practice exam

							                                   Unit One – Review
                                     Practice Exam
Review Exam Topics
    Significant Figures/Scientific Notation 10%
    Stoichiometry, Limiting Reactant, % Yield (BCA) 25%
    Molarity/Dilution 15%
    Subatomic Particles/Isotopes 10%
    Mass % and Empirical Formula 10%
    Density (including water) 5%
    Hydrates 5%
    Conversions (metric, Kelvin,C volumes mL,cm3) 10%

Practice Exam
This portion of the review should be completed WITHOUT a calculator.
   1. Paul is 1.7 m tall. How tall is Paul in kilometers?
                                          in centimeters?



   2. How many cubic millimeters are in a liter of water?



   3. How many significant figures are in the following measurements?
        a. 10 cm                  b. 0.0020 g            c. 10 cows
        d. 10.0 mL                e. 100.10 K            f. 1.013 kg

   4. A student weighed 2.0 mL of water 3 times and obtained the following results:
      3.01 g, 2.99 g, 2.97 g. Is the balance the student is using accurate? Is it precise?
      Explain.




   5. Libby measures a liquid to be one hundred millimeters. She estimated her
      measurement to the nearest one-millimeter. Using significant figures, how should
      Libby report her measurement?




   6. Liquid nitrogen boils at 77 K. What is this in Celsius?



   7. What are the three basic components of an atom? What is the charge on each
      component? What is the relative mass of each component?
                                      Unit One – Review
                                        Practice Exam




   8. How do carbon-12 and carbon-13 differ? How are they the same?



    36
      Cl
9. 17     What is the mass number? The atomic number? How many protons does this
atom have? Neutrons?




   10. How many liters of oxygen will be required to completely combust 11.2 L of
      methane (CH4) gas?




   11. Approximately how many grams of sodium fluoride must be added to 100.0 mL
       of water to make a 0.4 M solution?




   12. Suppose 100.0 mL of a 1.0 M aluminum chloride (AlCl3) solution is added to a
       1.0 L volumetric flask. Water is added to the mark. What is the final
       concentration of chloride ions?




   13. Use the rules of significant figures to solve the following:
          a. 1.00 cm + 0.003 cm =


          b. (3.0 x 102 cm) x (3.00 x 103 cm) =


                     4.00 g
          c.                      
               (25 mL  20 .9mL )
                                 Unit One – Review
                                   Practice Exam
   14. What is the percent by mass of oxygen in SO2?




Calculator-Based Problems

   1. Vinegar is a solution that is 3.1 % acetic acid (HC2H3O2) by mass. What is the
      molarity of the acid in vinegar?




   2. When solid ClF is combined with fluorine gas, a compound forms that is 27 %
      chlorine and 73 % fluorine. What is the empirical formula of the resulting
      compound?




   3. The yellow precipitate of lead (II) iodide is recovered by mixing solutions of
      aqueous lead (II) nitrate and sodium iodide. After mixing, the precipitate is
      filtered and placed in a drying oven.
           a. How many grams of lead (II) iodide can be recovered by mixing 135.0 mL
              of 2.00 M sodium iodide with 250.0 mL of 1.00 M lead (II) nitrate
              (Pb(NO3)2)?




          b. Suppose a student recovers 65.0 grams lead (II) iodide when performing
             the reaction above. What is the student’s percent yield?
                        Unit One – Review
                          Practice Exam


c. Suggest possible sources of error based on the findings in part b.