Unit I      Safety Unit Analysis Measurement

 

 

 

 

Lesson            Day                 Date                Topic                                                   Homework

 

1.                                                         Safety                                                              1

2.                                                         Disssociation and Ionic Formulas                   2

3.                                                         Balancing and Word Equations                       3

4.                                                         Physical and Chemical Changes                      4

5.                                                         Matter and Bonding                                         5

6.                                                         Review and Lab Preparation                           6

7.                                                         Uncertainty Lab Day 1                                     Lab Handout

8.                                                         Uncertainty Lab Day 2

9.                                                         Measurement and Uncertainty                          7

10.                                                       Significant Figures                                           8

11.                                                       Unit Analysis 1                                                9

12.                                                       Unit Analysis 2                                                10         

13.                                                       Reading Scales                                                11

14.                                                       Density Calculations                                       12

15.                                                       Practice Test                                                   13

16.                                                       Test                                                    

 

 

 

 

 

Assignment # 1           Safety

 

Complete the safety map for the room by indicating the location of the three fire extinguishers, five doors, eyewash, fume-hood, fire blanket, aprons, eye-goggles, broken glass container, spill control pillows, four soap dispensers, three paper towel dispensers, and the soap sprayer. This is like a treasure hunt. Get up and look for everything.

 

  Assignment # 2      Ionic Formulas

 

Write the ionic formula, name, and dissociation equation for each combination indicated by the cell below.

 

Note that all ionic compounds (start with metals) are solids at room temperature.    

 

 

 

 

Li

Mg

Al

NH4

Na

OH

1

2

3

4

5

SO4

6

7

8

9

10

Br

11

12

13

14

15

F

16

17

18

19

20

NO3

21

22

23

24

25

PO4

26

27

28

29

30

S

31

32

33

34

35

C2O4

36

37

38

39

40

 

 

 

1.         LiOH              Lithium hydroxide                 LiOH(s)       Li+(aq)   +     OH-(aq)

 

 

2.        

 

   

3.         Al(OH)3                Aluminum hydroxide  Al(OH)3(s)       Al3+(aq)    +    3OH-(aq)

 

 

4.

 

 

5.         NaOH             Sodium hydroxide                  NaOH(s)      Na+(aq)    +    OH-(aq)

 

 

6.

 

 

7.         MgSO4            Magnesium sulphate              MgSO4(s)      Mg2+(aq)    +    SO42-(aq)

 

 

8.

 

 

9.         (NH4)2SO4      Ammonium sulphate              (NH4)2SO4(s)      2NH4+(aq)   +      SO42-(aq)

 

 

10.

 

 

11.       LiBr                Lithium bromide                    LiBr(s)        Li+(aq)    +    Br-(aq)

 

 

12.

 

 

13.      AlBr3               Aluminum bromide                 AlBr3(s)          Al3+(aq)    +    3Br-(aq)

 

 

14.

 

 

15.       NaBr               Sodium bromide                     NaBr(s)      Na+(aq)    +    Br-(aq)

 

 

16.

 

 

17.       MgF2               Magnesium Fluoride              MgF2(s)        Mg2+(aq)   +   2F-(aq)

 

 

18.

 

 

19.       NH4F                Ammonium Fluoride                NH4F(s)      NH4+(aq)    +    F-(aq)

 

 

20.

 

 

21.       LiNO3             Lithium nitrate                         LiNO3(s)       Li+(aq)    +   NO3-(aq)

 

 

 

22.

 

 

23.       Al(NO3)3         Aluminum nitrate                   Al(NO3)3(s)       Al3+(aq)    +    3NO3-(aq)

 

 

24.

 

 

25.       NaNO3            Sodium nitrate                       NaNO3(s)       Na+(aq)    +    NO3-(aq)

 

 

26.

 

 

 

28.       AlPO4             Aluminum phosphate AlPO4(s)      Al3+(aq)    +    PO43-(aq)

 

 

29.      

 

 

30.        Na3PO4           Sodium phosphate                  Na3PO4(s)      3Na+(aq)    +    PO43-(aq)

 

 

31.      

 

 

32.       MgS                Magnesium sulphide              MgS(s)       Mg2+(aq)    +    S2-(aq)

 

 

33.  

 

 

34.      (NH4)2S          Ammonium sulphide               (NH4)2S(s)       2NH4+(aq)    +    S2-(aq)

 

 

35.      

 

 

36.

 

 

37.       MgC2O4        Magnesium oxalate         MgC2O4(s)      Mg2+(aq)    +    C2O42-(aq)

 

 

38.

 

 

39.       (NH4)2C2O4  Ammonium oxalate         (NH4)2C2O4(s)    2NH4+(aq)   +  C2O42-(aq)

 

 

 

 

 

  Assignment #3 Chemical Equations from Word Equation

 

 

1.         Aqueous potassium hydroxide is reacted with aqueous sulphuric acid producing a solution of potassium sulphate and water.

 

 

2KOH(aq)     +     H2SO4(aq)          K2SO4(aq)    +     2H2O(l)

 

 

 

2.         Sodium metal is reacted with zinc iodide in solution.  The products obtained are aqueous sodium iodide in and zinc metal.

 

 

 

 

 

 

3.         Solid calcium sulphate dihydrate is added to gaseous sulphur trioxide producing solid calcium sulphate and aqueous sulphuric acid.

 

 

CaSO4.2H2O(s)     +     2SO3(g)          CaSO4(s)    +     2H2SO4(aq)

 

 

 

4.         Solid calcium phosphate and aqueous sodium nitrate are formed when solutions of sodium phosphate and calcium nitrate are mixed.

 

 

 

            2Na3PO4(aq)   +        3Ca(NO3)2(aq)          ®            Ca3(PO4)2(s)    +   6NaNO3(aq)          

 

 

5.         Sodium phosphite reacts with calcium nitrate in solution to produce two new ionic compounds. The calcium compound is solid while the other is aqueous.

 

 

             2Na3PO4(aq)   +        3Ca(NO3)2(aq)          ®            Ca3(PO4)2(s)    +   6NaNO3(aq)  

 

 

6.         Gaseous sulphur trioxide, a pollutant released into the atmosphere by burning coal reacts with liquid water in the air to make a solution of sulphuric acid (acid rain).

 

 

 

           SO3(g)    +    H20(l)     ®    H2SO4(aq)

 

 

 

 

 

 

Assignment # 4            Physical and Chemical Changes Balancing Equations                       

 

Classify as a physical or chemical change.

