass Relationships

Mass Relationships. The Mole and Stoichiometry. The Mole. A mole is the number of atoms in exactly 12 grams of 12 C (carbon-12 isotope) One mole is equal to 6.02x10 23 particles A particle will be an atom(elements) or molecule(compounds) The number 6.02x10 23 is known as Avogadro’s number.

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Mass Relationships

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  1. Mass Relationships The Mole and Stoichiometry

  2. The Mole • A mole is the number of atoms in exactly 12 grams of 12C (carbon-12 isotope) • One mole is equal to 6.02x1023 particles • A particle will be an atom(elements) or molecule(compounds) • The number 6.02x1023 is known as Avogadro’s number

  3. Molar Mass • The mass of one mole of any chemical substance is numerically equal to the periodic table weight of the substance • The gram mass of one mole of substance is known as the molar mass • Molar mass has the unit grams per mole (g/mol) • Molar mass is used as a conversion factor between gram and mole values

  4. Molar Mass • What is the molar mass of carbon dioxide? • Formula: CO2 Formula mass: 44 amu • Molar Mass: 44 g/mol

  5. Molar Mass • What is the molar mass of carbon dioxide? • Formula: CO2 Formula mass: 44 amu • Molar Mass: 44 g/mol

  6. Conversions using molar mass • Convert 5.0 g of CO2 to moles of CO2 • Divide 5.0 g by the molar mass • 5.0 x 1 mole = 0.114 moles CO2 • 44 g

  7. Conversions using molar mass • Convert 2.0 mol of CO2 to grams of CO2 • Multiply moles by the molar mass • 2.0 mol x 44g = 88 g CO2 • 1 mole

  8. Conversions using Avogadro’s # • Convert 2.0 mol of CO2 to molecules of CO2 • Multiply moles by Avogadro’s # • 2.0 mol x 6.02x1023 = 2.4x1024 CO2molecules • 1 mole

  9. Conversions using Avogadro’s # • Convert 2.0x1026 mol of CO2 to moles of CO2 • Divide moles by Avogadro’s # • 2.026 CO2 x 1 mole = 330 CO2 molecules • 6.02x1023

  10. Quiz Time!

  11. Make the following computations • What is molar mass of water? • A) 12 g/mol • B) 16 g/mol • C) 18 g/mol • D) 19 g/mol

  12. Make the following computations • What is the mass of 2 moles of water? • A) 24 g/mol • B) 36 g/mol • C) 18 g/mol • D) 9.0 g/mol

  13. Make the following computations • How many moles are in a 1.0 kg sample of water? • A) 56 g/mol • B) 6.0 E23 g/mol • C) 18 g/mol • D) 6.0 E26 g/mol

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