Unit 1

Unit 1 Safety, Review and Measurement

Lesson Day Date Topic Homework

1. Safety Assignment # 1

2. Review Assignment # 2

3. Balancing Equations Assignment # 3

4. Formulas Equations Assignment # 4

5. Measurement and Uncertainty

6. Uncertainty Lab Day 1

7. Uncertainty Lab Day 2

8. Significant Figures Assignment # 5

9. Unit Analysis 1 Assignment # 6

10. Unit Analysis 2 Assignment # 7

11. Review Assignment # 8

12. Practice Test Assignment # 9

Assignment # 1 Safety and Review

Complete the safety map for the room by indicating the location of the fire extinguishers, doors, eyewash, , fire blanket, , eye-goggles, broken glass container, soap dispensers, paper towel dispensers, and soap sprayers. This is like a treasure hunt. Get up and look for everything.

Room

#

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.

*For those that start with H (covalent compounds) the two largest formulas are solids, the next three larger formulas are liquids, and the three smallest are gases.

The last one, which you can drink, is a liquid.

	Li	Mg	Al	NH₄	Na	Ba	K	Ca	*H
OH	1	2	3	4	5	6	7	8	9
SO₄	10	11	12	13	14	15	16	17	18
Br	19	20	21	22	23	24	25	26	27
F	28	29	30	31	32	33	34	35	36
NO₃	37	38	39	40	41	42	43	44	45
PO₄	46	47	48	49	50	51	52	53	54
S	55	56	57	58	59	60	61	62	63
C₂O₄	64	65	66	67	68	69	70	71	72
Cr₂O₇	73	74	75	76	77	78	79	80	81

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Chemical Equations from Word Equations

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

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.

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

Assignment # 2 Physical Chemical Changes Balancing Equations

Classify as a physical or chemical change.

1. Spoiling of food

2. Vaporization of ice

3. Stretching of a rubber band

4. Dynamite explosion

5. Shattering of glass

6. Decaying of dead bodies

7. Extraction of iron from form (Fe₂O₃)

8. Spontaneous combustion of oily rags

9. Grinding of wheat

10. Melting snow

11. 2 H₂O →2 H₂ + O₂ + Energy

12. E + NaCl_(s) → NaCl_(aq)

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

mp bp physical state

a) Mercury

b) Bromine

c) Chlorine

Classify as a physical or chemical properties.

14. Sugar chars when heated

15. Yellow color of sulphur

16. Tarnishing ability of sulphur

17. Flexibility of a spring

18. Thermal conductivity of iron

19. Hardness of a diamond

20. Stability of nitrogen

21. Describe 11 and 12 as exothermic or endothermic

Write Ionic Formulas

22. Aluminum oxide

23. Aluminum chloride

24. Ammonium acetate

25. Barium phosphate

26. Calcium hydroxide

27. Sodium hydroxide

28. Strontium phosphate

29. Iron II phosphate

30. Cobalt III sulphate pentahydrate

31. Copper II nitrate hexahydrate

Write a balanced equation and include all phase symbols

32. Sodium chloride dissolving in water (endothermic).

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

34. List three chemical and physical properties.

Assignment # 2 Classifying Matter And Balancing Equations

1. Label each as chemical or physical.

a) Ice cubes turn to water

b) Steam forms water droplets in a mirror

c) Milk is made into ice milk

d) Ice cubes shrink in a freezer

e) Perspiration “dries”

f) Bromine is liquefied from solid bromine

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

a) Rain

b) Snow

c) Frost

d) Steam

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.

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

a) Photosynthesis (CO₂+H₂O→Sugar+oxygen)

b) Antifreeze boils out of a radiator

c) A firefly emits light

d) A nail is magnetized

e) A nail rusts

f) Leaves turn color in autumn

g) Food spoils

h) Dynamite explodes

I) Grinding of wheat into flour

j) Shattering of glass

k) Extraction of iron from iron ore (Fe₂O₃)

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

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

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

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

a) Methane (CH₄)

b) Pizza

c) Milk shake

d) Zinc

e) Laughing gas

f) Clean air

g) Chocolate chip cookie

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.

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.