 

1.         Spoiling of food                                              Chemical

                       

2.         Vaporization of ice                                          Physical

                       

3.         Stretching of a rubber band                             Physical

                       

4.         Dynamite explosion                                         Chemical

                       

5.         Shattering of glass                                           Physical

           

6.         Decaying of dead bodies                                 Chemical

                       

7.         Extraction of iron from form (Fe2O3)              Chemical

                       

8.         Spontaneous combustion of oily rags              Chemical

                       

9.         Grinding of wheat                                           Physical

                       

10.       Melting snow                                                  Physical

                       

11.       2 H2O          2 H2     +          O2    +     Energy                                  Chemical

           

12.       E    +     NaCl(s)                     NaCl(aq)                                                                            Physical

 

13.       Determine the physical state of each element at -5 0C (use the Handbook, Textbook, or Net to determine the melting point and boiling point of each).

 

                                                            mp                   bp                                physical state

 

a) Mercury                              -38.87 oC                     356.58 oC        liquid

 

b) Bromine                              -7.2 oC                         58.78 oC          liquid                                                  

c) Chlorine                              -100 oC                        -34.6 oC           gas                                                                 

 

 

Classify as a physical or chemical properties.

 

14.       Sugar chars when heated                     chemical property     

                       

15.       Yellow color of sulphur                      physical property

 

16.       Tarnishing ability of sulphur               chemical property

                       

17.       Flexibility of a spring                          physical property

                       

18.       Thermal conductivity of iron               physical property

                       

19.       Hardness of a diamond                        physical property

                       

20.       Stability of nitrogen                             chemical property

                       

21.       Describe 11 and 12 as exothermic or endothermic                                       

 

Write Ionic Formulas

 

22.       Aluminum oxide                                  Al2O3

                       

23.       Aluminum chloride                              AlCl3

                       

24.       Ammonium acetate                              NH4CH3COO

                       

25.       Barium phosphate                                Ba3(PO4)2

                       

26.       Calcium hydroxide                              Ca(OH)2

                       

27. Sodium hydroxide                                     NaOH

                       

28.       Strontium phosphate                            Sr3(PO4)2

                       

29.       Iron II phosphate                                 Fe3(PO4)2

                       

30.       Cobalt III sulphate pentahydrate          Co2(SO4)3.5H2O

                       

31.       Copper II nitrate hexahydrate              Cu(NO3)2.6H2O

 

Write an equation

 

32.       Sodium chloride dissolving in water (endothermic).

                       

                        NaCl(s)   +  energy      Na+(aq)   +   Cl-(aq)

 

33.       Lead II nitrate reacting with sodium phosphate to produce solid Lead II phosphate and sodium nitrate (exothermic and three chemicals are             aqueous).

 

            3Pb(NO3)2(aq)  +  2Na3PO4(aq)         Pb3(PO4)2(s)    +   6NaNO3(aq)

 

34.       List three chemical and physical properties.

 

 

Chemical:                   reactivity        flammability               stability          

 

Physical:                     mass                colour                          density

 

 

 

1.         Label each as chemical or physical.

 

            a) Ice cubes turn to water                                physical

            b) Steam forms water droplets in a mirror      physical

            c) Milk is made into ice milk                          physical

            d) Ice cubes shrink in a freezer                       physical

            e) Perspiration “dries”                                   physical

            f) Bromine is liquefied from solid bromine    physical

 

2.         What change in physical state occurs during the formation of the following?

 

            a) Rain            condensation

            b) Snow           freezing

            c) Frost            freezing

            d) Steam          evaporation

 

3)         A sealed glass bulb is half-filled with water, on which some ice and wood are floating.  The remainder of the bulb is filled with air.  How many physical states are present?  Identify them.

 

            solid:   ice and wood

            liquid:  water

            Gas:    air and water vapour

 

 

4)         Classify each of the following as a physical or chemical change.

 

a)         Photosynthesis (CO2   +   H2O          Sugars   +   oxygen)               Chemical

b)         Antifreeze boils out of a radiator                                                        Physical

c)         A firefly emits light                                                                             Chemical

d)         A nail is magnetized                                                                            Physical

e)         A nail rusts                                                                                          Chemical

f)         Leaves turn color in autumn                                                                 Chemical                                                      

g)         Food spoils                                                                                         Chemical

h)         Dynamite explodes                                                                              Chemical

I)         Grinding of wheat into flour                                                                 Physical

j)         Shattering of glass                                                                               Physical

k)         Extraction of iron from iron ore (Fe2O3)                                             Chemical

 

5)         Identify the chemical and physical changes in the following sequences:

           

a)         A lump of sugar is ground to a powder Physical and then heated in air Physical.  It melts Physical, then darkens Chemical, and finally bursts into flames and burns Chemical.

b)         Gasoline is sprayed into the carburetor Physical, mixed with air Physical, converted to vapor Physical, burned Chemical, and the combustion roducts expand the cylinder Physical.

           

 

 

Balancing Equations

 

1.         2KNO3                                            2KNO2            +          O2

 

 

2.         CaC2   +          2O2             Ca                   +          2CO2

 

 

3.         C5H12  +          8O2             5CO2   +          6H2O

 

 

4.         K2SO4  +          ­BaCl2                      2KCl   +          BaSO4

 

 

5.         2KOH +          H2SO4                     K2SO4 +          2H2O

 

 

6.         Ca(OH)2         +          2NH4Cl                   2NH4OH         +          CaCl2

 

 

7.         5C       +          2SO 2           CS2      +          4CO

 

 

8.         Mg3N2 +          6H2O          3Mg(OH)2     +           2NH3

 

 

9.         V2O5   +          5Ca             5CaO  +          2V

 

 

10.       2Na2O2                   +          ­2H2O          4NaOH           +          O2

 

 

11.       Fe3O4  +          4H2              3Fe      +          4H2O

 

 

12.       Cu       +          2H2SO4                 CuSO4  +       2H2O        +    SO 2

 

 

13.       2Al      +          3H2SO4                   3H2      +          Al2(SO4)3

 

 

14.       2Si4H10            +          13O2           8SiO2  +          10H2O

 

 

15.       4NH3   +          O2                           2N2H4 +          2H2O

 

16.       2C15H30           +          45O2           30CO2 +          30H2O

 

 

17.       2BN                 +          3F2                              2BF3                          +          N2

 

 

18.       CaSO4 . 2 H2O    +     2SO3                           CaSO4        +          2H2SO4

 

 

19.       2C12H26           +          37O2           24CO2 +          26H2O

 

 

20.       C7H6O3           +          7O2               7CO2    +       3H2O

 

 

21.       9Na                 +          4ZnI2                                 8NaI                +          NaZn4

 

 

22.       3LiAlH4          +      4BF3                3LiF     +    3AlF3      +   2B2H6

 

 

23.       HBrO3                +       5HBr                      3H2O              +          3Br2

 

 

24.       15O2   +      2All4C3   +          54H2O                     28Al(OH)3   +   6CH4

 

 

25.       2Ca(NO3)2 . 3H2O  +  3LaC2    2Ca(NO3)2   +  3La(OH)2    +   3C2H2

 

 

26.       1CH3NO2       +   3Cl2        1CCl3NO2       +         3HCl

 

 

27.       Ca3(PO4)2   +   3SiO2   +   5C      3CaSiO3   +   5CO   +   2P

 

 

28.       Al2C6   +   6H2O            2Al(OH)3   +        3C2H2

 

 

29.       2NaF   +          CaO   +   H2O                    CaF2   +   2NaOH

 

 

30.       4LiH   +          AlCl3                       LiAlH4             +          3LiCl

 

 

31.       2CaF2   +   2H2SO4   +   SiO2         2CaSO4   +     SiF4   +   2H2O

 

 

 

 

Some Tough Ones

 

Sorry, you are going to have to figure these out for yourself! Good luck!

