| Chapter Vocabulary | ||
| #1 | What is the definition of Mole Ratio? | Conversion factor that relates the amount of moles of any two substances involved in a chemical reaction. |
| #2 | (T/F) Throughout chapter nine we have been studying reaction stoichiometry? | True |
| #3 | The substance that is not used up completely in a chemical reaction? | Excess Reactant |
| #4 | What is the definition of theoretical yield? | the maximum amount of product that can be produced from a |
| #5 | The ratio of the actual yield to the theoretical yield multiplied by 100 | Percent yield |
| Stoic Process | ||
| #1 | What is the first step to take before calculating a stoichiometry problem? | Balance the Equation |
| #2 | A balanced chemical equation allows one to determine the | Molar Ratio |
| #3 | When the limiting reactant in a chemical reaction is completely used, the reaction....? | the reaction stops |
| #4 | The coefficients in a chemical equation represent the | relative numbers of moles of reactants and products |
| #5 | The reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction? | Limiting Reactant |
| Molar Calculations | ||
| #1 | In the reaction 2Al2O3 → 4Al + 3O2, what is the mole ratio of aluminum to oxygen? | 4:3 |
| #2 | In the reaction 2Al2O3 --> 4Al + 3O2, what is the mole ratio of Oxygen to Aluminum Oxide?? | 3:2 |
| #3 | Avagadro's Number is 1 mole = ? | 6.022 * 10^23 |
| #4 | For the reaction C + 2H2 --> CH4, how many moles of hydrogen are required to produce 10 mol of methane, CH4? | 20 moles |
| #5 | For the reaction 2H2 + O2→ 2H2O, how many moles of water can be produced from 6.0 mol of oxygen? | 12 moles |
| Mass Calculations | ||
| #1 | What is molar mass of C6H10O2 | 114.16g/mol |
| #2 | For the reaction HCl + NaOH → NaCl + H2O, how many moles of hydrochloric acid are required to produce 150. g of water? | 8.32 moles HCL |
| #3 | For the reaction HCl + NaOH → NaCl + H2O, how many grams of hydrochloric acid are required to produce 100 g of water? | 202g HCL |
| #4 | For the reaction 2Fe + O2 → 2FeO, how many grams of iron oxide are produced from 8.00 mol of iron? | 574g FeO |
| #5 | For the reaction 2Fe + O2 → 2FeO, how many grams of Oxygen are required to produce 350 g of FeO | ~40.0g |
| Everything Else | ||
| #1 | What is the measurement for volume @ STP? | 22.4 L |
| #2 | What is the actual yield? | What you actually make during the experiment |
| #3 | In the reaction A + B → C + D, if the quantity of B is insufficient t, then B is what? | The limiting reactant |
| #4 | What is the formula for Percent Yield? | % Yield= (Actual YIeld/Theoretical Yield) * 100 |
| #5 | For the reaction SO3 + H2O → H2SO4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid? | 320g |
| Final Question | |
| For the reaction 2Na + Cl2 → 2NaCl, calculate the percent yield if 200. g of chlorine react with excess sodium to produce 240. g of sodium chloride. | 72.8% |