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Mr. Dolgos Regents Chemistry

PRACTICE PACKET Unit 1: Matter & Measurement

Name__________________________

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Vocabulary&&Define&these&in&your&own&words&so&that&you&can&easily&remember&them.&&You&can&use&the&flash&

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Physical&property____________________________________________________________________________________&&Chemical&property___________________________________________________________________________________&&STP____________________________________________________________________________________________________&&Monatomic&element__________________________________________________________________________________&&Diatomic&element____________________________________________________________________________________&&Solid___________________________________________________________________________________________________&&Liquid_________________________________________________________________________________________________&&Gas_____________________________________________________________________________________________________&&Aqueous_______________________________________________________________________________________________&&Filtration______________________________________________________________________________________________&&Distillation____________________________________________________________________________________________&&Evaporation___________________________________________________________________________________________&&Chromatography_____________________________________________________________________________________&&Conductivity__________________________________________________________________________________________&&Solubility______________________________________________________________________________________________&&Phase&change_________________________________________________________________________________________&&Element_______________________________________________________________________________________________&&Compound____________________________________________________________________________________________&&Mixture________________________________________________________________________________________________&&Homogeneous&mixture______________________________________________________________________________&&Heterogeneous&mixture______________________________________________________________________________&

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Lesson 1Classify each as one of the following: element (E), compound (C), heterogeneous mixture (Hetero), homogeneous mixture (Homo)

For the following, use the same classifications as above (some of these may have more than one answer though!)

Cannot be decomposed by chemical means Contains two or more elements Can be separated by filtrationCan be separated by distillation Cannot be separated by physical means Composed of pure matter Two liquids mixed at the molecular level Has a consistent density throughout the sample Can be separated by chromatography Properties stay the same when broken apart into its simplest form Something with varying boiling points throughout

Beaker of distilled water (H2O) Beaker of Lake Ontario water Balloon filled with air Thermometer full of mercury Tank of carbon dioxide (CO2) Glass of Kool-AidPiece of copper wire Slab of concrete Slab of iron Bowl of chicken noodle soup Salt water MilkPepperoni Pizza CarbonAirTable salt Sugar dissolved in water GraniteOxygenSand in water

Elements, Compounds, and MixturesClassify each of the pictures below by placing the correct label in the blanks below:

A= Element D= Mixture of compoundsB= Compound E= Mixture of elements and compoundsC= Mixture of elements

Each circle represents an atom and each different color represents a different kind of atom. If two atoms are touching then they are bonded together.

1) 2) 3)

4) 5) 6)

7) 8) 9)

10) 11) 12)

13) 14) 15)

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Drawing Particle Arrangements Draw a diagram of a:

pure diatomic pure diatomic mixture of mixture of mixture of element compound two elements an element & two diatomic

a compound elements & a compound

1.) In terms of composition/type of atoms, what is the difference between a monatomic element, a diatomic element, and a diatomic compound?

2.) Use the following key for parts a-c. = element X = element Z

a.) 8 atoms of element X in gaseous form b.) 4 molecules of compound X2Z in liquid form

c.) Homogeneous mixture of element Z with element X (10 atoms of each element).

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(1) aluminum (2) octane (3) silicon (4) xenon

20. Which substance can be decomposed by chemical means?(1) ammonia (2) oxygen (3) phosphorus (4) silicon

21. Which substance can not be broken down by a chemical reaction?(1) ammonia (2) argon (3) methane (4) water

22. Two substances, A and Z, are to be identified. Substance A can not be broken down by a chemical change.Substance Z can be broken down by a chemical change. What can be concluded about these substances?

(1) Both substances are elements. (2) Both substances are compounds. (3) Substance A is an element and substance Z is a compound. (4) Substance A is a compound and substance Z is an element.

23. Which terms are used to identify puresubstances?(1) an element and a mixture (2) an element and a compound (3) a solution and a mixture (4) a solution and a compound

24. Two different samples decompose when heated. Only one of the samples is soluble in water. Based on thisinformation, these two samples are

(1) both the same element (2) two different elements (3) both the same compound (4) two different compounds

25. Tetrachloromethane, CCl4, is classified as a(1) compound because the atoms of the elements are combined in a fixed proportion (2) compound because the atoms of the elements are combined in a proportion that varies (3) mixture because the atoms of the elements are combined in a fixed proportion (4) mixture because the atoms of the elements are combined in a proportion  that  varies

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Physical or Chemical Change? – Identify whether each of the followingchanges is a physical change or a chemical change. Write a “P” on the line for a physical change and a “C” for a chemical change.

