Warm Up #6 Balance the following: __H3PO4(aq) + __NaOH(aq)  __HOH(ℓ) + __Na3PO4(aq) Write the noble gas notation Silver (Ag), and also write the orbital notation (the arrows) for it. You are given 89.6 grams of Fe2O3. How much of this amount is purely Iron (Fe)?

Chapter 12.1 Stoichiometry

Stoichiometry…big word, review topic Why we balance? Law of Conservation of Mass (mass/matter can not be created/destroyed) Stoichiometry – using balanced equations to find out how much product is formed from reactants How? MOLE-to-MOLE RATIOS

Ex. 3H2(g) + N2(g)  2NH3(g) Mole to Mole Ratio – the amount of moles of one thing compared to the other. __ to __ ratio USE COEFFICIENTS H2 to NH3 ratio = 3 to 2 ratio H2 to N2 ratio = 3 to 1 ratio

Ex. 3H2(g) + N2(g)  2NH3(g) (at STP) what this equation tells us Ratio: 3 mol H2 to 1 mol N2 to 2 mol NH3 Mass: 3(2.02 g) + (28.02 g) = 2 (17.04 g) 34.08 g = 34.08 g Volume: 3 mol H2 = (3 x 22.4L) = 67.2 L H2 H2 N2 NH3

Converting: Grams H2 into mol NH3 3H2(g) + N2(g)  2NH3(g) You are given: 34 grams H2. How many mol NH3 are made? USE T-CHARTS. Start with 34 grams H2 Convert into mol (ALWAYS). (1 mol H2 = 2.02 g) Periodic table Mole to Mole Ratio (3 mol H2 = 2 mol NH3) Balanced equation DONE

Grams A to Grams B Flow Chart Moles A Moles B

Grams A to Grams B T-Chart Moles A Moles B Grams B Grams A Grams A Moles B Moles A Mole to Mole Ratio Given Periodic Table Periodic Table