1. If you started with 130.8 grams of zinc yesterday, how much sulfur would you have wanted? WHY? Day 1 9-28

2. 820 g of Sulfur (S) = __________ mols? 820 g S 32.066 g S 1 mol S = 2.6 * 10 1 mols S x

3. 1.00 * 10 13 atoms of Tin (Sn) = __________ g? 1.00 * 10 13 atoms Sn 118.71 g Sn 1 mol Sn = atoms Sn 6.022 * 10 23 xx

4. Define mole. Explain how a mole is like a counter. Explain how a mole relates to mass.

5. Particles Molecules Atoms Mass (grams) Volume (liters) MOLES Avogadro’s # - 6.022e23 Molar mass Molar Volume – 22.4 L/mol

6. 36 g of C = _______ atoms of C? 36 g C atoms C 1 mol C = 12.0 g C 6.02 * 10 23 1.8e24 atoms C x x

7. Elements = atomic mass – mass of 1 mole  P.T. Compounds = molar mass – mass of 1 mole  simple calculation

8. H 2 (SO) 4 : 2 H: 2 * 1.0079 g = 2.0158 g 4 S: 4 * 32.066 g = 128.26 g 4 O: 4 * 15.999 g = 63.996 g ADD 194.28 g Molar Masses of Molecules

9. 820 g Ba 3 (PO 4 ) 2 = _____ mols Ba 3 (PO 4 ) 2 820 g Ba 3 (PO 4 ) 2 = 1.4 mols Ba 3 (PO 4 ) 2 601.93 g Ba 3 (PO 4 ) 2 1 mol Ba 3 (PO 4 ) 2 x

10. Ba 3 (PO 4 ) 2 : 3 Ba: 3 * 137.33 g = 411.99 g 2 P: 2 * 30.974 g = 61.948 g 8 O: 8 * 15.999 g = 127.99 g ADD 601.93 g Molar Masses of Molecules

11. 64 g O 2 = _____ mols O 2 64 g O 2 = 2 mols O 2 32 g O 2 1 mol O 2 x

12. 8.0 mols Sr(NO 3 ) 2 = _________ molecules Sr(NO 3 ) 2 8.0 mols Sr(NO 3 ) 2 = 6.022 * 10 23 molecules Sr(NO 3 ) 2 1 mol Sr(NO 3 ) 2 4.8 * 10 24 molecules Sr(NO 3 ) 2 x

13. Mole Molar mass Avogadro’s number Molecule Activity series 6.022 * 10 23 g/mol Single replacment reaction Particles, atoms, molecules cation

14. Get out your lab reports! Day 2 9-29

15. A mole is a ___________, plus it relates to ________. ONE MORE THING… IT RELATES TO VOLUME! …FOR GASES counter mass

16. Avogadro’s law: equal volumes of gases at the same temperature and pressure contain equal numbers of molecules 2H 2 (g) + O 2 (g) 2H 2 O(g) 2 moles 1 mole 2 moles 2 volumes1 volume 2 volumes

17. Standard Temperature and Pressure (STP) 1 atm and 273.15K IF conditions are not specified, assume STP

18. Standard molar volume of a gas: the volume occupied by one mole of gas at STP = 22.41410 L = 22.41410 dm 3 Conversion factors: 1 mol22.414L 22.414L 1 mol

19. Particles Molecules Atoms Mass (grams) Volume (liters) MOLES Avogadro’s # - 6.022e23 Molar mass Molar Volume – 22.4 L/mol

20. HOMEWORK

21. Converting: Mass to moles Moles to mass Moles to atoms / molecules / particles Atoms / molecules / particles to moles Moles to liters Liters to moles Changing a substance = = ______________ ___________ = _____________ = ________________

22. A chemical reaction produces 0.0680 mol of oxygen gas. What volume in liters is occupied by this gas sample at STP? 1.52 L O 2

23. A chemical reaction produces 98.0 mL of sulfur dioxide gas at STP. What was the mass (in grams) of the gas produced? 0.280 g SO 2 1 st pd stopped 4-13

24. LAB BONUS – Explanation group???

25. 896 dL of CO 2 gas contains how many atoms? 2.4e24 6 th pd stopped 4-13

26. Front row: 1.204 kg Barium Phosphate = ___ molecules barium phosphate 2 nd row back: 0.141 kg Nitrous acid = ___ molecules Nitrous acid 3 rd row back: 48,100 cg Nitrogen Trichloride = ___ molecules Nitrogen Trichloride 4 th row back + Murtin: 16.22 kg Ferric Chloride = ___ molecules Ferric Chloride

27. 2 nd row back: 3 rd row back: 4 th row back: Front row: 1.204 kg Barium Phosphate = ___ molecules barium phosphate 0.141 kg Nitrous acid = ___ molecules Nitrous acid 16.22 kg Ferric Chloride = ___ molecules Ferric Chloride + Murtin 48,100 cg Nitrogen Trichloride = ___ molecules Nitrogen Trichloride

28. Barium PhosphateNitrous acid Nitrogen Trichloride Ferric Chloride Ba 3 (PO 4 ) 2 HNO 2 NCl 3 FeCl 3 602 g/mol47 g/mol 120.5 g/mol 162 g/mol 1.2e24 molecules Ba 3 (PO 4 ) 2 1.8e24 molecules HNO 2 2.4e24 molecules NCl 3 6.0e25 molecules FeCl 3

29. Homework # 3 Period 1 LAB no notes Period 6 LAB no notes

30. 45 L of hydrogen gas = how many grams? You may work w/ a partner (Do NOT change seats) – GET THE ANSWER!!!

31. Yesterday the reaction would only work if we used specific amounts, but why might those amounts still be important for reactions that work regardless? Zn + S  ZnS

32. 4-6 1.What is molar mass? 2.Where (how) do you find the molar mass of an element?

33. 3-30 1.Why is a mole better than other counters like a dozen? 2.How many grams of nitrogen do you have if you have 2.0 moles?

34. 1. A mole… I. Can count the # of atoms II. Can count the # of molecules III. Can tell you how much mass you have IV. Is a universal unit Choose all that apply! 4-7

35. 1. A mole is a _________, plus it relates to ______. 2. Molar mass of Be(NO 3 ) 2 3. 3.0 grams of Be(NO 3 ) 2 = ___ moles 4. = ___ molecules?

36. 1. 44.8 L of C 2 H 6 gas = ___ moles at STP 2. Explain how you convert grams to # of atoms. 1. Explain how you convert grams to # of atoms.