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Review: Molar Mass of Compounds

Review: Molar Mass of Compounds. Ex. Molar mass of CaCl 2 Avg. Atomic mass of Calcium = 40.08g Avg. Atomic mass of Chlorine = 35.45g Molar Mass of calcium chloride = 40.08 g/mol Ca + (2 X 35.45) g/mol Cl  _ 110.98 ______ g/mol CaCl 2. 20 C a 40.08. 17 Cl 35.45. Practice.

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Review: Molar Mass of Compounds

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  1. Review: Molar Mass of Compounds • Ex. Molar mass of CaCl2 • Avg. Atomic mass of Calcium = 40.08g • Avg. Atomic mass of Chlorine = 35.45g • Molar Mass of calcium chloride = 40.08 g/mol Ca + (2 X 35.45) g/mol Cl _110.98______ g/mol CaCl2 20 Ca40.08 17Cl 35.45

  2. Practice • Calculate the Molar Mass of calcium phosphate • Formula = • Ca3(PO4)2 Masses elements: Ca = 40.08g/mole P = 30.97 g/mole O = 16.00 g/mole • Molar Mass = (40.08 g/mole)(3) + (30.97 g/mole)(2) + (16 g/mole)(8) = 310.18 g/mole

  3. Mole Conversions

  4. Atoms or Molecules Divide by 6.02 X 1023 Multiply by 6.02 X 1023 Moles Multiply by atomic/molar mass from periodic table Divide by atomic/molar mass from periodic table Mass (grams)

  5. Review • 5.7 kg = ?? mg

  6. 3.5 dozen roses = ?? Roses • 2.5 mol roses = ?? Roses (use Avogadro's #)

  7. Practice • Find the mass of 0.89 mol of CaCl2. • Find the molar mass of the compound: • Make the conversion:

  8. Practice • A bottle of PbSO4 contains 158.1 g of compound. How many moles of PbSO4 are in the bottle?

  9. Calculations molar mass Avogadro’s numberGrams Moles particles/formula units/atoms Everything must go through Moles!!!

  10. Practice • Determine the number of atoms that are in 0.58 mol of Se.

  11. Practice • How many moles of barium nitrate (BaNO3) contain 6.80 x 1024 formula units?

  12. Calculations molar mass Avogadro’s numberGrams Moles particles/formula units/atoms Everything must go through Moles!!!

  13. 2.5 g Roses = ?? Roses • Atomic mass of 1 Rose is 3.0 g/mol

  14. Multi-step Practice • How many molecules are in 5.1g of TiO2?

  15. Multi-step Practice • If you burned 6.10 x 1024 molecules of ethane (C2H6), what mass of ethane did you burn?

  16. Molar Volume • Definition: The volume of one mole of an ideal gas at standard conditions (STP) equal to 22.4 L. • STP = standard temperature and pressure which is 0ºC and 1 atmospheric pressure • 1 mole gas at STP = 22.4 L

  17. Practice • A container with a volume of 893L contains how many moles of air at STP?

  18. Practice • A chemical reaction produced 0.37 mol of N2 gas. What volume will the gas occupy at STP?

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