1. Wake-up Al + H 2 SO 4  Al 2 (SO 4 ) 3 + H 2 1.Balance the equation above. 1.How many grams of H 2 SO 4 will react with 18g of Al?

2. STOICHIOMETRY What does volume have to do with stoichiometry?

3. Stoichiometry Problem Inventory How many moles of Ammonia could I make from 3 moles of Nitrogen? _____ N 2 (g) + _____H 2 (g)  ______ NH 3 (g) 132 Given: 3 mol N 2 mol N 2 mol NH 3 1 2 6 mol NH 3 = Mole to Mole Problems Given = Moles Unknown = Moles

4. Stoichiometry Problem Inventory How many grams of Ammonia will be produced from 3 grams of Nitrogen? _____ N 2 (g) + _____H 2 (g)  ______ NH 3 (g) 132 Given:3g N 2 g N 2 mol NH 3 1 28 5.1 g NH 3 = Mass and Moles Problems Given = Mass Unknown = Mass Mass to Mass/Moles Problems Given = Mass Unknown = Moles Mass to Mass/Moles Problems Given = Moles Unknown = Mass mol N 2 1 1 3 mol NH 3 g NH 3 16

5. Converting Mass to Mass Problems Use Road Map Provided Follow Directions – like following a recipe!

6. STP Standard Temperature and Pressure The standard temperature is 273 K (0° Celsius) and the standard pressure is 1 atm (atmosphere) pressure.

7. STP and Moles At STP, one mole of gas occupies 22.4 L of volume.

8. Conversion Factor for Volume at STP and Moles

9. Example #1 _____ N 2 (g) + _____H 2 (g)  ______ NH 3 (g) 132 Given:25g N 2 g N 2 mol NH 3 1 28 40.0L NH 3 = Mass to Volume mol N 2 1 1 3 mol NH 3 L NH 3 22.4 What volume of NH 3 at STP is produced if 25g of N 2 is reacted with an excess of H 2 ?

10. Example #2: What volume of hydrogen at STP is produced when 2.5g of zinc react with an excess of hydrochloric acid? ___ Zn + ___ HCl  ___ ZnCl 2 + ___ H 2 112 Circle the known. Box what you are trying to find. 2.5 g Zn g Zn mol Zn 65.4 1 mol Zn mol H 2 1 1 L H 2 1 22.4 = 0.85 L H 2 1