 What do the following all have in common? DDozen CCouple FFew BBaker’s Dozen TTen.

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Presentation transcript:

 What do the following all have in common?

DDozen CCouple FFew BBaker’s Dozen TTen

 Mole- counting unit standing for 6.02 x particles  Tells us how many particles of a compound are actually involved in a reaction  1 mole = 6.02 x particles 602,000,000,000,000,000,000,000 particles Avogadro’s Number

 1 mole of water = how many particles?  1 mole of sugar = how many particles  6.02 x particles = how many moles?

 A dozen eggs would make a HUGE omelet!  A mole of eggs would make an omelet big enough to cover the Earth thirty times!

 Atoms and Molecules are TINY!  A drop of water contains 10 trillion water particles!

 6.02 x makes a chemist’s life a lot easier  It’s impossible to keep track of one atom  so scientist discovered this number that gives us the molar mass of an atom  Molar mass is the mass of 6.02 x particles of a given substance  Mass is given in grams

 We don’t always have exactly 1 mole, though.  When we have different amounts of moles, we can convert between atoms and moles

MolesParticles Multiply by Avogadro’s Number Divide by Avogadro’s Number

 A lab experiment calls for 2.00 moles of Calcium. How many particles of Calcium are required?  How can we solve this?  Dimensional Analysis! ▪ ID what we’re given and what the question’s asking for and set up the T-Chart 2 moles Calcium 1 mole Calcium 6.02 x particles

 You have 12.04x10 23 atoms of sulfur. How many moles of sulfur do you have?

 Molar Mass = the mass of 1 mole of a substance  Tells us what mass of a substance is used in a reaction

Molar mass: mass of 1 mole of in grams 1 mole C atoms = ___________ particles 1 mole of C atoms has a molar mass of_________ g. Molar mass of O = ___________ Molar mass of Li = ____________ For any element, the Molar Mass = Mass Number 3.2

What is the mass of one mole of: C S Cu Fe Hg 3.2

1) Count out the atoms in the compound 2) Look up the Molar Mass for each element 3) Multiply the Molar Mass of each element by the # present in the compound 4) Sum the Molar Masses

 No more than 4 at a station  10 min at each station max  If completed before 10 min is up, check answers up at the front  Use your station buddies for help before asking Ms. Herndon!

 NO2  SO 2  (NH 4 ) 3 PO 4  C 6 H 12 O 6

1) How many particles are in a mole? 2) Determine the Molar Mass for the following problems. Don’t forget your UNITS! a. Helium (He) b. KCl 4 c. Cu(OH) 2

 If I had 20 Dollars, and the cost of one pair of kicks is 4 dollars for 1 pair, how many pairs could I have? 20 Dollars 4 Dollars 1 pair(20/4) pairs5 pairs Now... What’s my conversion factor? What unit am I given? What unit is the question asking for?

 If I had 20 grams of helium, and one mole of helium is 4 grams, how many moles of helium could I have? 20 grams He 4 grams He 1 mole He(20/4) moles He5 moles He What’s my conversion factor? What unit am I given? What unit is the question asking for?