 

 

___FeCl2  +   ___KNO3    +       ___HCl       ___FeCl3  + ___NO   +___ H2O  +   ___KCl

 

 

___Cu   +         ___HNO3                          ___Cu(NO3)2   +     ___NO   +     ___H2O

 

 

___ KMnO4     +   ___ HBr              ___MnBr2   +   ___Br2   +   ___KBr   +   ___H2O

 

 

___ K2Cr2O7   +           ___HCl        ___KCl   +   ___CrCl3   +   ___H2O   +   ___Cl2

 

 

 

 

 

 

Assignment # 5            Balancing Equations Naming Formulas

 

 

6.         Classify the following as elements, compounds, or mixtures:

 

a)         Methane  (CH4)                       compound

b)         Pizza                                        mixture

c)         Milk shake                               mixture

d)         Zinc                                         element

e)         Laughing gas                             compound

f)         Clean air                                 mixture

g)         Chocolate chip cookie             mixture

 

7.         A pure blue powder when heated in a vacuum releases a greenish colored gas and leaves behind a white solid.  Is the original blue powder a compound or element?  Explain.

 

            Compound, because it decomposed into two elements.

 

 

 

8.         A shiny, metallic-like substance conducts an electric current without a change in its properties.  The substance is heated until it liquefies and then   an electric current is passed through the liquid again without a change in properties.  Is the substance likely to be an element or compound? Explain.

 

Element, because it could not be decomposed by electrolysis or heating.

 

9.         Describe the difference between chemical and physical change in terms of what occurs with the atoms involved.

 

Chemical change involves chemical bonds being broken and new ones being formed.

Physical change involves changes in state (s), (l), (g), and (aq). Chemical bonds are not broken.

 

1.         2Al      +          6HCl                       2AlCl3 +          3H2

 

2.         Zn        +          2KOH                     K2ZnO2   +      H2

 

3.         B2O3   +          3Mg                        3MgO +          2B

 

4.         2C6H11OH      +          17O2           12H2O  +        12CO2

 

5.         2C12H26           +          37O2              26HOH   +    24CO2

 

6.         2Na     +          2H2O                      2NaOH           +          H2

 

7.         2PbS   +          3O2                         2PbO  +          2SO2

 

8.         SiCl4    +          4Na                         Si         +          4NaCl

 

9.         2Mg    +          CO2                         2MgO +          C

 

10.       2Al      +          3H2SO4                   Al2(SO4)3   +   3H2

 

Write Formulas for each

 

11.       Zinc phosphate                                                Zn3(PO4)2

 

12.       Ammonium carbonate                                      (NH4)2CO3

 

13.       Iron III oxalate                                     Fe2(C2O4)3

 

14.       Copper II tripolyphosphate pentahydrate        Cu5(P3O10)2.5H2O

 

15.       Cobalt II borate                                               Co3(BO3)2

 

16.       Triphosphorus tetroxide                                  P3O4

 

17.       Dicarbon hexachloride                                    C2Cl6

 

18.       Trisilicon octafluoride                                                Si3F8

 

19.       Sodium tetraborate                                          Na2B4O7

 

20.       Aluminum dichromate                         Al2(Cr2O7)3

 

21.       Calcium oxide                                                 CaO

 

22.       Silver thiosulphate                                          Ag2S2O3

 

 

Write balanced chemical equations and include phase symbols for each formula.

 

23. Aqueous calcium nitrate is reacts with a solution of sodium phosphate producing solid calcium phosphate and aqueous sodium nitrate.

 

            3Ca(NO3)2(aq)     +    2Na3PO4(aq)      Ca3(PO4)2(s)    +   6NaNO3(aq)

 

24. Gaseous nitrogen trihydride reacts with oxygen gas to produce gaseous nitrogen monoxide and gaseous water and energy.

 

 

            4NH3(g)   +   5O2(g)         4NO(g)  +  6H2O(g)   +  energy

 

 

25. Phosphoric acid reacts with Calcium hydroxide both in solution to produce and aqueous salt and water.

 

 

            2H3PO4(aq)   +  3Ca(OH)2(aq)          Ca3(PO4)2(aq)  +  6H2O(l)

 

 

26. Write an equation for the combustion of sucrose.

 

 

            C12H22O11(s)   +  12O2(g)     12CO2(g)   +   11H2O(l)

 

 

27. Write an equation for the cellular respiration of vitamin C.

 

 

            C6H8O6(s)   +  5O2(g)     6CO2(g)   +   4H2O(l)

 

 

28. Describe what you know about covalent or molecular compounds.

 

Formula starts with a nonmetal

Shared electrons

Full valance shells

Stable compounds

 

Worksheet # 6                        Balance each equation.

 

1.         2Sb                  +          5Cl2                         2SbCl5            

 

2.         2FeCl2                     +          Cl2                           2FeCl3

 

3.         2P                    +          3I2                           2PI3

 

4.         Na2S                +          2HCl                       2NaCl             +          H2S

 

5.         3NaOH           +          FeCl3                       3NaCl +          Fe(OH)3

 

6.         3KOH             +          H3PO4                     K3PO4 +          3H2O

 

7.         2NaOH           +          CuSO4                    Na2SO4   +   Cu(OH)2  

 

8.         2HNO3            +          Ca(OH)2                  2H2O  +       Ca(NO3)2

 

9.         2NH3               +          3CuO                     3H2O  +   3Cu            +   N2                                                                                                      

 

10.       N2        +    4C    +       Na2CO3                  2NaCN            +    3CO

 

11.       2NH3               +          5O                           2NO    +          3H2O

 

12.       4NH3               +          7O2                         4NO2   +          6H2O

 

13.       2NH3               +          4O2                         N2O5   +          3H2O

 

14.       2P                    +          5N2O                       P2O5    +          5N2

 

15.       2Al                  +          6HCl                       2AlCl3 +          3H2

 

16.       Zn                    +          2KOH                     K2ZnO2   +      H2

 

17.       B2O3               +          3Mg                        3MgO +          2B

 

18.       2CH3OH         +          3O2                         4H2O  +          2CO2

 

19.       C6H12O6                                                     2C2H5OH   +    2CO2

 

20.       2Na     +          2H2O                                  2NaOH           +          H2

 

21.       2PbS               +          3O2                         2PbO  +          2SO2

 

22.       SiCl4    +          4Na                                     Si         +          4NaCl

 

23.       2Mg    +          CO2                                     2MgO +          C

 

24.       2Al      +          3H2SO4                               Al2(SO4)3   +   3H2

 

 

 

 

 

Write balanced chemical formulas for each ionic compound.

