Engage Whoosh bottle Elephant Toothpaste KI  +  Pb(NO 3 ) 2 Mg  +  HCl  with balloon and Erlenmeyer
Prior knowledge? <ul><li>Atomic mass </li></ul><ul><li>Dimensional analysis </li></ul><ul><li>Writing formulas </li></ul><...
What should be taught? <ul><li>1 mole = 6.02 x 10 23  atoms or molecules </li></ul><ul><li>1 mole = (molar mass) grams </l...
What will constitute mastery? <ul><li>The student will be able to: </li></ul><ul><li>Calculate atoms, ions, molecules and ...
<ul><li>Calculate the number of grams and/or atoms in 5.6 moles of iron. </li></ul><ul><li>Calculate the number of moles i...
<ul><li>When 15.0 g of phosphorus trichloride react with 2.5 g of chlorine gas, the actual yield of phosphorus pentachlori...
<ul><li>S(s)  +  O2 (g)     SO2 (g)  ∆H = -296 kJ/mol </li></ul><ul><li>Calculate the heat evolved when 275 g S is burned...
<ul><li>Jane Smith </li></ul><ul><li>[email_address] </li></ul><ul><li>Karen Compton [email_address] </li></ul><ul><li>Cla...
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Stoichiometry

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Presented by Karen Compton, Jane Smith and Claudia Wallace in the ACT2 stand at CAST2010 in Houston, Texas

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Stoichiometry

  1. 2. Engage Whoosh bottle Elephant Toothpaste KI + Pb(NO 3 ) 2 Mg + HCl with balloon and Erlenmeyer
  2. 3. Prior knowledge? <ul><li>Atomic mass </li></ul><ul><li>Dimensional analysis </li></ul><ul><li>Writing formulas </li></ul><ul><li>Writing balanced equations </li></ul>
  3. 4. What should be taught? <ul><li>1 mole = 6.02 x 10 23 atoms or molecules </li></ul><ul><li>1 mole = (molar mass) grams </li></ul><ul><li>Mole ratios using a balanced equation </li></ul><ul><li>1 mole of gas @ STP has a volume of 22.4 L </li></ul><ul><li>Limiting reactants </li></ul><ul><li>% composition </li></ul><ul><li>Empirical formulas </li></ul><ul><li>Molecular formulas </li></ul><ul><li>Percent yield </li></ul><ul><li>Theoretical yield </li></ul><ul><li>Actual yield </li></ul>
  4. 5. What will constitute mastery? <ul><li>The student will be able to: </li></ul><ul><li>Calculate atoms, ions, molecules and moles </li></ul><ul><li>Mass  mass calculations </li></ul><ul><li>Empirical formula/ molecular formulas calculations </li></ul><ul><li>Percent yield/theoretical yield calculations </li></ul>
  5. 6. <ul><li>Calculate the number of grams and/or atoms in 5.6 moles of iron. </li></ul><ul><li>Calculate the number of moles in 56.9 grams of sulfur. </li></ul><ul><li>Calculate the mass of barium sulfate produced when 30.0 g of sulfuric acid react with 25.0 g of barium hydroxide. </li></ul>
  6. 7. <ul><li>When 15.0 g of phosphorus trichloride react with 2.5 g of chlorine gas, the actual yield of phosphorus pentachloride is 5.6 g. What is the percent yield? </li></ul><ul><li>Analysis shows that a compound contains 44.3% phosphorus and 55.7 % oxygen. What is the empirical formula of this compound? </li></ul><ul><li>Experimentation shows that the molar mass of this compound is 283.89 g/mol. What is the molecular formula? </li></ul>
  7. 8. <ul><li>S(s) + O2 (g)  SO2 (g) ∆H = -296 kJ/mol </li></ul><ul><li>Calculate the heat evolved when 275 g S is burned </li></ul>
  8. 9. <ul><li>Jane Smith </li></ul><ul><li>[email_address] </li></ul><ul><li>Karen Compton [email_address] </li></ul><ul><li>Claudia Wallace </li></ul><ul><li>[email_address] </li></ul>

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