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| In expanding on "mole calculations", what three(3) types of calculations can one use? | 1) Mole-Mole Relationships 2) Mass-Mole Relationships 3) Mass-Mass Relationships |
| It is important to do what when doing a reaction? | To know "how much product is formed when a certain amount of reactant is used |
| Being able to gaudge chemical reactions, helps us with what? | In using "chemical equations" |
| What does "STP" stand for? | "Standard Temperature and Pressure (STP)" |
| What is the Kelvin temperature for STP? | 273 Kelvin, one atmosphere |
| What are the two(2) parts of a "reaction"? | "Reactants" and "Products" |
| What is another name for "reactants "? | "Reagents" |
| How many mol of HNO3 are required to form 6.5 mol of H2O? | 4H2O |
| How many grams of would be formed if 4.25 mol of HNO3 were consumed? | 51.1 g S |
| How many liters of NO gas at STP would be formed from 2.25 mol Bi2S3? | 101 L NO |
| How many moles of HNO3 would be reacted with 24.5 g BiS3? | 0.351 mol HNO3 |
| How many grams of S would be formed if 20.25 g Bi2S3 were consumed? | 3.788 g S |
| How many liters of NO gas at STP would be formed along with 205 g of S? | 95.6 L NO |
| What is the percent yield of S if 1000.0 of BiS3 is reacted to form 10.0 g of S? | 53.5% |
| If 100.0 g of Bi2S3 is reacted with 99.00 g of HNO3 which reagant is limiting? | Bi2S3 |
| Which "reagant" would be "limiting"? | The one with the "smallest mole" ration is the "limiting reagent" |
| What is the percent yield of H2O if 50.0 L of NH3 gas at STP is reacted to form 60.0 L of H2O gas at STP? | 80.0% |
| If 100.0 L of NH3 is reacted with 110.0 L of O2 which reagent is limiting? | O2 |
| If 10.0 L of NH3 reacts with 20.0 L of O2 what mass of H2O would be formed? | 24.0 L H2O |
| Using the following chemical equation, answer the questions: 3NAHCO3 + H3PO4 -----> 3CO2 + 3H2O + Na3PO4 1) Number of moles of CO2 produced from 5.0 moles of H3PO4 2) The number of CO2 gas at STP formed from 3.0 moles of NaHCO3 3) The number of grams of NaHCO3 needed to produce 6.80 moles of water 4) Liters of CO2 gas at STP resulting when 49.0 g of H3PO$ reacts 6) Calculate the percent yield of Na3PO4 if 350 g of Na3PO$ are formed from 692 g of NaHCO3 7) If 100.0 g of NaHCO3 is reacted with 100.0 g of H3PO4 which reagent is limiting? | 1) 15 mole CO2 2) 67 liters CO2 3) 571 grams NaHCO3 4) 33.6 liters of CO2 5) 692 grams Na HCO3 6) 77.8% 7) NaHCO3 |
| Using the following chemical equation, answer the follwoing questions: H2 + CuO --------> Cu + H2O 1) If 112.0 liters of hydrogen gas STP are reacted with CuO, how many grams of water will be produced? 2) What would be the percent yield of water if 112.0 liters of H2 formed 80.0 g of H2O? 3) iF 20.0 g of H2 reacts with 40.0 g of CuO which reagent is limiting? | 1) 90.06 grams H2O 2) 88.9% 3) CuO |
| Using the following chemical equation, answer the following questions: C6H12 + 9O2 --------> 6CO2 + 6H2O 1) How many liters of CO2 gas at STP are formed when 25.8 liters of oxygen gas at STP are consumed? 2) How many moles of H2O are formed when 0.500 mol of the C6H12 are burned? 3) What is the percent yield of CO2 if 13.0 liters of CO2 gas at STP are formed from 25.8 liters of oxygen gas at STP? 4) 54.0 liters of C6H12 gas at STP are reacted with 7.00 liters of O2 gas at STP - which reagent is limiting? | 1) 17.2 liters CO2 2) 3.00moles H2O 3) 75.6% 4) O2 |
| Using the following chemical equation, answer the following questions: Fe3O4 + 4CO -----> 3Fe + 4 CO2 1) Calculate the liters of CO2 gas at STP produced when 50.2 grams of Fe3O4 are reacted 2) What is the percent yield of CO2 if 8.00 liters of CO2 gas at STP are formed from the reaction of 100.4 g of Fe3O4? 3) If 100.0 g of Fe3O4 is reacted with 100.0 L of CO, which reagent is limiting? | 1) 19.4 liters CO2 2) 20.6% 3) Fe3O4 |
| Using the following chemical equation, answer the following questions: 4Fe(CrO2)2 + 8K2CO3 + 7O2 -------> 2Fe2O3 + 8(K2CrO4 + 8CO2 1) The number of grams of Fe(CrO2)2 required to react with 5.00 liters of O2 at STP 2) The number of grams of Fe(CrO2)2 required to produce 3.0 grams of FCe2O3 3) The number of Grams of Fe(CrO2)2 required to produce 4.00 grams of K2CrO4 4) The number of liters of oxygen gas at STP required to produce 224 liters of CO2 gas at STP 5) What is the percent yield of Fe2O3 if 2.90 g of Fe2O3 are formed from reaction of 10.0 g of Fe(CrO2)2? | 1) 28.5 grams of Fe(CrO2)2 2) 8.4 grams Fe(CrO2)2 3) 2.30 grams Fe(CrO2)2 4) 196 liters O2 5) 81.2% |
| Using the following chemical equation, answer the following questions: 4 NH3 + 7O2 -----> 4NO2 + 6H2O 1) How many moles of NH3 must react if 24.8 moles of water are produced? 2) Determine the number of moles of H2O that would be formed from the combuston of 86.0 grams of NH3 3) If 88.4 liters of NO2 gas at STP are formed, what number of moles of oxygen must have been consumed? 4) 134 liters of NH3 gas at STP would combine with what volume (liters of gas at STP) of oxygen? 5) Calculate the percent yield of H2O if 80.0 g of H2O are formed from reaction of 80.0 L of O2 gas at STP? 6) Which reagent is limiting if 95.0 L of NH3 gas at STP is reacted with 160.0 L of O2 gas at STP? | 1) 16.5 moles NH3 2) 7.57 moles of H@O 3) 6.91 moles of H2O 4) 235 liters H2O 5) 82.9% 6) O2 |
| Using the following chemical equation, answer the following question: 4Al(s) + 3O2(g) ------> 2Al2O3(s) How many grams of Al2O3 could be produced from 225 grams of Al reacting with 300. liters of O2 gas at STP? | 425. grams of Al2O3 (Al was the limiting reactant) |
| Using the following chemical equation, answer the following question: 3Mg(OH02(s) + 2H3PO4(aq) -----> 6H2)(l) + Mg3(PO4)2(s) How many moles of water could be produced from the reaction of 575 grams pf Mg(OH)2 with 5.00 L of a 2.50 M H3PO4 solution? | 19.7 moles of H2O (Mg(OH)2 is the limiting reactant) |
| Using the following chemical equation, answer the following question: 2C8H18(l) + 25O2(g) -----> 16CO2(g) + 18H2O(g) All gases are at STP - How many liters of C)2 would be produced from the reaction of 5.0 L of C8H18 with 55 l of O2? | 35 L CO2 (O2 was the limiting reactant) |