 

25. Calcium hydroxide                        Ca(OH)2     

 

26. Aluminum sulphate                        Al2(SO4)3

 

27. Iron III oxide                                 Fe2O3               

 

28. Zinc acetate                                   Zn(CH3COO)2       

 

29. Barium carbonate                          BaCO3             

 

30. Sodium phosphate                         Na3PO4  

 

31.Cobalt II nitride                              Co3N2

 

32. Gallium sulphate                           Ga2(SO4)3

 

33. Aluminum fluoride                        AlF3             

 

34. Ammonium sulphate                       (NH4)2SO4

 

35. Aluminum acetate                          Al(CH3COO)3

 

Write balanced chemical formulas for each molecular (covalent) compound.

 

36. carbon monoxide                           CO            

 

37. dinitrogen tetraiodide                    N2I4

 

38. triphosphorus hexafluoride            P3F6  

 

39. dinitrogen dioxide                         N2O2          

 

 

Write balanced chemical equations for each word equation. Include phase symbols for all formulas.

 

40. Solid sodium oxide dissolves in water to make sodium oxide solution.

 

            Na2O(s)                    2Na+(aq)                    +                O2-(aq)

 

 

41. Solid aluminum sulphate dissolves in water to make a solution

 

            Al2(SO4)3(s)             2Al3+(aq)                   +          3SO42-(aq)

 

 

42. Barium phosphate plus sodium sulphate (both in water) yields solid barium sulphate and aqueous sodium phosphate.

 

            Ba3(PO4)2(aq)  +  3Na2SO4(aq)    3BaSO4(s)  +  2Na3PO4(aq)

 

 

43. Lead metal added to Sulphuric acid solution produces lead IV sulphate precipitate and diatomic hydrogen gas.

 

            Pb(s)  +  2H2SO4(aq)    Pb(SO4)2(s)  +  2H2(g)

 

 

44. Potassium iodide (aq) plus lead II nitrate (aq) yields potassium nitrate (aqueous) plus lead II iodide (solid).

 

            2KI(aq)  +  Pb(NO3)2(aq)    2KNO3(aq)  +  PbI2(s)

 

 

45. Calcium carbonate (solid) plus aqueous hydrochloric acid yields (aqueous) calcium chloride, carbon dioxide gas and water.

 

            CaCO3(s)  +  2HCl(aq)    CaCl2(aq)  +  CO2(g)  +H2O(l)

 

 

46. Potassium nitrate (aq) plus iron III hydroxide (aq) yields iron III nitrate (aq) plus potassium hydroxide (aq).

 

            3KNO3(aq)  +  Fe(OH)3(aq)    Fe(NO3)3(aq)  +  3KOH(aq)

 

 

You are good if you can do these. On your own of course!

 

1.         ___HCl    +   ____K2CrO4   ____KCl   + ____CrCl3    +____H2O      +____Cl2

 

 

2.         __K2Cr2O7  +  __KI   +  __H2SO4     __K2SO4  + __Cr2(SO4)3 + ___I2 +___H2O

 

 

 

Worksheet # 7            Measurement and Uncertainty        

 

1. Five different voltmeters are used to measure the voltage in a circuit. Determine the average and uncertainty.

 

25.61V      

25.63V

25.65V                        25.63 ± 0.02 V

25.64V

25.63V

Six thermometers give the following readings. Determine the average and the uncertainty.

 

352.4 0C

352.5 0C

352.6 0C

352.5 0C

352.7 0C

352.6 0C

 

                                                                       

2.         Determine the average and uncertainty for the data:

 

            25.56 g            25.54g             25.52g             25.53g             25.55g

 

Answer            25.54 ±  0.02 g

 

3.         Determine the average and uncertainty for the data:

 

            5.216 oC         5.218 oC         5.213 oC         5.214 oC         5.416 oC        

 

            Answer                                               

 

4. How many significant figures are in each number?

 

25.63               4                                  101                  3                      0.0075             2

 

0.0002             1                                  1.00                 3                      2.005               4

 

10.031             5                                  1.0002             5                      10005              5

 

0.00521           3                                  2.51 x 104        3                      3 x 10-7            1

 

2 x 105             1                                  2.00 x 103        3                      250.                 3

 

5. Round off to three significant figures.

 

0.05211                            0.0521                                     0.0087251                    0.00873          

 

85.337                               85.3                                        2.6177 x 10-5                    2.62 x 10-5          

 

2.5175 x 10-18                       2.52 x 10-18                                    25.731 x 105                 2.57 x 106

 

 

Round off each measured number to three significant figures.

 

6.         0.002567                                 .00257

 

7.         94549                                      9.45 x 104

                       

8.         15.00                                       15.0

 

9. Round off the following numbers to three significant figures:                                                        

 

a)         35.234      35.2                                    b)         2.34521                       2.35                             c)         0.035219         0.0352

d)         2533521   2530000                             e)         6255520000                6260000000

 

10. State the number of significant figures in each approximate number.

                       

a)         305                  3          b)         25.25               4                      c)         3.00     3

d)         0.001               1          e)         3.0050                    5                

f)         6.25 x 1023           3                 g)         7.00 x 10-2       3                      h)         1001    4

 

11. Add or subtract the measured quantities.

 

   25.31                           22.0                          22.7                             35.271

+   6.4                          +   0.04                    +    0.77                      +     0.2

   31.7                             22.0                          23.5                             35.5

 

 22.71                            25.217                         2.51639                       8.0558

- 0.299                         + 0.017                  -     1.2358                    +     .3259297

22.41                             25.234                        1.2806                         8.3817

 

                                     

 

25.634   +  2.365  -   0.25498  +  0.225  =                                          27.969

 

12.       15.239  +  5.36                                                                        20.60

 

 

13.       2.6679   -    1.23                                                                      1.44

 

 

14.       2.059378  x  1024    +   5.3    x   1022                                       2.112 x 1024

