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 https://www.youtube.com/watch?v=TEl4jeETVmg

Avogadro’s Number 6.02x1023

Mole A mole is just a number like… Pair = 2 Trio = 3 mole = (mol) 602000000000000000000000 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

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

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

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

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

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!

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.

Mole Song https://www.youtube.com/watch?v=PvT51M0ek5c

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 10 23 C atoms = 12g C

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

Stoichiometry of Chemical Formulas

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

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!

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?

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

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

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

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!

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!

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

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

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!

Examining Molar Relationships in Balanced Equations 6CO2 + 12 H2O + 2804kJ  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

Mole - Mole Relationships Practice

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