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Chapter 10 The Mole

Chapter 10 The Mole. Standard # 3: Conservation of Matter and Stoichiometry. This is when it counts!! Help one another!. Calculating Masses of compounds and molecules. 2(N) 2(14.0) +5(O) +5(16.0). N 2 O 5. 108.0amu. K+1. Br - 1. K=39.1 + Br=79.9. KBr. 119.0amu. Al+3.

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Chapter 10 The Mole

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  1. Chapter 10The Mole Standard # 3: Conservation of Matter and Stoichiometry

  2. This is when it counts!! Help one another!

  3. Calculating Masses of compounds and molecules 2(N)2(14.0) +5(O)+5(16.0) N2O5 108.0amu K+1 Br -1 K=39.1 + Br=79.9 KBr 119.0amu Al+3 OH-1 Al=27.0 +3(OH)=3(17.0) 78.0amu Al(OH)3 Cu+2 OH-1 Cu= 63.5 2(OH)= 2(17.0) +2(H2O)= 2(18.0) Cu(OH)2 .2H2O 133.5amu

  4. Grams!! Let’s talk about the units… Ounces!! Pounds!! A.M.U!! 1. A.M.U.= _______ ________ __________ Used to determine the mass of : 1 atom or 1 molecule a. 1 atom of Nitrogen = b. 1 molecule of water= Atomic Mass Unit 14.0 amu 18.0 amu

  5. Continuation….amu units NOT USEFUL when measuring because it’s too small!!!

  6. The preferred unit…… G-unit Q: If one atoms is the mass in amu………… the REAL question is: HOW MANY ATOMS WILL IT TAKE TO GET THE SAME NUMERICAL VALUE FOR A MASS IN GRAMS? 2. Grams: More useful because we can measure this unit.

  7. Are you ready for this???? It takes 6.022 X 1023 atoms for the mass to be in grams. We call this number Avogadro’s number

  8. Examples: 1) 6.022 X 1023 atoms of N= 14.0 grams 16.0 grams 2) 6.022 X 1023 atoms of O= 3) 6.022 X 1023 atoms of Ag= 107.9 grams 18.0 grams 4) 6.022 X 1023 molecules of water=

  9. Opening Question 1. Calculate the mass ofone atom/compound of a. Fluorine: b. Magnesium Phosphate: 19.0 amu 262.9 amu 2. Calculate the mass of 6.022X1023atoms/molecules of a. Ca: b. Calcium Hydroxide: 40.1 grams 74.1 grams 3. What’s the difference between amu and grams? Amu is the unit used when measuring the mass of one atom or substance Gram is the unit used when measuring the mass of one 6.022 X 1023 atoms or substances

  10. So, what’s a mole? a quantity of a substance. Dozen donuts = 12 Pair of tickets = 2 Ream of paper = 500

  11. 1 mole = atomic mass of substance = 6.022 X 10 23 atoms, particles, molecules, formula units = 22.4 L for a gas

  12. Examples: 1 mol of H2O= 1 mol of CO2= 1 mol of Ag= 6.022 X 10 23 atoms 6.022 X 10 23 molecules 6.022 X 10 23 molecules 22.4 L 107.9 grams 18.0 grams 44.0 grams

  13. Yeah!! Calculations together! Yeah!!

  14. Get ready! • One sheet of paper • Pencil • I will give you a periodic table. • Be quiet! • Good luck!!

  15. Quiz 1 • The mass unit for one atom is: • The mass unit for Avogadro’s quantity of atoms: • How many atoms are in a mole? 4. How many Liters (for a gas) are in a mole? 5. Please calculate the molar mass for the following: a. Water: b. Cu(OH)2 c. C6H12O6 • If there are 5.85 moles of CO2, how many grams are there? 7. If you have 100.0grams of water, how many molecules are there? Don’t forget units and round mass to nearest tenth!!

  16. Put your pencil away!! Get out a grading pen !!

  17. Total /13 Quiz 1 amu+1 Grams +1 6.022 X 1023 atoms +1 • The mass unit for one atom is: • The mass unit for Avogadro’s quantity of atoms: • How many atoms are in a mole? 4. How many Liters (for a gas) are in a mole? 5. Please calculate the molar mass for the following: a. Water: b. Cu(OH)2 c. C6H12O6 • If there are 5.85 moles of CO2, how many grams are there? 7. If you have 100.0grams of water, how many molecules are there? 22.4 L +1 18.0 g +1 97.5 g +1 180.0 g +1 5.85mol (44.0g) =257 grams (1mol) +1 work +1correct answer +1 unit +1correct answer 100.0 g H2O (1mol) (6.022X1023molecules)= (18.0g) (1 mol) 3.35 X 1024 molecules +1 work +1 unit

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