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Unit  6  Exam - Ch10 and CH 11
 Look at the following pages in your book and notes to help you for the test:
In your book:
      Page: 303 - 305  -  KMT - kinetic molecular theory
      Page: 306 - deviations of real gases from ideal behavior
      Page: 308 - 312 - Pressure
      Page: 313 - 323 - Gas Laws (boyle's, charles', Gay-Lussac's, combined, & dalton's)
      Page: 333 - 336 - Volume-Mass relationships of gases
      Page: 340 - 346 - ideal Gas Law with density and molar mass
      Page: 347 - 350 - Stoichiometry of gases
      Page: 351 - 354 - diffusion and effusion 
 
Below is the answer key to your Review and Video Lessons for objectives being tested on your exam.
 Review the following video link to view a
Video one: "Review of Stoichiometry - the ideal gas law" - http://www.youtube.com/watch?v=fzeW_ZUENhs
 

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Unit  6  Exam - Ch9
 Look at the following pages in your book and notes to help you for the test:
In your book:
      Page: 280 - 281  -  Mol to Mol Calculations
      Page: 286 - 287  -  Mass to Mass Calculations
      Page: 288 - 291  -  Limiting Reactants:
      Page: 293 - 294  -  Percent Yield:  
 
Below is the answer key to your Review and Video Lessons for objectives being tested on your exam.
 
Stochiometry & law of Conservation of mass:      www.youtube.com - Video 1
                                                                                           
 
 Mole to Mole Calculations:   www.youtube.com - Video 1
                                                       
 
Mass to Mass Calculations:      www.youtube.com - Video 1
                                                          
 
Limiting reactant/reagent:  www.youtube.com - Video 1
                                                   www.youtube.com - Video 2    (good examples)
 
 Percent Yield:  the following video will explain theoretical yield, actual yield and how to calculate percent yield...
                               www.youtube.com - Video 1  (Good explanation)
                               www.youtube.com - Video 2  (good example)
                               www.youtube.com - Video3      (forward to 5:58 for percent yield)
                               

  • Ch9 Stoichiometry Extra Problems

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    Answers to the 7 questions:
    #1.  Balanced combustion reaction (1,5,3,4) Answer= .5 mol O2 
    #2.  Balanced reaction = (2,1,2)  Answer = 3.9 mol O2 
    #3.  Balanced combustion reaction= (1,2,1,2) answer = 91.2g O2 
    #4.  Use: (22.4L H2 = 1mol H2), answer = 68.04 L H2 
    #5.   Balanced reaction = (2,1,1,2) Answer = 1.12 g PbBr2 
    #6.   limiting = COCl2   Excess NaOH = .35 g NaOH
    #7.  Theoretical Yield=104.7g Ca3(PO4)2  and Percent Yield = 71.6 %
    , (Last Modified about a minute ago )
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  • U6 exam Review

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    U6 Stoichiometry Review 
    Key:  please use the key to help you with your work.
     
    mole to mole 
    1.  Balanced equation: (2,2,1), answer = 1.25 mol Cl2 
    2.  .45 mol Na2SO4 
    mass to mass 
    3.  Balanced reaction: (1,1,1,2), answer = 9.66 g PbCrO4
    4.  49.9 g LiBr
    Limiting reactant 
    5.  O2 is limiting reactant
    6.  Li is limiting reactant
    7.  H2SO4 is the limiting reactant,     34.9 g Al2(SO4)3,      8.1 g Al(OH)3  
    Percent yeild:
    1.  75%
    2.  2.07 g
    3.  theoretical = 53.0g C6H5Cl  and   % yield = 73.2%
     
     
    Unit 6 Review Pre-AP.docx, 21.45 KB (Last Modified on December 16, 2011 )
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Unit  5  Exam - Ch8 Notes and files
 Look at the following files to help you study for the test. 

Unit  4 Exam - Ch7.3 and 7.4 Notes and files
 Look at the following files to help you study for the test. 

  • Unit 4 Notes

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    Unit 4 notes:
    1.  Molar Mass Calculations
    2.  Molar conversions
    3.  % composition
    4.  empirical formula
    5.  molecular formula
     
     
    Unit 4 mole notes.pdf, 121.28 KB (Last Modified on November 7, 2011 )
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  • Unit 4 Review Questions: Extra Problems

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    The following questions will help you review for the test.  Here are the answers for you to check your work:
     
    #1 molar mass = 134.0 g, 5.6 e21 molecules C4H6O5
    #2 molar mass= 90.0 g, 538.2 g H2C2O4
    #3 a.  molar mass = 121.1 grams H7SC3N1O2
          b.  26.5 % S
          c.  1.24 moles of H7SC3NO2
     
          d.  
           answer   1.50g H7SC3NO2  x  1 mol H7SC3NO2                       7mol H               6.02 e23 atoms H
                        -------------------------      --------------------------------   x   ---------------------------  x   ----------------------       =
                                     1                 121.0 g H7SC3NO2           1mol H7SC3NO2         1 mole H
     
    5.22e22 H7SC3NO2
    #4  22.4 L
     #5.  1.96 g/L N2O
     #6)   molar mass=80.0grams,  35%N, 5%H, 60%O
     #7)  molar mass=52.84g,  10.1%C,  .8%H, 60%Cl 
    #8) .25 mol C, .26mol H, .76mol I,  CHI3
    #9) 3.41 mol C, 4.58molH, 3.41molO;    C3H4O3;   n=2  C6H8O6 (molecular)
    #10  omit 
    , (Last Modified about a minute ago )
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Unit 3 Exam - Ch7 Notes and files
 Look at the following files to help you study for the test. 
Notes for formula writing and Naming compounds
for the Powerpoint notes, go to the Notes link. 

  • notes_ionic compounds

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    notes for Writing and Naming ionic compounds
    both Binary and Ternary Compounds 
    notes_Ionic compounds.pdf, 6.91 KB (Last Modified on October 22, 2011 )
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  • Unit3 extra problems

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    Review Handout - Unit 3 Extra Problems
    here is a copy of the review given to you on thursday and Friday.
    Practice problems that will help you with the test.  download if you need this page 
    unit 3 extra practice.pdf, 57.96 KB (Last Modified on October 22, 2011 )
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  • notes_compound types

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    Notes - Review of Compounds for test
     
    notes_compounds.pdf, 73.95 KB (Last Modified on October 22, 2011 )
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  • ions handount

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    ion handout for monatomic and polyatomic ions
    ions sheet.pdf, 66.77 KB (Last Modified on October 22, 2011 )
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Unit 2 Exam - Ch3 Notes and files
Look at the following files to help you study for the test. 

CH3 Isotope Notes-
Notes for anyone that needs to update the homework notes.  
copy them and study for the test Monday.
 

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