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

Balancing Equations

1. ___KNO₃ → ___KNO₂ + ___O₂

2. ___CaC₂ + ___O₂ → ___Ca + ___CO₂

3. ___C₅H₁₂ + ___O₂ → ____CO₂ + ___H₂O

4. ___K₂SO₄+ ___BaCl₂ → ____KCl + ___BaSO₄

5. ___KOH + ___H₂SO₄ → ____K₂SO₄ + ___H₂O

6. ___Ca(OH)₂ + ___NH₄Cl → ____ NH₄OH + ___CaCl₂

7. ___C + ___SO₂ → ___CS₂ + ___CO

8. ___Mg₃N₂+ ___ H₂O → ____ Mg(OH)₂ + ___NH₃

9. ___V₂O₅ + ___Ca → ___CaO + ___V

10. ___Na₂O₂+ ___H₂O → ____NaOH + ___O₂

11. ___Fe₃O₄ + ___H₂ → ____Fe + ___H₂O

12. ___Cu + ___H₂SO₄ → ____CuSO₄ + ___H₂O + ___SO₂

13. ___Al + ___H₂SO₄ → ____ H₂ + ___ Al₂(SO₄)₃

14. ___Si₄H₁₀ + ___O₂ → ___SiO₂ + ___H₂O

15. ___NH₃ + ___O₂ → ___N₂H₄ + ___H₂O

16. ___C₁₅H₃₀ + ___O₂ → ___CO₂ + ___H₂O

17. ___BN + ___F₂ → ___BF₃+ ___N₂

18. ___CaSO₄ ^.2 H₂O + ___SO₃ → ___CaSO₄ + ___H₂SO₄

19. ___C₁₂H₂₆ + ___O₂ → ___CO₂ + ___H₂O

20. ___C₇H₆O₃ + ___O₂ → ___CO₂ + ___H₂O

21. ___Na + ___ZnI₂→ ___NaI + ___NaZn₄

22. ___LiAlH₄ + ___BF₃ → ___LiF + ___AlF₃ + ___B₂H₆

23. ___HBrO₃ + ___HBr → ___H₂O + ____Br₂

24. ___O₂ + ___Al_l4C₃ + ___H₂O → ___Al(OH)₃ + ___CH₄

25. ___Ca(NO₃)₂ ^.3H₂O + ___LaC₂ → Ca(NO₃)₂ + ___La(OH)₂ + ___C₂H₂

26. ___CH₃NO₂ + ___Cl₂ → ___CCl₃NO₂ + ___HCl

27. ___Ca₃(PO₄)₂ + ___SiO₂ + ___C → ___CaSiO₃ + ___CO + ___P

28. ___Al₂C₆ + ___H₂O → ___Al(OH)₃ + ___C₂H₂

29. ___NaF + ___CaO + ___H₂O → ___CaF₂ + ___NaOH

30. ___LiH + ___AlCl₃ → ___LiAlH₄ + ___LiCl

31. ___CaF₂ + ___H₂SO₄ + ___SiO₂ → ___CaSO₄ + ___SiF₄ + ___H₂O

32. ___CaSi₂ + ___SbCl₃ → ___Si + ___Sb + ___CaCl₂

33. ___TiO₂ + ___B₄C + ___C → ___TiB₂ + ___CO

34. ___NH₃ + ___O₂ → ___NO + ___H₂O

35. ___SiF₄ + ___NaOH → ___Na₄SiO₄ + ___NaF + ___H₂O

36. ___NH₄Cl + ___CaO → ___NH₃ + ___CaCl₂ + ___H₂O

37. ___NaPb + ___C₂H₅Cl → ___Pb(C₂H₅)₄ + ___Pb + ___NaCl

38. ___Be₂C + ___H₂O → ___Be(OH)₂ + ___CH₄

39. ___NpF₃ + ___O₂ + ___HF → ___NpF₄ + ___H₂O

40. ___NO₂ + ___H₂O → ___HNO₃ + ___NO

Some Tough Ones

___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 # 3 Balancing Equations

1. ___Al + ___HCl → ___AlCl₃ + ___H₂

2. ___Zn + ___KOH → ___K₂ZnO₂ + ___H₂

3. ___B₂O₃ + ___Mg → ___MgO + ___B

4. ___C₆H₁₁OH + ___O₂ → ___H₂O + ___CO₂

5. ___C₁₂H₂₆ + ___O₂ → ___HOH + ___CO₂

6. ___Na + ___H₂O → ___NaOH + ___H₂

7. ___PbS + ___O₂ → ___PbO + ___SO₂

8. ___SiCl₄ + ___Na → ___Si + ___NaCl

9. ___Mg + ___CO₂ → ___MgO + ___C

10. ___Al + ___H₂SO₄ → ___Al₂(SO₄)₃ + ___H₂

_{Write Formulas for each}

_{11. Zinc phosphate}

_{12. Ammonium carbonate}

_{13. Iron III oxalate}

_{14. Copper II tripolyphosphate
pentahydrate}

_{15. Cobalt II borate}

_{16. Triphosphorus tetroxide}

_{17. Dicarbon hexachloride}

_{18. Trisilicon octafluoride}

_{19. Sodium tetraborate}

_{20. Aluminum dichromate}

_{21. Calcium oxide}

_{22. Silver thiosulphate}

