AP Chemistry Stoichiometry 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 underwater welding. 2 Al + Fe2O3 2 Fe + Al2O3 + energy Chemical Equations In a reaction: atoms are rearranged mass AND energy are conserved charge 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. Solid lithum reacts w/oxygen to form solid lithium oxide. 4 Li(s) + O2(g) Li+ O2– 2 Li2O(s) + Aqueous aluminum sulfate reacts w/aqueous barium chloride to form a white precipitate of barium sulfate. The other compound remains in solution. Ba2+ Cl– Al3+ SO42– Al2(SO4)3 (aq) + 3 BaCl2 (aq) 3 BaSO4 (s) + 2 AlCl3 (aq) Methane gas (CH4) reacts with oxygen to form carbon dioxide gas and water vapor. Furnaces burn primarily methane. CH4(g) + 2 O2(g) CaC2(s) + H2O(l) CO2(g) + 2 H2O(g) C2H2(g) + CaO(s) 3 CaSi2 + 2 SbI3 6 Si + 2 Sb + 3 CaI2 2 Al + 3 6 CH3OH 2 Al(CH3O)3 + 3 H2 2 C2H2(g) + 5 O2(g) C3H8 + 5 O2 2 C4H10 + 13 O2 2 CO2(g) + 2 H2O(l) 4 3 CO2 + 4 H2O 8 4 CO2 +10 5 H2O Complete combustion of a hydrocarbon, or of a compound containing C, H, and O (e.g., methanol, CH3OH) yields CO2 and H2O. Another pattern of reactivity: alkali metal hydrogen + water + metal hydroxide gas e.g., 2 Rb(s) + 2 H2O(l) 2 RbOH(aq) + H2(g) Two (of the several) Types of Reactions combination (synthesis): simpler substances combine to form more complex substances -- form: A + B AB AB + C ABC sodium + chlorine gas 2 Na + Cl2 A + B + C ABC sodium chloride 2 NaCl decomposition: complex substances are broken down into simpler ones -- form: AB A + B ABC AB + C lithium chlorate Li+ ClO3– 2 LiClO3 water ABC A + B + C lithium chloride + oxygen Li+ Cl– 2 LiCl + 3 O2 hydrogen gas + oxygen gas 2 H2O 2 H2 + O2 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., C3H8), 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 = 6.02 x 1023 particles substance of that substance Find the molar mass and formula weight of ammonium phosphate. NH4+ PO43– (NH4)3PO4 N: 3 (14.0 g) = 42.0 g H: 12 (1.0 g) = 12.0 g P: 1 (31.0 g) = 31.0 g O: 4 (16.0 g) = 64.0 g m.m. = 149.0 g f.w. = 149.0 amu percentage composition: the mass % of each element in a compound equation: g element x 100 % of element = molar mass of compound Find the percentage of oxygen, by mass, in calcium nitrate. Ca(NO3)2 6(16.0) %O= = 58.5% O 40.1 2(14.0) 6(16.0) Empirical Formula and Molecular Formula lowest-terms formula shows the true number and type of atoms in a m’cule Compound Molecular Formula Empirical Formula glucose C6H12O6 CH2O propane C3H8 C3H8 butane C4H10 C2H5 naphthalene C10H8 C5H4 sucrose C12H22O11 C12H22O11 octane C8H18 C4H9 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. “What’s your flavor of ice cream?” A ruthenium/sulfur compound is 67.7% Ru. Find its empirical formula. 1 mol Ru 0.670 mol Ru 0.670 1 67.7 g Ru 101.1 g Ru 1 mol S 1.006 mol S 0.670 1.5 32.3 g S 32.1 g S RuS1.5 Ru2S3 A sample of a compound contains 4.63 g lead, 1.25 g nitrogen, and 2.87 g oxygen. Name the compound. 1 mol Pb 0.0223 mol Pb 0.0223 1 4.63 g Pb 207.2 g Pb 1 mol N 0.0893 mol N 0.0223 4 1.25 g N 14.0 g N 1 mol O 0.1794 mol O 0.0223 8 2.87 g O 16.0 g O ? PbN4O8 ? Pb(NO2)4 Pb? 4 NO2– lead(IV) nitrite
