2. How big is a mole. (Not the animal, the other one
How big is a mole? (Not the animal, the other one.) - Daniel Dulek TED TALK

3. Avogadro’s Number
6.02x1023

4. Mole A mole is just a number like… Pair = 2 Trio = 3
mole = (mol)
Mole
A mole is just a number like…
Pair = 2 Trio = 3
Dozen = 12 Baker’s dozen = 13
Gross = 144 Score= 20
Century=100 Ream=500
Pair, trio
Dozen, baker dozen
Gross, score
Century, ream
mole

5. How BIG is a mole? 9.12 x 1013 There are ~ 6.6 billion people on Earth
How many Earths would it take to equal the population
of 1 mole?
9.12 x 1013

6. If you spent $800 billion dollars a day how many years would it take to spend a MOLEion dollars?
2.06 x 109 years

7. If you had a mole of cats . . . They would create a sphere larger than
Earth!

9. NO!  If you had a mole of H2O could you swim in it?
Water molecules are so small
that a mole of H2O = 18ml

10. In chemistry we don’t work with individual atoms or molecules because they are too small to be weighed or measured
We have to work with LOTS of atoms in order to measure them
THAT’s WHERE THE
MOLE COMES IN!

11. How small are atoms?
There are more atoms in one gram of salt than grains of sand on all the beaches
of all the oceans in all
the world.

13. Mole Song

14. of the in
Gram ATOMic Mass
mass is in grams of 1 mole of atoms of an element
In other words……
1 mol C atoms = 6.02 x C atoms = 12g C

15. Practice Remember. 1 mole = 6
Practice Remember mole = 6.02x1023 atoms or molecules = ______ g from the periodic table

16. Stoichiometry of Chemical Formulas

17. Gram Formula Mass Gram Molecular Mass Molar Mass
of the in
Gram Formula Mass Gram Molecular Mass Molar Mass
mass in grams of 1 mole of a substance
In other words Add it all up!
1 mole of NaCl = 58g = 6.02x1023 particles of NaCl
1 mole of H2O = 18g = 6.02x1023 molecules of H20

18. Now….. Use the gram formula mass and the gram atomic mass to determine
how many moles or atoms of an element are found in some mass of a substance
how much mass that element contributes to the mass of the entire substance
Use factor label & follow the units!

19. Stoichiometry of Chemical Formulas
If you have 1 molecule of (NH4)2SO4
How many atoms of N are there?
How many atoms of H? S? O?
Total weight?

20. Practice Remember. 1 mole = 6
Practice Remember mole = 6.02x1023 atoms or molecules = ______ gfm from the pt

21. Gases ONLY Molar Volume @STP 1 mole of ANY gas O2 (g) NH3 (g) He (g)
contains 6.02 x 1023 molecules and
occupies a volume of 22.4L

22. standard temperature & pressure
STP
standard temperature & pressure
0oC or 273K
101.3kPa or 1 atm

23. Remember . . . 1 mole of O2(g) = 32g 1 mole of NH3(g) = 17g
Gases also have mass
1 mole of O2(g) = 32g
1 mole of NH3(g) = 17g
 we can calculate Density!

24. D = m/v
A sample of oxygen contains 3 moles of particles at STP what is its density?
2 steps
Convert moles to mass AND volume
Calculate density
If mass or volume is given, use it and convert the other……. THEN calculate D!

25. 1 mole = 6.02x1023 atoms or molecules = gfm = 22.4L (g)
Remember . . .
1 mole = 6.02x1023 atoms or molecules = gfm = 22.4L (g)

26. Stoichiometry of Chemical Equations
The study of quantitative relationships that can be derived from chemical equations.
“it’s a simple matter
of weight ratios . . .”

27. Stoichiometry cookies
If you look at chemical equations as recipes it may be easier to understand that
changing the amount of a reactant will change the amount of the product IN THE SAME RATIO!

28. Examining Molar Relationships in Balanced Equations
6CO H2O kJ  6O2 + C6H12O6 +6H20
Balanced equations
Law of conservation of mass / matter
ATOMS are not created or destroyed during a chemical reaction, they are only rearranged to form new substances.
# atoms on reactant side = # atoms on product side
Law of conservation of E
E on the reactant side = E on the product side

29. Mole - Mole Relationships
Practice

30. The End