_{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.

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

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

26. Write an equation for the combustion of sucrose.

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

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

Worksheet # 4 Balancing Equations Naming Formulas

1. ___Sb + ___Cl₂ → ___SbCl₅

2. ___FeCl₂+ ___Cl₂ → ___FeCl₃

3. ___P + ___I₂ → ___PI₃

4. ___Na₂S + ___HCl → ___NaCl + ___H₂S

5. ___NaOH + ___FeCl₃ → ___NaCl + ___Fe(OH)₃

6. ___KOH + ___H₃PO₄ → ___K₃PO₄ + ___H₂O

7. ___NaOH + ___CuSO₄ → ___Na₂SO_{4 +}__Cu(OH)₂

8. ___HNO₃ + ___Ca(OH)₂ → ___H₂O + __Ca(NO₃)₂

9. ___NH₃ + ___CuO → ___H₂O + ___Cu + ___N₂

10. ___N₂ + ___C +___Na₂CO₃ → ___NaCN + ___CO

11. ___NH₃ + ___O → ___NO + ___H₂O

12. ___NH₃ + ___O₂ → ___NO₂ + ___H₂O

13. ___NH₃ + ___O₂ → ___N₂O₅ + ___H₂O

14. ___P + ___N₂O → ___P₂O₅ + ___N₂

15. ___Al + ___HCl → ___AlCl₃ + ___H₂

16. ___Zn + ___KOH → ___K₂ZnO₂ + ___H₂

17. ___B₂O₃ + ___Mg → ___MgO + ___B

18. ___CH₃OH + ___O₂ → ___H₂O + ___CO₂

19. ___C₆H₁₂O₆ → ___C₂H₅OH + ___CO₂

20. ___Na + ___H₂O → ___NaOH + ___H₂

21. ___PbS + ___O₂ → ___PbO + ___SO₂

22. ___SiCl₄ + ___Na → ___Si + ___NaCl

23. ___Mg + ___CO₂ → ___MgO + ___C

24. ___Al + ___H₂SO₄ → ___Al₂(SO₄)₃ + ___H₂

Write balanced chemical formulas for each ionic compound.

25. Calcium hydroxide

26. Aluminum sulphate

27. Iron III oxide

28. Zinc acetate

29. Barium carbonate

30. Sodium phosphate

31. Cobalt II nitride

32. Gallium sulphate

33. Aluminum fluoride

34. Ammonium sulphate

35. Aluminum acetate

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

36. carbon monoxide

37. dinitrogen tetraiodide

38. triphosphorus hexafluoride

39. dinitrogen dioxide

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.

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

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

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

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

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

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

You are good if you can do these.

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

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

Worksheet # 5 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

25.64V

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

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?

25.63 101 0.0075

0.0002 1.00 2.005

10.031 1.0002 10005

0.00521 2.51 x 10⁴ 3 x 10^-7

2 x 10⁵ 2.00 x 10³ 250.

5. Round off to three significant figures.

0.05211 0.0087251

85.337 2.6177 x 10^-5

2.5175 x 10^-1825.731 x 10⁵

Round off each measured number to three significant figures.

