Chapter 10 the mole avogadro s number
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Chapter 10 - The Mole & Avogadro’s Number. Measuring Matter Sections 10.1  10.3. Measuring Matter/Counting Units. One pair = 2 (boots, shoes) One dozen = 12 (eggs, donuts, roses) One gross = 144 (pencils) One ream = 500 (sheets of paper).

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Chapter 10 - The Mole & Avogadro’s Number

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Chapter 10 the mole avogadro s number

Chapter 10 - The Mole & Avogadro’s Number

Measuring Matter

Sections 10.1  10.3


Measuring matter counting units

Measuring Matter/Counting Units

One pair = 2

(boots, shoes)

One dozen = 12 (eggs, donuts, roses)

One gross = 144 (pencils)

One ream = 500 (sheets of paper)


Measuring a mole units used to count particles

Measuring a Mole – units used to count particles

  • 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


How big is a mole

How Big is a Mole?

  • 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


History of avogadro s number

History of Avogadro’s Number

  • 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


The law of conservation of mass

The Law of Conservation of Mass

  • 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


The law of definite proportions and ratios of atoms

The Law of Definite Proportions and Ratios of Atoms

  • 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


Relationships between moles atoms and the gram mole

Relationships between moles, atoms and the gram mole

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


In conclusion

In Conclusion:

  • 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


Moles particles conversion

x 6.02 x 1023

Moles

Particles

Atoms, molecules, ions, formula units

÷ 6.02 x 1023

Moles Particles Conversion


Example problems

  • Convert 3.5 moles to atoms

  • Convert 18.06 x 1023 atoms to moles

Example Problems:


Convert from moles to particles

Convert from moles to particles

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


Convert from particles to moles

Convert from particles to moles

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


You try these

You try these…

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


Homework complete on another sheet of paper showing your work

HomeworkComplete on another sheet of paper showing your work!

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


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