1. Gas Stoichiometry LAST PHASE OF STOICHIOMETRY, WOOHOO!!!!!

3. Gas Stoichiometry  We have looked at stoichiometry:  1. using masses and molar masses (periodic table walk g/1mole)  2. using molecules (avogardo’s number = 6.02 X 10²³ molecules or atoms= 1 mole)  3. Using mol rations from the balanced equation.  Grams X  Molar mass of X  mole ratio  Molar Mass of Y  Grams of Y

4. Gas Stoichiometry  We can use stoichiometry for gas reactions  At times you will be able to use 22.4 Liters/1 mole at STP (standard temperature and pressure)  Standard Temperature (273 K, 0C, 32F)  Standard Pressure (1 atm, 100 kPa)

5. __CH 4 + __ O 2  __CO 2 + __H 2 O  If you have 0.167 moles of CH 4, many grams of H 2 O are produced?  0.167 moles CH 4 x 2 mol H 2 O x 18.0 g H 2 O = 6 g H 2 O  1 mol CH 4 1 mol H 2 O

6. __CH 4 + __ O 2  __CO 2 + __H 2 O  What volume of CO 2 (at STP) is produced if only 2.15 g of the CH 4 is burned?  2.15 g CH 4 x 1 mol CH 4 x 1 mol CO 2 x 22.4 Liters CO 2 = 3L CO 2  16 grams CH 4 x 1 mol CH 4 1 mol CO 2