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Wednesday, May 11, 2010

Wednesday, May 11, 2010. Weston Preparatory Academy Chemistry Classes. Wednesday, May 12, 2010. Warmup: Daily class diary/ journal OR: What happens when water and electricity mix? Guess or tell a story. HW due today: p.311 #1-7 all.

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Wednesday, May 11, 2010

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  1. Wednesday, May 11, 2010 Weston Preparatory Academy Chemistry Classes

  2. Wednesday, May 12, 2010 • Warmup: Daily class diary/ journal OR: What happens when water and electricity mix? Guess or tell a story. • HW due today: p.311 #1-7 all. • HW due tomorrow: p. 319 #1-14 odd; due Friday: p. 327 #1-9 all; due Mon. May 17: p. 329 #1-21 odd. • Notes, discussion, group tutoring!

  3. Morgan & Pac’s Slide • Thug Life is a movement if you ain’t with us you against us. Get money….. THUG LIFE THUG LIFE WHAO!!!!!!!!

  4. PAGE 311 #1-7 ; SKIP #5; due today. • What conversion factor is present in almost all stoichiometry calculations? (pg. 303) • For a given substance, what information links mass to moles? (see pg. 230) number of particles to moles? (it’s Avogadro’s number) • What conversion factor will change moles CO2 to grams CO2? (see P.Table) Moles H2O to molecules H2O? (see P. Table)

  5. Chapter 9Reading Notes: • Page 302. • Balanced equations show proportions. • 2H2 + O2 2H2O

  6. Chapter 9Reading Notes: Balanced equations show proportions. • 2H2 + O2 2H2O • For every 2 moles of Hydrogen gas, There is 1 mole of oxygen gas and there are 2 moles of water produced from the reaction.

  7. Chapter 9Reading Notes: • 2H2 + O2 2H2O • 12 hydrogen atoms- 6 oxygen atoms- 12 water molecules • 500 hydrogen- 250 oxygen – 500 water • ½ mole hydrogen- ¼ mole oxygen – ½ mole water • The coefficients show the RATIO of molecules and atoms of reactants and products to each other.

  8. PAGE 311 #1-7 ; SKIP #5; due today. • 4. Br2 + Cl2 2BrCl • A. Look at the mole ratios! The number of moles of Cl2 is the HALF as many as the moles of BrCl • B. Convert grams to moles of Cl2, then multiply the number of moles by 2 (due to the mole ratio). Multiply this number of moles by the molar mass of BrCl found in the periodic table. • C. Convert molecules to moles. That is the same number of moles need of Br2 (mole ratio is 1:1)

  9. PAGE 311 #1-7 ; SKIP #5; due today. • 6. Why do you need to use amount in moles to solve stoichiometry problems? Why can’t you just convert from mass to mass?(Using coefficients from balanced equation shows relationships of numbers of particles, not masses!)

  10. PAGE 311 #1-7 ; SKIP #5; due today. • 7. TWO reactions are described. • A. LiOH + CO2  LiCO3 + H2O(NOW BALANCE THIS BEFORE WRITING IT DOWN!) and NaOH + CO2  NaCO3 + H2O • B. Convert 288 g CO2 to moles CO2 using the molar mass from the periodic table. Then… multiply or divide according to the mole ration (look at the coefficients from your balanced chemical equations, part A). Then… multiply number of moles by the molar mass (of LiOH, then NaOH) of the substance to calculate the number of grams.

  11. PAGE 311 #1-7 ; SKIP #5; due today. • 7. TWO reactions are described. • A. LiOH + CO2  LiCO3 + H2O(NOW BALANCE THIS BEFORE WRITING IT DOWN!) and NaOH + CO2  NaCO3 + H2O • B. Convert 288 g CO2 to moles CO2 using the molar mass from the periodic table. Then… multiply or divide according to the mole ration (look at the coefficients from your balanced chemical equations, part A). Then… multiply number of moles by the molar mass (of LiOH, then NaOH) of the substance to calculate the number of grams. • C. Comment on the number of grams of each that are needed, the cost per mole of each, and the cost to transport large masses of material into space.

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