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Gas Stoichiometry LAST PHASE OF STOICHIOMETRY, WOOHOO!!!!! Slide 2 Slide 3 Gas Stoichiometry We have looked at stoichiometry: 1. using masses and molar masses (periodic table walk g/1mole) 2. using molecules (avogardos number = 6.02 X 10 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 Slide 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) Slide 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 Slide 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