           

 

15.       8.5  x  10 -24    +   5.37894    x   10-25                                     9.0 x 10-24

 

 

16.       2.3  x  10 16    +   8.224    x   1019                                            8.226 x 1019

 

 

17.       5.6  x  10 –8    +   9.5563    x   10-6                                           9.612 x 10-6

 

 

18.       9.55  x  10 -10    +   5.4455    x   10-12                                       9.60 x 10-10

 

 

19.       2.66  x  10 -16    +   3.445    x   10-18                                         2.69 x 10-16

 

 

20.       3CaSi2   +       2SbCl3         6Si   +              2Sb   +             3CaCl2

 

 

21.       2TiO2      +     B4C     +     3C                      2TiB2   +   4CO

 

 

22.       4NH3   +          5O2             4NO   +           6H2O

 

23.       SiF4     +   8NaOH           Na4SiO4     +      4NaF   +   4H2O

 

 

24.       2NH4Cl   +      CaO      2NH3   +  CaCl2   +   H2O

 

 

25.       4NaPb   +   4C2H5Cl      Pb(C2H5)4   +   3Pb   +   4NaCl

 

 

26.       Be2C               +   4H2O      2Be(OH)2   +   CH4

 

 

27.       4NpF3   +   O2   +   4HF      4NpF4   +   2H2O

 

 

28.       3NO2   +   H2O      2HNO3   +         NO

 

 

 

Worksheet # 8

 

1.         25  x 3                         2.  3.35  x  0.26                       3.  799  x  877

 

            8  x  101 or  80                        0.87                                  7.01  x  105 or  701000

 

4.         (6.2 x 103)( 3.55 x 1012)                      5.         (6.3 x 107)(2.51 x 10-7)

                                                                                                (3.214 x 10-5)

                       

                        2.2  x  1016                                                      4.9  x  105

 

6.         (7.52 x 1016)(3.1 x 1012)                      7.         3.5 x 102  ÷  3.1 x 103

            (2.5 x 10-7)

 

                        9.3  x  1035                                                      1.1  x  10-1

 

8. (2.00 x 1023)(3.51 x 10-22)(3.5 x 103)

      (7.5 x 10-3)(3.511 x 1012)(6.6 x 10-6)

 

                        1.4

 

9.  (5.200 x 10-5)(6.02 x 10-12)(3.58 x 1017)

       (2.337 x 10-3)(6.2154 x 1012)(5.22 x 10-12)

 

                        1.48  x  103

 

10.       156   x   256   x  21   x  0.0005687                                         

0.02569   x   13.235   x   2654           

 

                                    0.53  

 

11.       (8.5  x  10 -24)  ( 5.37894    x   10-25)   ( 4.532    x   1015)

             (2.059378  x  10 24)  (5.3    x   1022)  ( 9.37894    x   10-13)

 

                                                2.0  x  10-67

 

 

12.       25.7 x  0.21                 5.4

                       

13        35 x 105                      3.7  x  103

 

14.       51.71 x  22.3                1.15  x  103              

 

15.       22 x 305                      6.7  x  103

 

 

16. Write three examples of exact numbers.

 

6 fish   8girlfriends     3pens

 

17. Write three examples of approximate numbers.

 

1.2 cm             2.45 Kg           2.233 V

 

Circle the uncertain digit and underline the uncertainty in each of the following numbers.

 

18.       35.2 ±   0.1 g                19.        22.221 ± 0.005 mm                20.         100. ± 2 lb.

 

21. Give the largest and smallest value of the approximate number

 

 35.21 ± 0.02 g                        largest: 35.23 g                      smallest: 35.19 g

 

 

22.          26.215                      23.    65.222                            24.    22  -  0.01

              -  0.3                                 +  1.03                                       

               25.9                                   66.25                                          22

 

25.          10. + 0.1                   26.  33.3  +  0.35                     27.  29.39  + 0.2

 

               10.                                        33.7                                         29.6

 

 Calculate the average measurement and the uncertainty of each measuring device below:

 

28. The mass (in grams) readings on a balance:

 

58.56

58.59

58.51

58.61

58.57

58.56

 

Answer            58.6  ±  0.1 g

 

 

29. The voltage (in mV) readings on a number of voltmeters:

                       

123.2

            124.5

124.0

124.3

124.3

 

Answer            124.3  ±  0.3 mV

 

30. State the number of significant digits for each number:

 

a)  0.00200 L    3         b)         5.000 g            4          c)         1.00003 A 6

 

d)  1000.000 Mm   7  e)         2.5 x 1076               2                 f)         78.89 m     4

 

 

31. Perform the following calculations and round to the appropriate level of uncertainty (assume all numbers are from measurements):

 

a)         18 + 0.21                                             18                   

 

 

b)         62.1  x  3021.56                                  1.88  x  105

 

 

c)         1.05 g + 253.8 mg + 24.98 mg Watch units!  

           

            1.05

            0.2538

            0.02498

 

            1.32 g

 

d)         (9.442 x 10-3)(3.21 x 108)                    3.03  x  106

 

 

e)         231.4  -  8.2295                                   223.2                          

 

 

f)         (8.995 x 106) + (3.55 x 107)                   4.45  x  107

 

 

g)         12.0355 + 1.024                                  13.060

                       

 

h)         (4.56 x 10-8)(2.5  x 1035)                      1.1  x  1028

                                                                                                           

 

i)         (9.24 x 1010)(5.233  x 104)                   4.84  x  1015

 

 

32. State the difference between accuracy and precision.

 

 

Accuracy refers to how close a measurement is to the true or accepted value.

 

Precision is the opposite of uncertainty and refers to the variation of a measurement with different measuring devices.

The lower the variation the greater the precision and the higher the uncertainty.

 

 

 

Worksheet # 9         Unit Analysis 1          

 

All work must be shown as illustrated below. The work is more important than the answer.

