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The Mole

The Mole. The mole is:. A very large number Used to count large numbers of small things including: Atoms of elements Molecules of molecular compounds Formula units of ionic compounds. One Mole of:. Eggs would cover the Earth to a depth of about 6 km ( 4 miles)

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The Mole

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  1. The Mole

  2. The mole is: • A very large number • Used to count large numbers of small things including: • Atoms of elements • Molecules of molecular compounds • Formula units of ionic compounds

  3. One Mole of: • Eggs would cover the Earth to a depth of about 6 km ( 4 miles) • Rice grains would occupy a cube about 193 km (120 miles) on each side • Ice hockey pucks would be equal in mass to that of the Earth (1 puck=160 g) • Basketballs would just about fit perfectly into a plastic bag the size of the Earth.

  4. If: • Someone had a mole of 5 peso coins and decided to buy kite string at the cost of 500,000 pesos per cm, the string would stretch the earth one million times and then to the moon and back another twenty thousand times. Enough would be left over to sell back at 5 pesos per cm and then have enough money to buy every man, woman and child in Chile a new car.

  5. If: • You started counting when you first learned to count and counted by ones, eight hours a day five days a week, for 50 weeks a year, you could retire from counting at the age of 65 as a good counter. • This number is close to the world pop. If all the people now living were to count until they retired at 65, all of them together could ONLY count all the atoms of iron in the head of a straight pin. This same army of counters could count all the leaves on all the trees bushes and shrubs on Earth in about two months

  6. Mole vs. Cells • Assuming that each human has 60 trillion body cells and that the earth’s population is about 7 billion: • The total number of living human body cells on earth is less than one half of a mole

  7. One mole is: • Equal to the molar mass (Mr) of an element or a compound • Equal to 22.4 L of an ideal gas at standard temperature and pressure (STP conditions) • Equal to6.02 x 10 23 atoms of an element molecules of a compound formula units of an ionic compound

  8. Molar mass • Abbreviated Mr • The mass of an element or a compound that is equal to one mole of that element or compound • 1 Mr = 1mole • Ex: The Mr of Iron is ________ • Units are grams/mole or g/mol • Round all units from table to 2 decimal places

  9. Molar Mass practice • 1. NaCl 11. Cu(NO3)2 2. H2SO4 12. KMnO4 3. KNO3 13. H2O2 4. CaCl2 14. H3PO4 5. C2H6 15. (NH4)3PO4 6. Ba(OH)2 16. Fe2O3 7. NH4Br 17. NaC2H3O2 8. Ca3(PO4)2 18. Mg(C2H3O2)2 9. Al2(SO4)3 19. Hg2Cl2 10. Mg(NO3)2 20. K2SO3

  10. Check.. The units are in grams/mole • 1) 58.45 11) 189.57 2) 98.09 12) 158.04 3) 101.11 13) 34.02 4) 110.98 14) 98.00 5) 30.08 15) 149.12 6) 171.35 16) 159.70 7) 97.95 17) 82.05 8) 310.18 18) 142.41 9) 342.17 19) 472.08 10) 148.3 3 20) 158.27

  11. Mass – Mole Practice Calculate the grams present in: • 0.200 moles of H2S 2) 0.100 moles of KI 3) 1.500 moles of KClO3

  12. Mass/Mole Practice Calculate the grams present in: 1) 0.200 moles of H2S = 6.82 grams 2) 0.100 moles of KI = 16.6 grams 3) 1.500 moles of KClO3 =182.8 grams

  13. Find the mass in grams of: 4) 0.750 moles of NaOH = 30.0 grams 5) 3.40 x 10-5 moles of Na2CO3 = 3.60 x 10-3 gram or 0.00360

  14. Mole/Mass PracticeConvert the following to moles 1) 2.00 grams of H2O 2) 75.57 grams of KBr 3) 100. grams of KClO4

  15. Mole/Mass Practice 1) 2.00 grams of H2O = 0.111 mole 2) 75.57 grams of KBr = 0.6350 mole 3) 100.0 grams of KClO4 = 0.722 mole

  16. Convert the following into moles: 4) 8.76 grams of NaOH = 0.219 mole NaOH 5) 0.750 grams of Na2CO3 = 7.08 x 10-3 mole 0.00708 mole

  17. Convert the following from moles into particles • Calculate the number of molecules in 1.058 mole of H2O 2) Calculate the number of atoms in 0.750 mole of Fe 3) Why is #1 asking for molecules and #2 for atoms?

  18. Answers • Calculate the number of molecules in 1.058 mole of H2O = 6.369 x 1023 molecules 2) Calculate the number of atoms in 0.750 mole of Fe = 4.52 x 1023 atoms

  19. Convert the number of particles into moles • How many moles are there in 1.806 x1024 molecules of water? • How many moles are there in 3.01 x1022 atoms of copper?

  20. Answers • How many moles are there in 1.806 x1024 molecules of water? = 3.0 moles of water 2) How many moles are there in 3.01 x1022 atoms of copper? = 0.05 moles of copper

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