1. Stoichiometry AP Chemistry In the thermite reaction, a mixture of powdered aluminum and powdered iron(III) oxide react to yield iron and aluminum oxide. The reaction burns hot enough to be useful in under- water welding. 2 Al + Fe 2 O 3  2 Fe + Al 2 O 3 + energy

2. In a reaction: atoms are rearranged AND mass energy charge are conserved Balancing Chemical Equations = law of conservation of mass same # of atoms of each type on each side of equation Hint: Start with most complicated substances first and leave simplest substances for last. Chemical Equations

3. 2 Solid lithum reacts w /oxygen to form solid lithium oxide. O 2 (g) Li(s) Li 2 O(s) + Li + O 2– + 4 Aqueous aluminum sulfate reacts w /aqueous barium chloride to form a white precipitate of barium sulfate. The other compound remains in solution. Al 3+ SO 4 2– Ba 2+ Cl – Al 2 (SO 4 ) 3 (s) + BaCl 2 BaSO 4 AlCl 3 (aq) + 332

4. Methane gas (CH 4 ) reacts with oxygen to form carbon dioxide gas and water vapor. CH 4 (g) + O 2 (g) CO 2 (g) H 2 O(g) + 22 Furnaces burn primarily methane. CaSi 2 + SbI 3 Si + Sb + CaI 2 Al + CH 3 OH Al(CH 3 O) 3 + H 2 CaC 2 (s) + H 2 O(l) C 2 H 2 (g) + CaO(s) 32263 3 26 2 3

5. 2 C 2 H 2 (g) + O 2 (g) CO 2 (g) + H 2 O(l) 5 42 2 C 3 H 8 + O 2 CO 2 + H 2 O 534 Complete combustion of a hydrocarbon, or of a compound containing C, H, and O (e.g., methanol, CH 3 OH) yields CO 2 and H 2 O. C 4 H 10 + O 2 CO 2 + H 2 O 13 4 5 2 8 10 Another pattern of reactivity: e.g., alkali metal hydroxide hydrogen gas water++ 2 Rb(s) + 2 H 2 O(l)  2 RbOH(aq) + H 2 (g)

6. 2 C 2 H 2 (g) + O 2 (g) CO 2 (g) + H 2 O(l) 5 42 C 3 H 8 + O 2 CO 2 + H 2 O 534 Complete combustion of a hydrocarbon, or of a compound containing C, H, and O (e.g., methanol, CH 3 OH) yields CO 2 and H 2 O. C 4 H 10 + O 2 CO 2 + H 2 O 13 2 8 10 Another pattern of reactivity: e.g., alkali metal hydroxide hydrogen gas water++ 2 Rb(s) + 2 H 2 O(l)  2 RbOH(aq) + H 2 (g)

7. Two (of the several) Types of Reactions combination (synthesis): simpler substances combine to form more complex substances sodium + chlorine gas sodium chloride A + B  AB AB + C  ABC A + B + C  ABC Na Cl 2 + NaCl22 -- form:

8. decomposition: complex substances are broken down into simpler ones lithium chlorate lithium chloride + oxygen water hydrogen gas + oxygen gas Li + ClO 3 – Li + Cl – LiClO 3 LiCl + O 2 2 2 3 H 2 O 2 H 2 + O 2 2 -- form: AB  A + B ABC  AB + C ABC  A + B + C

9. formula weight: the mass of all of the atoms in a chemical formula (unit is amu) -- If the substance is a molecular substance (e.g., C 3 H 8 ), then the term molecular weight is also used. molar mass: the mass of one mole of a substance (unit is usually grams) -- recall that 1 mole of any substance 6.02 x 10 23 particles of that substance =

10. formula weight: the mass of all of the atoms in a chemical formula (unit is amu) -- If the substance is a molecular substance (e.g., C 3 H 8 ), then the term molecular weight is also used. molar mass: the mass of one mole of a substance (unit is usually grams) -- recall that 1 mole of any substance 6.02 x 10 23 particles of that substance =

11. (NH 4 ) 3 PO 4 H: 12 (1.0 g) = 12.0 g N: 3 (14.0 g) = 42.0 g m.m. = 149.0 g P: 1 (31.0 g) = 31.0 g NH 4 + PO 4 3– O: 4 (16.0 g) = 64.0 g Find the molar mass and formula weight of ammonium phosphate. f.w. = 149.0 amu

12. percentage composition: the mass % of each element in a compound % of element = g element molar mass of compound x 100 Find the percentage of oxygen, by mass, in calcium nitrate. Ca(NO 3 ) 2 % O == 58.5% O equation:

13. Empirical Formula and Molecular Formula Compound Molecular Formula Empirical Formula glucoseC 6 H 12 O 6 propaneC3H8C3H8 butaneC 4 H 10 naphthaleneC 10 H 8 sucroseC 12 H 22 O 11 octaneC 8 H 18 lowest-terms formula shows the true number and type of atoms in a m’cule CH 2 O C3H8C3H8 C2H5C2H5 C5H4C5H4 C 12 H 22 O 11 C4H9C4H9

14. “What’s your flavor of ice cream?” Finding an Empirical Formula from Experimental Data 1. Find # of g of each element. 2. Convert each g to mol. 3. Divide each “# of mol” by the smallest “# of mol.” 4. Use ratio to find formula.

15. A ruthenium/sulfur compound is 67.7% Ru. Find its empirical formula. RuS 1.5 Ru 2 S 3

16. A sample of a compound contains 4.63 g lead, 1.25 g nitrogen, and 2.87 g oxygen. Name the compound. PbN 4 O 8 Pb(NO 2 ) 4 Pb ? 4 NO 2 – lead(IV) nitrite ? ?