1) _____ water boiling

2) _____ iron rusting

3) _____ butter melting

4) _____ alcohol evaporating

5) _____ wood rotting

6) _____ leaves changing color

7) _____ glass breaking

8) _____ mowing the lawn

9) _____ magnetizing a nail

10) _____ baking a cake

11) A piece of wood burns to form ash _______

12) Water turns into steam _______

13) A piece of cork is cut in half ______

14) A bicycle chain rusts _______

15) Food is digested in the stomach ________

16) Water is absorbed by a paper towel ________

17) Hydrochloric acid reacts with zinc _______

18) A piece of an apple rots on the ground _______

19) A tire is inflated with air ______

20)A plant turns sunlight, CO2, and water into sugar and oxygen ______

21) Sugar dissolves in water _______

22) Eggs turn into an omelet ______

23) Milk sours _____

24) A popsicle melts ______

25) Turning brownie mix into brownies ______

Classification of Matter - Fill in the Blanks

Word Bank: Chemical changes Chemical property Compound Element Heterogeneous matter Homogeneous matter

Matter Mixture Physical changes Physical property Property Substance

___________________ is anything that has mass and volume. Matter that has uniform characteristics throughout if called ______________________. Matter that has parts with different characteristics is called ______________________. A characteristic by which a variety of matter is recognized is called a(n) __________________________. A characteristic that can be observed without producing new kinds of matter is called a(n) __________________________. A characteristic that depends on how a kind of matter changes its composition (or fails to change its composition) during interactions with other kinds of matter is called a(n) ____________________________. ________________________ alter the identity of a substance, whereas __________________________ do not.

Matter can also be classified according to the basic types of matter it contains. A simple substance that cannot be broken down into other substances by chemical means is called a(n) ____________________. A chemical combination of simple substances is called a(n) _________________________. A physical combination of different substances that retain their individual properties is called a(n)______________________. Either an element or a compound may be referred to as a(n) __________________.

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Lessons 1 & 2

Understanding Chemical Formulas - Subscripts, Parentheses, Coefficients

BaF2

Subscripts

- the 2 in this formula is called the subscript. It refers only to the element preceding it. In this case the F (fluorine).

Al(NO3)3

Parentheses

- in some chemical formulas it is necessary to use parentheses. The subscript outside the parentheses refers to all the elements inside

the parentheses. In this example there are: one Al (aluminum), three N (nitrogen), and nine O (oxygen).

3 BaF2

Coefficients

- the 3 in this formula is called the coefficient. It refers to each element that follows. In this case there would be 3 Ba (barium) and 3

F2 (a total of 6 fluorine).

Examples - calculate the number of atoms in each of the following formulas:

1. KCl - one K (potassium) - one Cl (chlorine)

total of 2

2. HNO3 - one H (hydrogen) - one N (nitrogen) - three O (oxygen)

total of 5

3. Al(OH)3 - one Al (aluminum) - three O (oxygen) - three H (hydrogen)

total of 7

4. 4 K2SO4 - eight K (potassium) - four S (sulphur) - sixteen O (oxygen)

total of 28

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Lesson 2

Directions: Use the information on the front of this sheet to calculate the individual and total number of atoms in each of the following.

1. NaCl Na –

Cl –

Total 6. 6 H2SO4 H –

S –

O –

Total

2. Al(C2H3O2)3 Al –

C –

H –

O –

Total 7. Si(HCO3)4 Si –

H –

C –

O –

Total

3. 2 KOH K –

O –

H –

Total 8. 2 HNO3 H –

N –

O -

Total

4. KMnO4 K –

Mn –

O –

Total 9. 2 Al(CO2)3 Al –

C –

O -

Total

5. K2SO4 K –

S –

O –

Total 10. 3 B2(CO3)3 B –

C –

O –

Total

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Lesson 3

Answer the questions below by circling the number of the correct response

1. The separation technique shown in thediagram at the right is

(1) filtration

(2) distillation

(3) chromatography

(4) recrystallization

2. The separation of substances in a mixturedepends on the fact that the substances inthe mixture (1) have different properties,(2) are chemically combined, (3) have largeparticles, (4) show the Tyndall effect.

3. A mixture of sand and salt is separated using the apparatusshown at the right by pouring water through the mixture. Whatmaterial will be found in the filtrate after pouring water through themixture?

(1) sand and saltwater

(2) water only

(3) salt only

(4) saltwater only

4. The liquid portion of a mixture is recovered during distillation by(1) solar evaporation, (2) recrystallization, (3) chromatography,(4) condensation.

5. The water in a swimming pool is kept free of debris by the processof (1) simple crystallization, (2) fractional distillation, (3) filtration,(4) chlorination

6. A filter is able to separate mixtures because it is (1) porous,(2) homogeneous, (3) heterogeneous, (4) impermeable.

7. The separation of mixtures based on the different boiling points ofthe components of the mixture is called (1) chromatography,(2) distillation, (3) filtration, (4) recrystallization.