6. 0.002567

7. 94549

8. 15.00

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

a) 35.234 b) 2.34521

c) 0.035219 d) 2533521

e) 6255520000

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

a) 305 b) 25.25

c) 3.00 d) 0.001

e) 3.0050 f) 6.25 x 10²³

g) 7.00 x 10^-2 h) 1001

11. Add or subtract the measured quantities.

25.31 22.0 22.7 35.271

+ 6.4 + 0.04 + 0.77 + 0.2

22.71 25.217 2.51639 8.0558

- 0.299 + 0.017 - 1.2358 + 0.3259297

25.634 + 2.365 - 0.25498 + 0.225 =

12. 15.239 + 5.36

13. 2.6679 - 1.23

14. 2.059378 x 10²⁴ + 5.3 x 10²²

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

16. 2.3 x 10 ¹⁶ + 8.224 x 10¹⁹

17. 5.6 x 10 ^–8 + 9.5563 x 10^-6

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

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

Assignment # 6

1. 25 x 3

2. 3.35 x 0.26

3. 799 x 877

4. (6.2 x 10³)( 3.55 x 10¹²)

5. (6.3 x 10⁷)(2.51 x 10^-7)

(3.214 x 10^-5)

6. (7.52 x 10¹⁶)(3.1 x 10¹²)

7. 3.5 x 10²÷ 3.1 x 10³

(2.5 x 10^-7)

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)

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)

10. 156 x 256 x 21 x 0.0005687 0.02569 x 13.235 x 2654

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)

12. 25.7 x 0.21

13. 35 x 105

14. 51.71 x 22.3

15. 22 x 305

16. Write three examples of exact numbers.

17. Write three examples of approximate numbers.

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

22. 26.215 23. 65.222 24. 22 - 0.01

- 0.3 + 1.03

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

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

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

58.56 g

58.59 g

58.51 g

58.61 g

58.57 g

58.56 g

Answer

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

123.2

124.5

124.0

124.3

Answer

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

a) 0.00200 L b) 5.000 g

c) 1.00003 A d) 1000.000 Mm

e) 2.5 ^x10⁷⁶f) 78.89 m

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

a) 18. + 0.21

b) 62.1 ^x 3021.56

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

d) (9.442 ^x10^-3)(3.21 ^x10⁸)

e) 231.4 - 8.2295

f) (8.995 ^x10⁶) + (3.55 ^x10⁷)

g) 12.0355 + 1.024

h) (4.56 ^x10^-8)(2.5 ^x10³⁵)

i) (9.24 ^x10¹⁰)(5.233 ^x10⁴)

33. State the difference between accuracy and precision.

Worksheet # 7 Unit Analysis 1

1. 527 g to mg

2. 1.05 x 10⁶ um to m

3. 2.148 ML to mL

4. 0.0235 mg to kg

5. 8.32 x 10^-4 mL to ML

6. 772.5 us to ms

7. 3.06500 cg to Kg

8. 9.450 Mm to mm

9. 5.64 x 10³ mm² to cm²

Non-metric/Metric Conversions

Given that: 2.210 lb = 1.00 kg 4.54 L = 1.00 Gal

1.000 atm = 101.3 kPa 1.61 km = 1.00 mile

14 lb = 1 stone 2000 lb = 1 ton

16 oz = 1 lb

10. 170. lb to kg

11. 648 kPa to atm

12. 256 oz to tons

13. 0.025 ton to mg

14. 0.236 Gal to mL

15. 5.8 x 10⁶ mL to Gal

16. 5.66 x 10⁶ mg to stones

17. 15 miles to mm

18. 5.63 x 10⁹ µm to miles

Worksheet # 8 Unit Analysis 2

1. 605 µm to mm

2. 6.5 x 10^-6 Mm to m

3. 20.0 Km to cm.

4. 8.774 x 10¹⁵ µm to Mm.

5. 25 cL to ML

6. 648 KPa to mPa

7. 2.665 Mg to µg

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)

8. 152 mL to gal

9. 8.6 stone to oz

10. 4.3 m to miles

12. 15.2 mi/gal to L/km

13. 2.3 gal to mL

14. 45.2 oz to stones

15. 46.3 miles to m

16. 36 L/km to mi/gal

17. 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.

