Unit I Safety Unit
Analysis Measurement
Lesson Day Date Topic Homework
1. Safety
2. Disssociation and Ionic Formulas 2
3. Balancing and Word Equations 3
4. Physical and Chemical Changes 4
6. Review and Lab Preparation 6
7. Uncertainty Lab Day 1 Lab Handout
8. Uncertainty Lab Day 2
9. Measurement and Uncertainty 7
16. Test
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.
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.
29.
30.
31.
32.
33.
34.
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)
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
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
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.
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
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
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.
Given: |
$0.2045
Can. |
= |
1.00 Francs (French) |
|
$2.1860
Can. |
= |
Ł
1.00 ( |
|
$1.3572
Can. |
= |
$
1.00 |
|
$0.1534
Can. |
= |
1.00
Peso ( |
|
$0.0109
Can. |
= |
Ą
1.00 (Japanese Yen) |
|
$0.0263
Can. |
= |
1.00
Rupee ( |
|
$1.00
|
= |
1.9325
Marks ( |
Convert:
1. $300.00
137.24 Ł.
2. $1025.00
6681.88 pesos
3. $450.00
56031
yen
4. Ł 652.23 to francs.
6972.0 francs
5. 85.2 Marks to Ł.
27.4
Ł
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
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
9. 8.774 x 103 cm3 to 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 b) 1000 g c) 25.036 A d) 5.214 x 10-62 mL
1 kg
3 infinite 5 4
e) 0.0000005 L f) 8.2000 m
1 5
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
13. Show the interval on the number line that represents the range for the above measurement after it has been round off correctly.
|
|
|
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
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,
1 pizza = 2
Wendy’s burgers 100
brussel sprouts = 3 pieces of toast
5 pieces of
toast = 1
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
Sorry, the
answer is no.
Read each scale and estimate the measurement to the correct
number of significant figures.
46. 6.62 mL
47.
48.
49. 2.97 cm
50.
52. Vernier Scale in cm. 1.63 cm
53. Micrometer Scale in mm 10.93 mm
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
.
62. Read the graduated cylinder in mL. 52.8 mL
63. Read the buret in mL. 0.60 mL
64. Read the buret in mL. 15.45 mL
65. Read the buret in mL. 38.53 mL