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Basic mole calculations (pp.112-124) % composition problems/combustion analysis (pp.384-392)

Where we’ve been for ~ 3 weeks now:. Basic mole calculations (pp.112-124) % composition problems/combustion analysis (pp.384-392) Reaction balancing (pp. 392-395 ) `body parts’ calculations (no formal section in text) Next: Reaction stoichiometry ( pp. 396-406 ).

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Basic mole calculations (pp.112-124) % composition problems/combustion analysis (pp.384-392)

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  1. Where we’ve been for ~ 3 weeks now: • Basic mole calculations (pp.112-124) • % composition problems/combustion analysis (pp.384-392) • Reaction balancing (pp. 392-395) • `body parts’ calculations (no formal section in text) • Next: Reaction stoichiometry • (pp. 396-406)

  2. Reaction Stoichiometry problems:how chemists cook

  3. A non-chemical example of stoichiometry IN 1 + 2 + 3 200 g/box 300 g/block 500 g/dozen OUT Mass of 1 output souffle ? + 1 *300 g 2* 500 g + 3*200 cheese eggs condensed milk =1900 g/souffle

  4. Cooking and stoichiometry THE RECIPE 3 1 + 2 + 300 g/block 200 g/box 500 g/dozen 1900 g/souffle How many….to make whole # of souffles ? 12 • How many boxes of cream to make 4 souffles ? 2 • 600 grams cheese makes how many souffles ? • How many grams of eggs combine with 9 boxes of cream ? 3000 g 2 • 48 eggs combine with how many blocks of cheese ?

  5. Exam 2 MONDAY21 October 2013 Bring calculators !!!

  6. Reaction Stoichiometry problems:how chemists cook Sample of Typical Reaction stoichiometry problems C3H8+ 5O2 3CO2+ 4H2O BALANCED Example 1: (reactant  product) Given 16 grams of O2 predict the how many molecules of CO2 that can form.

  7. Another example of Reaction Stoichiometry problems:how chemists cook Typical Reaction stoichiometry problems (cont.) C3H8+ 5O2 3CO2+ 4H2O Example 2: (limiting reactant product) Given 1 gram of O2 and 1 gram of C3H8, what is the maximum weight of H2O we can make ?

  8. English-metric conversions (2 ptseach/4 pts total) Relevant Conversion factor : 1 lb =454 g = 0.454 kg =16 oz • Ex.How many oz in 567.5 g ? • _______oz in 567.5 g 20 2.2. Metric-metric symbols and conversions (16 pts) 10-12 p Ex. 200 g = ?? kg =200*10-9 =2*10-7

  9. 2.3. unknown metal density determination (4 pts) See density lab and review metal density determination 2.4 egg arithmetic (2 pt each/8 pts total)) A dozen monstrously large eggs from Aldi’s weighs 2000 g. Assuming 1 dozen =12 count: Ex. • If you have 50,000 grams of eggs, how many eggs do you have ? __________ egg count 300

  10. 2.5. Simple mole-weight-count conversions (3 pts each/18 pts total) SHOW WORK !!! Assuming that a mole count= 6*1023 and the gram atomic masses: C=12 g/mol O=16 g/mol H= 1 g/mol Ex. Glucose has the molecular formula C6H12O6 . What is its’ molecular weight ? ______g/mol 180 How many molecules of glucose are in 9 grams of glucose ? ______ molecules glucose in 9 grams Ex. 3*1022

  11. 2.6. Stoichiometry Problems (`Body Parts’): Show work ! (5 pts each/25 pts total) The molecular mass of dynamite=TNT (C7H5N3O6) is 227 g/mol. Given the atomic masses C=12 g/mol, H = 1 g/mol, N = 14 g/mol O=16 g/mol Ex. • How many grams of N are in a sample of TNT • containing 0.714 mol H ? _______ g N 6

  12. 2.7. % Composition problems and combustion problems ( 3 pts each/9 pts total) Ex. n/nmin n=w/at. wt 5 6 26.667 32 Ex. 0.8333 1 C6H32O1 Empiric formula=: ____________________ Ex. CxHy is burned to form 4.4 g CO2 and 1.8 g H2O. What is the empiric formula of CxHy ?

  13. 2.8 combustion analysis Ex. CxHy is burned to form 4.4 g CO2 and 1.8 g H2O. What is the empiric formula of CxHy ? CH2 2.9 Reaction Balancing (2 pt each/ 6 pts total) Balance these reactions: ___ C2 H6 + ___O2___CO2+ __H2O 6 4 2 5

  14. 2.9 Naming ( 1 pt/name; 4 pts total) Review Stock namingmethod presented in lab Given: carbonate = CO3-2 nitrate = NO3-1 Use the Periodic Table provided to name or determine the formula of the compounds below: CuCO3name=_______________ Copper (II) carbonate Calcium acetate =_____________ Ca(C2H3O2)2

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