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I. Converting between Particles and Moles II. Converting Between Mass and Moles

I. Converting between Particles and Moles II. Converting Between Mass and Moles. The Mole. B . Converting Moles to Particles. Suppose you want to determine how many particles of sucrose are in 3.50 moles of sucrose. You know that one mole contains 6.02 x 10 23 representative particles.

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I. Converting between Particles and Moles II. Converting Between Mass and Moles

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  1. I. Converting between Particles and MolesII. Converting Between Mass and Moles The Mole

  2. B . Converting Moles to Particles • Suppose you want to determine how many particles of sucrose are in 3.50 moles of sucrose. You know that one mole contains 6.02 x 1023 representative particles. • Therefore, you can write a conversion factor, Avogadro’s number, that relates representative particles to moles of a substance.

  3. B. Converting Moles to Particles • You can find the number of representative particles in a number of moles just as you can find the number of roses in 3.5 dozen. • For sucrose, the representative particle is a molecule, so the number of molecules of sucrose is obtained by multiplying 3.50 moles of sucrose by the conversion factor, Avogadro’s number.

  4. B. Converting Moles to Particles • There are 2.11 x 1024 molecules of sucrose in 3.50 moles.

  5. B. Converting Particles to Moles • Now, suppose you want to find out how many moles are represented by a certain number of representative particles. • You can use the inverse of Avogadro’s number as a conversion factor.

  6. B. Converting Particles to Moles • Example: • Zinc is used as a corrosion-resistant coating on iron and steel. It is also an essential trace element in your diet. • Calculate the number of moles that contain 4.50 x 1024 atoms of zinc (Zn).

  7. B. Converting Particles to Moles • Multiply the number of zinc atoms by the conversion factor that is the inverse of Avogadro’s number. 1 mole Zn = 4.50x1024 atoms Zn X 6.02x1023 atoms Zn = 7.48 mol Zn

  8. Question 1 Calculate the number of molecules in 15.7 mol carbon dioxide. Answer 9.45 x 1024molecules of CO2

  9. Question 2 Calculate the number of moles in 9.22 x 1023 atom iron. Answer 1.53 mol Fe

  10. A. Converting Mass to Moles • A roll of copper wire has a mass of 848 g. • How many moles of copper are in the roll? • Use the atomic mass of copper given on the periodic table to apply a conversion factor to the mass given in the problem.

  11. A. Converting Mass to Moles 1 mole Cu 848 g Cu X 13.4 mol Cu = 63.5 g Cu

  12. B. Converting Moles to Mass • Calculate the mass of 0.625 moles of calcium. • Use the molar mass of calcium to apply a conversion factor to the number of moles given in the problem.

  13. B. Converting Moles to Mass • According to the periodic table, the atomic mass of calcium is 40.078 amu, so the molar mass of calcium is 40.1g/mole.

  14. B. Converting Moles to Mass 0.625 mol Ca X 40.1 g Ca 25.1 g Ca = 1 mol Ca

  15. Question 3 Calculate the mass of 6.89 mol antimony. Answer 839g Sb

  16. Question 4 A chemist needs 0.0700 mol selenium for a reaction. What mass of selenium should the chemist use? Answer 5.53g Se

  17. Question 5 Calculate the number of moles in 17.2 g of benzene (C6H6). Answer 0.220 mol C6H6

  18. C. Converting Mass to Number of Particles • According to data from the periodic table, the molar mass of lead is 207.2 g/mol. Apply a conversion factor to convert mass to moles. 1 mole Pb 4.77 g Pb X 207.2 g Pb

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