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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

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

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