 

1.         527 g to mg

 

527 g  x  1 x  103 mg               =          5.27  x  105 g

                   1g

 

2.         1.05  x  106 um to m

 

1.05  x  106 μm  x        1 g                  =          1.05 m

                               1  x  106 μm

 

 

3.         2.148 ML to mL

 

 

2.148 ML        x          1  x  106 L       x          1  x  103 mL    =          2.148  x  109 mL

                                       1ML                              1L

 

4.         0.0235 mg to Kg

 

0.0235 mg       x          1g                    x          1kg                  =          2.35  x  10-8 kg

                                    1  x  103 mg                 1  x  103 g

 

 

5.         8.32  x 10-4  mL  to ML

 

           

8.32  x 10-4  mL  x      1 L        x        1 ML              =          8.32  x  10-13 ML

                                    1  x  103 mL    1  x  106 L

 

 

6.         772.5 us to ms

 

772.5  μs         x          1 ms                =          0.7725 ms

                                    1  x  103 μs     

 

 

7.         3.06500 cg to kg

 

3.06500  cg     x          1 g                   x          1 kg                 =          3.06500  x  10-5 Kg

                                    1  x  102 cg                  1  x  103 g

 

 

8.         9.450 Mm to mm

 

9.450 Mm       x          1  x  106 m       x  1  x  103 mm            =          9.450  x  109 mm

                                      1Mm                     1 m

 

 

9.         5.64  x  103  mm2 to cm2

 

5.64  x  103  mm2         x          1 cm2               =          5.64  x  101 cm2

                                                1  x  102 mm2  

 

 

 

 

 

 

1.         605 µm  to mm

 

0.605 mm

 

 

2.         6.5  x  10-6   Mm  to m

 

6.5 m

 

 

3.         20.0 km  to cm.

 

2.00  x  106 cm

 

 

 

4.         8.774  x  1015  µm to Mm.

 

8774 Mm

 

 

5.         25 cL  to  ML

 

2.5  x  10-7 ML

 

 

6.         648 kPa  to  mPa

 

6.48  x  108 mPa

 

 

7.         2.665  Mg  to  µg

 

2.665  x  1012 μg

 

 

Worksheet # 10

   

Use unit analysis and the conversion factors to perform the following conversions:

 

2.210 lb  =  1.000 kg               14 lb  = 1 stone (defined)        2000 lb   =  1 ton (defined)

 

1.61 km   =   1.00 mile            4.54 L  =  1.00 gallon              16 oz  =  1 lb (defined)

 

 

1.       170 lb to kg

           

170 lb x          1 kg         =    76.9 kg

                        2.210 lb

 

 

2.       648 KPa to atm

 

648 kpa     x     1 atm             =          6.40 atm

                        101.3 kpa

 

 

3.       256 oz to tons

 

256 oz             x          1 lb         x       1 ton    =          8.00  x  10-3  tons

                                    16 oz               2000 lb

 

 

4.       0.025 ton to mg

 

           

0.025 ton  x  2000 lb    x   1 kg   x   1  x  103 g   x     1  x 103 mg   =    2.3  x  107  mg

                        1 ton           2.21 lb      1 kg                    1 g

 

 

 

5.       0.236 Gal to mL

 

1.07  x  103 mL

 

 

6.       5.8 x 106 mL to Gal

 

1.3  x  104 Gal

 

 

7.       5.66 x 106 mg to stones

 

0.893 stones

 

 

8.       15 miles to mm

 

2.4  x  107 mm

 

 

9.       5.63 x 109 µm to miles

 

3.50 miles

 

 

10.         152 mL to gal

 

152 mL  x       1 L         x       1 gal    =          3.35  x  10-2  gal

                        1000 mL         4.54 L

 

 

 

11.         8.6 stone to oz

 

256 stone  x    14 lb       x       16 oz   =          1.9  x  103  oz

                        1 stone             1 lb

 

 

 

12.       4.3 m to miles

 

4.3 m  x           1 Km      x       1.00 mile         =          2.7  x  10-3  miles

                        1000 m            1.61 Km

 

 

 

13.       15.2 mi/gal to L/km

 

                       

1 gal          x    4.54 L    x       1 mi                 =          0.186 L/km 

15.2 mi            1 gal                1.61 km

 

 

 

14.       2.3  gal to mL

 

1.0  x  104 mL

 

 

 

15.       45.2 oz to stones

 

           

0.202 stones

 

 

15.       46.3 miles to m

 

7.45  x  104 m

 

 

 

17.       36 L/km to mi/gal 

 

0.078  mi/gal

           

 

18.       If 3 dogs are worth 2 cats, 8 cats are worth 2 lions, 5 lions are worth 8 elephants, 2 elephants are worth 8700000 ducks, 47 ducks are worth 63 geese, 14 geese are worth 27 snakes, 42 snakes are worth 778396 fruit flies, and a dog costs  $205.00, how much does a fruit fly cost? Use unit analysis and assume all conversions are exact.

 

1 FF  x  42 sn       x    14 ge  x 47 du x  2 el                x  5 li   x  8 ca x  3 do  x $205.00

           778396 FF      27 sn     63 ge     8700000 du        8 el      2 li       2 ca       1 dog

 

                        $ 4  x  10-9  for  one fruit fly

 

 

 

19.       Light travels 9.46 x 1015 m in one year. This distance is called a light-year. Calculate the speed of light in metres per second. Use unit analysis.

 

           

            3.00  x  108 m/s          

 

 

 

 

20.       The following trade ratios are used in a small country in the Middle East near Iran called Yrtsimehc.  A young man is in love with a beautiful woman, however, he must pay a dowry of 12 camels to marry her.  The young man is a yam farmer and has only 12,000 yams to trade.  Can he marry his true love?    

Use unit analysis to support your answer.

            15 pigs = 2 cows         3 cows = 2 horses       17 chickens = 1 pig    

            2 horses = 3 camels     20 lbs of figs = 16 chickens    56 yams = 10 lbs of figs

 

 

 

1.3 x 102 camels  Yes he can marry and have camels left over for the honeymoon.

 

 

 

 

 

 

Worksheet # 11            Review

 

Given:

$0.2045 Can.

=

1.00  Francs (French)

 

$2.1860 Can.

=

£ 1.00 (UK)

 

$1.3572 Can.

=

$ 1.00 U.S.

 

$0.1534 Can.

=

1.00 Peso (Mexico)

 

$0.0109 Can.

=

¥ 1.00 (Japanese Yen)

 

$0.0263 Can.

=

1.00 Rupee (India)

 

$1.00 U.S.

=

1.9325 Marks (Germany)

Convert:

1.      $300.00 Can. to £.

 

            137.24 £.

 

2.      $1025.00 Can. to pesos.

 

            6681.88 pesos

 

3.      $450.00 U.S. to yen.

 

            56031 yen

 

4.      £ 652.23 to francs.

 

            6972.0 francs

 

5.      85.2 Marks to £.

 

            27.4 £

 

6.      3842.35 Yen to Rupees.

 

            1592.46 Rupees

 

7.      9668.75 Francs to Marks.

 

            2815.39 marks


Black Market Trading Conversions

 

Given:

1 Ticket

=

2 CDs

 

5 Buttons

=

3 T Shirts

 

4 Tickets

=

1 Back Stage Pass

 

1 CD

=

3 T Shirts

 

7 Posters

=

3 Buttons

 

Convert:

1.                      28 Posters to buttons.

 

            28 Pos             x          3 But               =          12 buttons

                                                7 Pos

2.                      10. CDs to tickets.