18. 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.

19. 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

6 yams = 10 lbs of figs

Worksheet # 9 Unit Analysis and Measurement 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)

Assume all of the conversions have the number of significant figures indicated.

Convert:

1. $300.00 Can. to £.

2. $1025.00 Can. to pesos.

3. $450.00 U.S. to yen.

4. £ 652.23 to francs.

5. 85.2 Marks to £.

6. 3842.35 Yen to Rupees.

7. 9668.75 Francs to 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.

2. 10. CDs to tickets.

3. 100. Buttons converted to CDs.

4. 1 Back Stage Pass converted to T Shirts.

5. 280. Posters to Back Stage Passes.

6. 6 Back Stage Passes to buttons.

7. 6.372 hL to mL 6.372 x 10⁵ mL

8. 4.9 x 10¹⁵ µg to Mg 4.9 x 10³ Mg

9. 8.774 x 10³ cm³ to m³ 0.008774 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

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

a) 25.0 g 3 b) 1000 g = 1 kg infinite

c) 25.036 A 5 d) 5.214 x 10^-62 mL 4

e) 0.0000005 L 1f) 8.2000 m 5

Determine the average and uncertainty given the following measurements from a

12. Centigram balance

82.62 g

82.54 g

82.48 g

82.72 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.

Write chemical formulas for each ionic or molecular compound.

14. Iron III oxide

15. Triphosphorous hexoxide

16. Aluminum hydroxide

17. Nickel II phosphate octahydrate

Name each chemical formula

11. K₃PO₄

12. Mn₃P₂

13. Ga₂(SO₃)₂^. 6H₂O

14. P₄O₁₀

Worksheet # 10 Unit 1 Practice Test

Balance each equation.

1. ___Sb + ___Cl₂ ® ___SbCl₅

2.___NH₃ + ___O₂ ® ___N₂O₅ + ___H₂O

3. ___C₁₂H₂₆ + ___O₂ ® ___CO₂ + ___H₂O

4. ___Al + ____H₂SO₄ ® ____H₂ + ____Al₂(SO₄)₃

(The next one is the tough one!!)

5. ___Cu + ____HNO₃ ® ____Cu(NO₃)₂ + ____NO +____H₂O

6. Barium phosphate plus sodium sulphate (both in water) yields solid barium sulphate and aqueous sodium phosphate. Write a balanced equation with phase symbols

Write chemical formulas for each ionic or molecular compound.

7. Mercury II sulfide

8. Diphosphorous pentoxide

9. Barium hydroxide

10. Copper II sulphate hexahydrate

Name each chemical formula

11. Na₃PO₄

12. Co₃P₂

13. Al₂(CO₃)₂^. 6H₂O

14. Si₂I₆

15. Determine the average and uncertainty for the data:

25.56g

25.54g

25.52g

25.53g

25.55g

Answer

16. Determine the average and uncertainty for the data:

5.216 ^oC

5.218 ^oC

5.213 ^oC

5.214 ^oC

5.416 ^oC

Answer

Round off each measured number to three significant figures.

17. 0.002567

18. 94549

19. 15.00

Add or subtract the measured quantities.

20. 15.239 + 5.36

21. 2.6679 - 1.238

22 12.65449 + 0.2493

23. 8.57 x 10⁷ + 5.37894 x 10⁹

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

24. 156 x 256 x 21 x 0.0005687

.02569 x 13.235 x 2654 Answer

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

Complete the relationships:

26. Mg = g 27. km = m

28. L = mL 29. g = ng

30. µs = s 31. cg = g

32. pg = g 33. s = Ts

Use unit analysis to perform the following conversions:

34. 8.13 kg to cg.

35. 2.3 x 10¹² µm to Mm.

36. 1.52 x 10⁴ Mm to mm.

37. 2.13 Mg to cg.

38. 8.88 x 10¹² mm to Mm.

39. 8.52 x 10^-8 Mm to 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

41. 3.8 stone to oz

42. 25.6 m to miles

43. 26 mi/gal to L/km

44. 14.5 L/km to mi/gal

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?