The Mole!

1
The Mole!

• Also Known As
• The single most terrifying,
• horrific, scariest chemistry
• concept of the modern world.

2
What is a Mole?

• The term mole means a specific amount of a
  substance in chemistry. The amount that the mole
  is equal to is 6.02x1023.
• That is 602,000,000,000,000,000,000,000! We will
  use the scientific term since paper and ink costs
  us money and its not as hard on your hand.
• Think of the mole like you would the words
  dozen and pair they are words that mean a
  specific amount of something 12 and 2
  respectively. The mole just means a really big
  number and you could have a mole of anything
  atoms, molecules, tennis balls, donkeys, pencils,
  etc
• 6.02x1023 is called Avogadros number he was
  the guy that came up with it and realized its
  usefulness in the field chemistry.
• The symbol for the mole is mol Can you
  believe that?!?!
• Poor letter epoor lazy chemists.

3
Whats So Great About the Mole?

• The mole is incredibly useful in carrying out
  reactions and calculations in chemistry because a
  mole of any element or compound will weigh the
  same as its mass (in grams) as per the masses on
  the periodic table.
• What?!?!?!
• Look at it this wayThink of holding a small
  amount of carbon in your handsWell
• 1 mole of C 6.02x1023 atoms of C 12.01g of C
• It works the same way with molecules and/or
  compoundsThink of a small glass of water
• 1 mole of H2O 6.02x1023 18.02g of H2O
• (H2O 1.01 1.01 16.00 18.02)

4
The Mole You Know

• You learned (not learnt) in the chemistry unit
  of grade 10 science that you must balance all
  chemical equations. This was to satisfy the Law
  of Conservation of Mass what goes in
  (reactants), must come out (products).
• The coefficients you placed in the equation are
  the number of moles you need of each substance
  for the reaction to occur efficiently both
  reactants used up no leftover waste.
• Example The decomposition of water.
• 2H2O ? 2H2 O2
• This means that 2 moles of water will break apart
  to give us 2 moles of hydrogen gas and 1 mole of
  oxygen gas.

5
Conversions Particles Moles

• To convert between particles and moles you need
  to know that one mole is equal to 6.02x1023
  particles.
• The conversion factor here is 6.02x1023
  particles/mol.
• The following may help you
• by 6.02x1023 particles/mol
• of particles of moles
• x by 6.02x1023 particles/mol

6
Calculating Mass Using Moles

• Also Known As
• The Massive Return of the Mole People!!!

7
Molar Mass?

• The molar mass of a substance is the mass (g) of
  one mole of the substance.
• Basically, it is the mass (in grams) of 6.02x1023
  particles of a substance.
• Therefore, it would only make sense that the
  units for molar mass would be in grams/mole or
  g/mol.

8
Converting Moles to Grams

• To convert the number of moles you have into
  grams, or vice-versa, you need to know the molar
  mass of the substance you are dealing with.
• To get the molar mass of a substance, you have to
  add up the masses of all the parts of that
  substance using the atomic masses from the
  periodic table.
• For example C2H6 2(12.01) 6(1.01)
  30.08g/mol.
• Now we can use this molar mass much like we used
  Avogadros number in the previous conversions
  between particles and moles.
• x by g/mol
• of moles (mol) mass (g)
• by g/mol

9
The Big Picture

• We can nowand take pride in this
• go from particles ? moles vice versa.
• and go from moles ? mass vice versa.
• SoWe could go from particles to mass (or mass to
  particles) by using two steps.
• by 6.02x1023 particles/mol x by g/mol
• of particles of moles mass (g)
• x by 6.02x1023 particles/mol by g/mol

10
Holy Mole-y!

• Now you are ready to conquer the world of the
  mole!
• Just make sure that your answers make sense and
  you have used the correct units in your answers.
• NowGet to work!

11

• THE END!