 

            10 CD             x          1 ticket           =          5.0 tickets

                                                 2 CD

3.                      100. Buttons converted to CDs.

 

            20.0 CDs

 

4.                      1 Back Stage Pass converted to T Shirts.

 

            24 T-shirts

 

5.                      280. Posters to Back Stage Passes.

 

            3.00 BSP

 

6.                      6 Back Stage Passes to buttons.

 

            240 buttons

 

 

Use unit analysis to perform the following conversions:

 

 

7.         6.372 hL to mL            6.372 x 105 mL

 

            6.372 hL    x    1  x  102 L      x  103 mL=      6.372  x  105 mL

                                     1 hL                   1 L

 

8.         4.9 x 1015 µg to Mg      4.9 x 103 Mg

 

            4.9  x  103 Mg

 

9.         8.774 x 103 cm3 to m3  0.008774 m3

 

            8.774  x  10-3 m3

 

 

10. Given the following relationships, determine how many zings can be obtained when you trade 20.6 balls.

            4 clangs  = 3 dangs    7 dangs  = 3 jars        2 balls  = 5 clangs      6 jars  = 1 zing  

 

 

 

            2.76 zings

 

 

 

11. State the number of significant digits for each number:

      a)  25.0 g   3            b)       1000 g  infinite            c)  25.036 A    5            d)  5.214  x  10-62  mL  4

                                                1 kg

3                                        infinite                        5                                              4

 

e) 0.0000005 L      1                        f) 8.2000 m

1                                                    55

 

Determine the average and uncertainty given the following measurements from a

 

12.       Centigram balance      

 

82.62 g 

82.54 g 

82.48 g            82.6  ±  0.1 g   Note the uncertainty is in the first decimal place.

82.72 g 

82.65 g                                    82.6 ± 0.1 g

 

13.       Show the interval on the number line that represents the range for the above measurement after it has been round off correctly.

 

           

82.5

 

82.6

 

827

 
 

 


Write chemical formulas for each ionic or molecular compound.

 

 

14.       Iron III oxide                                       Fe2O3                                                 

 

15.       Triphosphorous hexoxide                    P3O6                                                                                                               

16.       Aluminum hydroxide                           Al(OH)3                                                         

 

17.       Nickel II phosphate octahydrate          Ni3(PO4)2 . 8H2O                                                        

 

 

Name each chemical formula

 

 

18.       K3PO4                                                  Potassium phosphate                                   

19.       Mn3P2                                                  Manganese II phosphide                                                                              

20.       Ga2(SO3)2 . 6H2O                                Gallium sulphite hexahydrate                                                                                              

21.       P4O10                                                   tetraphosphorus decoxide                                                               

 

 

 

 

 

Worksheet # 12         Density Calculations           

                    

 Density calculations

 

1.         Calculate the volume in cm3 of 25.3 g of iron.

 

25.3 g     x     1 cm3                 =          3.22 cm3

                      7.87 g

 

2.         Calculate the mass of 65 cm3 of iron in mg.

 

65 cm3             x       7.87 g             x      1000 mg        =          5.1 x 105 mg

                                 1 cm3                        1g

 

 

3.         Calculate the density of an expensive element that has a mass of 56.76 g and a volume of 2.938 cm3. Determine the identity of the element.

 

D         =          56.76 g            =          19.32 g/cm3

                        2.938 cm3

 

Au

 

4.         Calculate the density of a radioactive element that has a mass of 164.3 g and a volume of 8.693 cm3. Determine the identity of the element.

 

 

D         =          164.3 g            =          18.90 g/cm3

                        8.693 cm3

 

U

 

 

5.         Determine the volume in mm3 of a 55.3 g sample of lead.

 

55.3 g     x     1 cm3       x        1000 mm3        =          4.88   x  103 mm3

                      11.34 g              1 cm3

 

 

6.         Determine the mass of a 59.3 mm3 sample of lead.

 

59.3 mm3         x          1 cm3               x          11.34 g                        =          0.672 g

                                    1000 mm3                    1 cm3

 

 

 

7.         Determine the volume in mm3 of a 1.0 x 10-8 ton sample of gold.

 

 

1.0 x 10-8 ton   x   2000 lb   x    1.00 kg   x   1000 g    x    1 cm3    x    1000 mm3     =   0.47 mm3

                                1 ton             2.21 lb          1 kg           19.32 g          1 cm3

 

 

 

Worksheet 13         Practice Test

 

 

 

Balance each equation.

 

1.         2Sb                  +          5Cl2                                     2SbCl5

 

2.               2NH3   +          4O2                          N2O5    +          3H2O

 

3.         2C12H26            +          37 O2                       24CO2 +          26H2O

 

4.         2Al       +         3H2SO4                       3H2      +          Al2(SO4)3

 

 

            (The next one is the tough one!!)

 

5.         3Cu    +           8HNO3                       3Cu(NO3)2   +    2NO     +      4H2O   

 

 

 

            Write a balanced equation for each word equation including phase symbols.

 

6.         Barium phosphate plus sodium sulphate (both in water) yields solid barium sulphate and aqueous sodium phosphate.

 

            Ba3(PO4)2(aq)  +  3Na2SO4(aq)    3BaSO4(s)  +  2Na3PO4(aq)

 

 

            Write chemical formulas for each ionic or molecular compound.

 

 

7.         Mercury II sulfide                                                       HgS

 

8.         Diphosphorous pentoxide                                            P2O5                                                   

 

9.         Barium hydroxide                                                        Ba(OH)2

 

10.       Copper II sulphate hexahydrate                                   CuSO4.6H2O

 

 

Name each chemical formula

 

 

11.       Na3PO4                                                            sodium phosphate

 

12.       Co3P2                                                               cobalt II phosphide

 

13.       Al2(CO3)2 . 6H2O                                             aluminum carbonate hexahydrate

 

14.       Si2I6                                                                 disilicon hexaiodide

 

 

15.       Determine the average and uncertainty for the data:

 

            25.56g

            25.54g

            25.52g

            25.53g

            25.55g

 

Answer            25.54  ±  0.02g

 

 

16.       Determine the average and uncertainty for the data:

 

            5.216 oC         

            5.218 oC         

            5.213 oC         

            5.214 oC         

            5.416 oC          reject 

 

Answer            5.215  ±  0.003 oC                              

 

Round off each measured number to three significant figures.

 

17.       0.002567                     0.00257

 

18.       94549                          94500              or        9.45  x  104

                       

19.       15.00                           15.0

 

 

Add or subtract the measured quantities.

