Limiting Reagents and Percent Yield

Name: Panther ID: Worksheet S2 Limiting Reagents and Percent Yield SHOW ALL UNITS AND WORK 1. What is the balanced reaction of butane (C 4 H 10 ) with oxygen (O 2 ) to produce carbon dioxide (CO 2 ) and water (H 2 O)? (This is a combustion reaction) 2. What are the molar masses of butane (C 4 H 10 ), oxygen (O 2 ), carbon dioxide (CO 2 ) and water (H 2 O)? 3. For the diagram below, mark the path that you would use to determine how much carbon dioxide (in g) would be produced if 10 g of butane are combusted in excess oxygen. Indicate what substance is A and what substance is B in the diagram. 4. Now do the calculation. moles A moles B stoichiometric ratio from balanced equation grams A grams B mol/g g/mol g/mol mol/g

Name: Panther ID: 5. If you did the reaction outlined in # 3 and produced 5.4g carbon dioxide, what would be the percent yield? 6. If you had 10g of butane and 10g of oxygen, what is the maximum amount of carbon dioxide (in g) that could be produced? First describe the method you would use to determine this, and then do the calculation. 7. If you did the reaction outlined in #5 and produced 5.4g carbon dioxide, what would be the percent yield. Challenge question: 8. It we had a mole of people how many planets would we need at the current population density of the earth? (7 billion)