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Procedures / Review

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Procedures / Review

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  1. November12, 2013 Once you’re in, you’re in.When the bell rings, electronics and headphones away working on the Do Now (half sheet you picked up). You have until 5 minutes after the bell until this is collected. TURN IN STEM PROJECT DUE DATE #3.TURN IN ANY LATE STEM PROJECT ASSIGNMENTS AND ANY LATE HW.

  2. Procedures / Review • Entrance Routine • Pencils / Paper / Calculators • Cell Phones • Tardies (warm up and referrals) • Turning in work • Stem Project

  3. Tutoring • Today afterschool in 529 (2:30 – 3:30pm) – stem project • Thursday afterschool in 710 (2:30-3:30pm) – will not be available • Wednesday Lunch A

  4. Homework 11-12-13 • Solutions reading and anticipation guide ** • Anticipation guide due 11-13-2013 ** **graded

  5. Reaction Stoichiometry Test • Reviewing more today • 1 hour to finish tomorrow • New content tomorrow after test

  6. Have out • Guided Practice you picked up today • Reaction Stoichiometry flow sheet (raise hand if you can’t find it) • Blank sheet of paper for any misc. notes we need to take • Calculator if you have one; don’t ask to use mine – get one from the pink bucket. • Naming flow chart

  7. Objective • Utilize mole ratios from the balanced equation to calculate the quantity of one substance in a reaction given the quantity of the desired substance in the reaction (given moles or mass and ending with moles or mass)

  8. Part I Determine the formula for the following compounds: Iron (III) phosphate Calcium hydroxide Iron (III) sulfate Lead (IV) oxide Sodium carbonate Potassium dichromate Ca(OH)2 FePO4 PbO2 Fe(SO4)3 Na2CO3 K2Cr2O7

  9. Part II Calculate the mass of 1 mole of each of the substances in part I FePO4Ca(OH)2 Fe2(SO4)3 PbO2 Na2CO3 K2Cr2O7 151g 74g 208g 239g 294g 106g

  10. Part III Calculate the number of moles if you have 25g of each of the substances from part I FePO4Ca(OH)2 Fe2(SO4)3 PbO2 Na2CO3 K2Cr2O7 0.338 moles 0.166 moles 0.120 moles 0.105 moles 0.236 moles 0.085 moles

  11. Part IV Write equations for the following reactions: The combustion of propane (C3H8) The reaction between copper sulfate and sodium carbonate The reaction between hydrochloric acid and copper carbonate C3H8 + O2 → CO2 + H2O CuSO4 + Na2CO3 → Na2SO4 + CuCO3 HCl + CuCO3 → CuCl2 + H2O + CO2

  12. Part V Add state symbols to the following equations The combustion of propane (C3H8) The reaction between copper sulfate and sodium carbonate The reaction between hydrochloric acid and copper carbonate C3H8 + O2 → CO2 + H2O CuSO4 + Na2CO3 → Na2SO4 + CuCO3 HCl + CuCO3 → CuCl2 + H2O + CO2

  13. Part VI Balance the equations The combustion of propane (C3H8) The reaction between copper sulfate and sodium carbonate The reaction between hydrochloric acid and copper carbonate C3H8 + O2 → CO2 + H2O CuSO4 + Na2CO3 → Na2SO4 + CuCO3 HCl + CuCO3 → CuCl2 + H2O + CO2

  14. Part VII If 25g propane is burned, what mass of oxygen is required for complete combustion C3H8 + O2 → CO2 + H2O

  15. Part VII If 15g of copper carbonate is reacted with excess hydrochloric acid, calculate the mass of carbon dioxide formed. If 3.1g of carbon dioxide is formed, calculate the percent yield. HCl + CuCO3 → CuCl2 + H2O + CO2

  16. Part VII If 20g copper sulfate is reacted with 20g sodium carbonate, which reactant is the limiting reactant and what mass of precipitate is formed? CuSO4 + Na2CO3 → Na2SO4 + CuCO3

  17. Exit Ticket Ammonium hydrogen phosphate, (NH4)2HPO4, a common fertilizer, is made from reacting phosphoric acid, H3PO4, with ammonia, NH3. • Write the balanced equation for this reaction. • If 10.00 g of ammonia react, how many moles of fertilizer will be produced? c. What mass of ammonia will react with 280 kg of H3PO4?

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