 

20.       15.239  +  5.36                                                            20.60

 

 

21.       2.6679   -    1.238                                                        1.430                          

 

 

22        12.65449   +   0.2493                                                                                   12.9038

 

 

23.       8.57  x  107   +   5.37894    x   109                               5.4646  x  109

 

 

            Simplify the following rounding to the correct number of significant figures.

 

 

24.         156   x   256   x  21   x  0.0005680                                                   

           

                .02569   x   13.235   x   2654                                  Answer            0.53

 

 

25.       (8.5  x  10 -24) (5.37894   x  10-25) ( 4.532  x  1015)

                                                                                                                                                                 

            (2.059378  x 10 24)  (5.3   x  1022)  (9.37894   x  10-13)

 

                                                                                                Answer            2.0  x  10-67

 

                        Complete the relationships:

26.       1 Mg                =          1  x  106 g                    27.       1 Km               =          1  x  103 m

28.       1 L                   =          1  x  103 mL                 29.       1 g                   =          1  x  109 ng

30.       1  x  106 µs      =          1 s                               31.       1  x  102 cg       =         1  g

32.       1  x  1012pg     =          1 g                               33.       1  x  1012 s       =          1Ts

 

 

                        Use unit analysis to perform the following conversions:

 

34.       8.13 kg to cg.

 

            8.13  x  105 cg

 

 

 

 

35.       2.3 x 1012 µm to Mm.

 

            2.3 Mm

 

 

 

 

36.       1.52 x 104 Mm to mm.

 

            1.52 x 1013 mm

 

 

 

37.       2.13 Mg to cg.

 

            2.13 x 108 cg

           

 

 

 

38.       8.88 x 1012 mm to Mm.

 

            8.88 x 103 Mm

 

 

 

 

39.       8.52 x 10-8 Mm to pm.

 

            8.52 x 1010 pm

 

 

 

 

 

 

 

Use unit analysis and the conversion factors to perform the following conversions:

 

2.210 lb  =  1.000 kg               14 lb  = 1 stone (defined)        2000 lb   =  1 ton (defined)

 

1.61 km   =   1.00 mile            4.54 L  =  1.00 gallon              16 oz  =  1 lb (defined)

 

 

40.       635 mL to gal

 

            0.140 gal

 

 

 

41.       3.8 stone to oz

 

            8.5  x  102 oz

 

 

 

42.       25.6 m to miles

 

            0.0159 miles

 

 

 

43.       26 mi/gal to L/Km

 

            1 gal   x    4.55 L   x   1 mi                 =          0.11 L/Km

            26mi        1gal             1.61 km

 

44.       14.5 L/Km to mi/gal

 

            1 Km               x          4.54 L    x       1 gal                =          0.194 mi/gal

            14.5 L                         1 gal                1.61 km

 

 

 

 

 

45.       Mr. Iannone’s chemistry class is at a “Periodic Table” party.  Everyone at the party is hungry, and they decide as a group that everyone wants sushi, california rolls.  No one at the party has any money though.  One bright student remembers that the class has a credit for 15 pizzas at Boston Pizza.  Using the conversion factors below, will Mr. Iannone’s class be able to buy enough California rolls for their “Periodic Table” party if there are 28 students at the party? Assume all conversions are exact.

 

            1 pizza = 2 Wendy’s burgers                           100 brussel sprouts = 3 pieces of toast

            5 pieces of toast = 1 california roll                 30 tacos = 1 bag of Doritos

            4 Wendy’s burger = 7 tacos                            6 bowls of lime jello = 3 bag of Doritos

            1 bowl of lime jello = 1000 brussel sprouts

 

15 Pizzas x  2 WB  x  7 Tacos  x  1 Bag D x  6 Lime Jello  x  1000 Brussels  x  3 Toast  x  1 Cal Roll = 21 Cal Rolls

                    1 Pizz       4 WB                       30 Tacos     3 Bag D          1 Lime Jello      100 Brussels   5 Toast

 

Sorry, the answer is no.

 

 

Read each scale and estimate the measurement to the correct number of significant figures.

 

46.                                        6.62 mL        

                                            

                                                              

                                                          

 

 

47.                                         52.5 ml 

 

                                                                               

 

 

 

48.                                         21.5 mL

                                                             

 

 

 

49.                                                                              2.97 cm

 

 

 

 

       

                                                                                                                     

 

 

 

50.                                                                             9.23 mL

 

                                                                  

 

 

  51.       Micrometer Scale in mm.                            5.78 mm                                                                                                                                                                                  

File:578metric-micrometer.jpg

                                                                                   

 

 

52.       Vernier Scale in cm.                                    1.63 cm 

 

 

http://www.tresnainstrument.com/images/edu/3_RD2.jpg

 

                                                                                        

53.       Micrometer Scale in mm                            10.93 mm

 

http://www.faqs.org/photo-dict/photofiles/list/730/1144micrometer.jpg  

 

                                                                                               

 

 

           

 

 

 

54.       Calculate the volume in cm3 of 65.3 g of copper.

 

             7.29 cm3

 

 

55.       Calculate the mass of 208 cm3 of copper in mg.

 

            1.86 x 106 mg

 

 

56.       Calculate the density of an explosive element when wet that has a mass of 46.26 g and a volume of 24.70 cm3. Determine the identity of the element.

 

 

             1.873 g/cm3

 

57.       Calculate the density of a element found in your bathroom that has a mass of 46.31 g and a volume of 6.4409 cm3. Determine the identity of the element.

 

 

             7.190 g/cm3

 

 

58.       Determine the volume in mm3 of a 44.3 g sample of lead.

 

            3.90 x 103 mm3

 

 

59.       Determine the mass of a 19.3 mm3 sample of lead.

 

 

            0.219 g

 

60.       Determine the volume in mm3 of a 6.44 x 10-10 ton sample of copper.

 

           0.0650 mm3

 

61.       Read the graduated cylinder in mL.           21.31 mL

 

. http://www.eclipse.net/~pankuch/Newsletter/Pages_NewsF06/Methanol_Economy_files/image007.jpg

 

 

 

 

62.       Read the graduated cylinder in mL.           52.8 mL

 

http://www.uwplatt.edu/chemep/chem/chemscape/LABDOCS/CATOFP/measurea/concentr/titrate/pic/00322409.jpg 

 

   

63.       Read the buret in mL.             0.60 mL

 

http://www.chem.uiuc.edu/chem103/titration/images/readInitial.jpg                                                       

 

 

64.       Read the buret in mL.              15.45 mL

 

http://genchem.rutgers.edu/buread1.jpg        

 

 

65.       Read the buret in mL.             38.53 mL

 

http://biology.clc.uc.edu/Fankhauser/Labs/Anatomy_&_Physiology/A&P203/Titrations/VitC_protocol/15_finish_meniscus_P5020011.JPG