- 69 Views
- Uploaded on
- Presentation posted in: General

Chapter 10 - The Mole & Avogadro’s Number

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Chapter 10 - The Mole & Avogadro’s Number

Measuring Matter

Sections 10.1 10.3

One pair = 2

(boots, shoes)

One dozen = 12 (eggs, donuts, roses)

One gross = 144 (pencils)

One ream = 500 (sheets of paper)

- Atoms are so tiny chemists count them using a unit of measurement called a “mole”
- 1 mole = 6.02 x 1023 (Avogadro’s Number) atoms/particles/ions/formula units/molecules
- This is a very large number because it measures extremely tiny items
- 602,000,000,000,000,000,000,000

- One mole of pennies would allow every person on Earth to spend a million dollars an hour, day and night, and still have half of it unspent when they died
- One mole of popcorn would cover every dry
surface of the Earth to a depth of six miles

One mole of stacked pennies would reach to the moon and back 16 times

- One mole of marshmallows
would cover the United States

to a depth of 650 miles

- Avogadro: 1811 – equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
- Cannizzaro: 1861 – developed atomic weights for known elements
- Loschmidt: 1865 – determined the number of atoms present in a given volume of air
- Ostwald: 1902 – developed the concept of the mole
- 1971 – the true value, 6.02x1023, was actually determined and is called Avogadro’snumber since the entire string of events started with his findings in 1811

- According to the Law of Conservation of Mass,
Mass of reactants = mass of products

Mass of starting substances = mass of ending substances

- So the production of one water molecule requires 2 hydrogen atoms and 1 oxygen atom.
Therefore:

two atoms of hydrogen + one atom of oxygen 1 water molecule

And

12.04x1023 hydrogen atoms + 6.02x1023 oxygen atoms

6.02x1023 water molecules

- Law of Definite Proportions – atoms combine in small whole number ratios to form compounds
- Example: Water- two atoms of Hydrogen will always combine with one atom of Oxygen to form one molecule of water

The atomic mass ratio of hydrogen to oxygen is 1 amu : 16 amu

The gram mole ratio between hydrogen and oxygen is 1 g : 16 g

So, chemists can determine how many atoms are present in a sample.

One gram of hydrogen would contain exactly 6.02x1023 atoms, or Avogadro’s Number of atoms. Two grams of hydrogen atoms would contain 12.04x1023 hydrogen atoms.

Also, 16 gram moles of oxygen would contain 6.02x1023 atoms.

Therefore: 1 gram of hydrogen = 6.02x1023 atoms = 1 mole

2 grams of hydrogen= 12.04x1023 atoms= 2 moles

16 grams of oxygen= 6.02x1023 atoms= 1 mole

32 grams of oxygen= 12.04x1023 atoms= 2 moles

- 2 atoms of hydrogen + 1 atom of oxygen = 1 water molecule
- 2 amu of hydrogen + 16 amu’s of oxygen = 18 amu’s of water molecules
- 2 g of hydrogen + 16 grams of oxygen = 18 grams of water molecules
- 12.04x1023 atoms H + 6.02x1023 atoms O = 6.02x1023 atoms H2O molecules
- 2 moles of H atoms + 1 mole of O atoms = 1 mole of water molecules

x 6.02 x 1023

Moles

Particles

Atoms, molecules, ions, formula units

÷ 6.02 x 1023

- Convert 3.5 moles to atoms
- Convert 18.06 x 1023 atoms to moles

3) 2.7 moles of lithium

4) 1.8 moles of sodium chloride

5) 5.3 moles of bromine

6) 4.7 moles of potassium oxide

7) 4.32 x 1024 atoms of calcium

8) 2.7 x 1020 atoms of copper

9) 2.5 x 1024 molecules of sodium chloride

10) 5.32 x 1023 molecules of calcium chloride

11) 25 moles to particles

12) 4.08 x 104 particles to moles

13) 0.002 moles to particles

14) 2.3 x 1016 particles

Particles to moles5) 4.32 X 1024

6) 2.70 X 1020 7) 2.50 X 1024 8) 5.32 X 1023

Moles to particles

- 1) 2.7 moles
- 2) 1.8 moles
- 3) 5.3 moles
- 4) 4.7 moles