1. Get out your notes and locate the following problem: 896 dL of CO 2 gas contains how many atoms? 2.4e24 Day 4 10-3

2. Activity Series Lab Day 4 10-3

3. Propose an activity series based on the following results: A + BY  AY + B A + CY  NO RXN Day 5 10-4 A > B C > A CABCAB

4. CHAPTER QUIZ FRIDAY 10-7!!! Day 5 10-4

5. Read pages 360-361 AND complete # 15 on page 361. Day 4 10-3 Fe (s) + Pb(NO 3 ) 2(aq)  Fe(NO 3 ) 2(aq) + Pb (s) Ca (s) + 2H 2 O (l)  H 2(g) + Ca(OH) 2(aq) Cl 2(aq) + 2NaI (aq)  2NaCl (aq) + I 2(aq) Zn (s) + H 2 SO 4(aq)  ZnSO 4(aq) + H 2(g)

6. Percentage Composition Mass of element Mass of compound X (100) = % element in compound … tells how much an element contributes to the mass of the compound

7. Percentage Composition H 2 O??? 2 H: 2 * 1.0079 g = 2.0158 g 1 O: 1 * 15.999 g = 15.999 g 18.015 g (2.0158 g / 18.015) X 100 = 11.190% H (15.999 g / 18.015) X 100 = 88.810% O

8. Percentage Composition An unknown compound w/ a mass of 0.237 g is extracted from the roots of a plant. Decomposition of the sample produces 0.0948 g of C, 0.1264 g of O, and 0.0158 g of H. What is the % composition of the compound?

9. Day 6 10-5 0.112 kL of CO gas contains how many grams? How many atoms? 140 grams CO 6e24 atoms

10. Review (if needed) pages 325-327 AND complete #s 33, 34, 35, and 36 on pages 326 and 327. Day 5 10-4

11. Empirical formula – smallest whole- number mole ratio for a compound Empirical Formulas To Calculate: 1. Convert all elements involved to moles 2. Divide all elements by the smallest # of moles 3. Obtain smallest whole #ed ratio

12. A compound contains 13.5 g Ca, 10.8 g O, and 0.675 g H. What is the empirical formula? Empirical Formulas 1. Convert all eles. involved to moles 2. Divide all eles. by the smallest # of moles 3. Obtain smallest whole #ed ratio Ca = 0.337 moles O = 0.675 moles H =.675 moles Ca = 0.337 mols / 0.337 mols = 1 O = 0.675 mols / 0.337 mols = 2 H = 0.675 mols / 0.337 mols = 2 1 Ca : 2 O : 2 H CaO 2 H 2 Ca(OH) 2

13. Calculating Empirical Formulas In an unknown compound you find 4.04 g of N and 11.46 g O. Empirical formula?

14. 67.2 L of CH 4 gas = ___ grams 44.8 mg of solid Carbon = ___ L Day 1 10-6

15. Homework # 2 = now Postlabs = Friday 10-7 (tomorrow) Presentations = Wednesday 10-12 Chapter Quiz = Wednesday 10-12 Day 1 10-6

16. Empirical formula – smallest whole- number mole ratio for a compound Empirical Formulas vs. Molecular Formulas Molecular formula – actual # of atoms of each ele. in a molecular compound Sometimes But not always! the same.

17. Molecular Formulas To Calculate: Compare the molar mass of the empirical formula to the molar mass of the molecular formula Molecular formula – actual # of atoms of each ele. in a molecular compound

18. Determine the molecular formula of the compound with an empirical formula of CH and a formula mass of 78.110 amu Empirical mass = 13.019 g/mol x = 6 Molecular formula = C 6 H 6 Determining Molecular Formulas

19. In an unknown compound you find 4.04 g of N and 11.46 g O. Empirical formula? This unknown compound has a molar mass of 108.0 g/mol. What is the molecular formula? Empirical formula = N 2 O 5 Empirical mass = 108.009 g/mol Molecular formula = N 2 O 5

20. A sample of a compound contains 6.0 g of C and 16 g of O. The total sample is 22 g. The molecular molar mass is 44 grams Percentage Composition Empirical formula Molecular formula Determining Molecular Formulas

21. Review section 10.3 (if needed) and complete #s 45-49 for # 49 the %s can be treated as grams and used to find moles… Assignment due Tuesday 10-11

22. Calculate the mass of Cu produced? Mass of beaker and Cu – mass of beaker

23. Calculating percent yield Percent yield – a way to compare how much you “should” get to how much you actually got Percent Yield = Actual yield Theoretic yield X 100

24. A sample of a compound contains 6.0 g of C and 16 g of O. The total sample is 22 g. Percentage Composition Empirical formula Determining Molecular Formulas Pd. 6

26. - 2 molar mass convs. - 2 Av.’s # convs. - 2 Av.’s law convs. - 2 multi-step convs. - 1 percentage comp. - 1 empirical formula - 1 molecular formula - 3 content ?s (no math) 14 questions

28. Mass of element Mass of compound X (100) = % element in compound H 2 O??? 2 H: 2 * 1.0079 g = ________ g 1 O: 1 * ________ g = _________ g (__________________) X 100 = _______% H (___________________) X 100 = _______% O

29. A compound contains 13.5 g Ca, 10.8 g O, and 0.675 g H. What is the empirical formula? 1. Convert all eles. involved to moles 2. Divide all eles. by the smallest # of moles 3. Obtain smallest whole #ed ratio Ca = 0.337 moles O = 0.675 moles H =.675 moles Ca = 0.337 mols / 0.337 mols = 1 O = 0.675 mols / 0.337 mols = 2 H = 0.675 mols / 0.337 mols = 2 1 Ca : 2 O : 2 H Ca(OH) 2 13.5 g Ca 40 g Ca 1 mol Ca 10.8 g O 16 g O 1 mol O 0.675 g H 1 g H 1 mol H

30. Percentage Composition Empirical formula Molecular formula