8. Which method of separation is based on the fact that differentsubstances travel along a stationary phase at different rates as asolvent moves through them? (1) simple crystallization(2) recrystallization (3) distillation (4) chromatography

For each of the following situations, write the correct number on theanswer space to indicate if the best method of separation to use is (1) CHROMATOGRAPHY; (2) DISTILLATION; (3) FILTRATION; or(4) SIMPLE CRYSTALLIZATION

9. Separating starch and water

10. Separating chlorophyll and the other pigments in a leaf

11. Separating gasoline from other liquid hydrocarbons

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Scientific Notation - Chem E Only

1. 22,300,000,000,000,000 =

2. 6,320 =

3. 0.00256 =

4. 0.000000001200 =

5. 5.62 x 106 =

6. 1 x 102 =

7. 2.3 x 10-5 =

8. 34000000 =

9. 0.0000067 =

10. 25,864 =

11. 5.7 x 108 =

12. 6.34 x 10-11

Part A: Express each of the following in standard form.

1. 5.2 x 103 5. 3.6 x 101

2. 9.65 x 10–4 6. 6.452 x 102

3. 8.5 x 10–2 7. 8.77 x 10–1

4. 2.71 x 104 8. 6.4 x 10–3

Part B: Express each of the following in scientific notation.

1. 78,000 5. 16

2. 0.00053 6. 0.0043

3. 250 7. 0.875

4. 2,687 8. 0.012654

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Lesson 4

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Lesson 5

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Metric Use Reference Tables C and D to help you answer the following questions about the metric system.

1. Give the unit used to describe the following:

a. Mass _______ d. Time: ______

b. Volume _______ e. Temperature: ______

c. Energy _______ f. Pressure: ______

2. Complete the following number line by adding the prefixes that pertain to the marked values:

3. If a substance weighs 2.00 grams and you need the mass in kilograms, will the number appear to becomesmaller or larger? Explain your answer.

4. If a liquid has a volume of 5800 mL and you need the mass in Liters, will the number appear to becomesmaller or larger? Explain your answer.

5. If a substance has a mass of 0.00235 grams and you need the mass in milligrams, will the number appearto become smaller or larger? Explain your answer.

6. Convert the following:

a. 900 km = __________ m h. 568 mm = __________ m

b. 200 kg = __________ g i. 52 mg = __________ g

c. 5.00 m = __________ km j. 0.025 J = __________ mJ

d. 7000 J = __________ kJ k. 0.859 s = __________ ms

e. 800 cm = __________ m l. 0.0256 m = __________ um

f. 20 cg = __________ g m. 0.000589g = __________ ng

g. 2.0 L = __________ cL n. 0.00005987 m= __________ pm

Lesson

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Determine!the!Number!of!Sig!Figs!in!each!measurement!

Round!each!measurement!to!3!sig!figs!

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Significant Figures Worksheet

Identify the number of significant figures:

1. 3.0800 ______

2. 0.00418 ______

3. 7.19x10-5 ______

4. 91,600 ______

5. 0.0003003 ______

6. 3.200x109 ______

7. 250 ______

8. 780,000,000 ______

9. 0.0101010 ______

10. 0.00800 ______

Round to 3 significant figures:

1. 7.8975 ______

2. 7976.896 ______

3. 80.000 ______

4. 848001 ______

5. 7.89765x10-8 ______

6. 78765.085 ______

7. 8999.99 ______

8. 1.0000 ______

9. 0.008978 ______

10. 0.000076097078 ______

Solve using the proper number of significant figures:

1. 4.86097 + 90.9048 ________

2. 3578.9 – 423.84 ________

3. 89038.9357 + 345.98 – 89.847 ________

4. 8975.8947 x 56.8 ________

5. 5.78x10-9) 7.789x104) ________

6. 9.856x108)/ 5.8x10-6) ________

7. 76.9478 + 7865.9) x 6.780 – 5.76) ________

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Significant Figures Practice

Count the number of Significant figures:

Round to three significant figures:

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(Rounding!Sig!Figs!in!Calculations!

Problem! Unrounded!answer! Rounded!answer!

1.((1.2(m(+(2.35(m(=((

(

( (

2.((2.6538(cm(x(2.1(cm(=((

(

( (

3.((5.681(dm(–(2(dm(=((

(

( (

4.((3845.2(m3(÷(25.2354(m3(=((

(

( (

5.((25(cm(+(3(cm(=((

(

( (

6.((1.2(m(x(2(m(=(

(

( (

7.((859678.2354(cm(–(

568426.1(cm(=((

(

( (

8.((5.3(m(x(5.2398(m(x(2(m(=((

(

( (

9.((45.25252(nm(+(45.8563(

nm(=(( (

10.((68.23(hm(÷(38.255(hm(

(

( (

Lesson 6

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11.((2.354(m(+(2.354(m(((+(

2.35(m(=(

(

( (

12.((0.28524(m(x(0.25124(m(

x(1.235(m(=(

(

( (

13.((100(cm(–(1.0(cm(=(

(

( (

14.((100(cm(x(1(cm(=((

(

( (

15.((0.000456(m(+(0.00524(

m(=((

(

( (

16.((1254.1(cm(÷(100(cm(=((

(

( (

17.((45.23547(g(–(20.584(g(=((

(

( (

18.((1(L(x(1.0(L(=(

(

( (

19.((0.00245(L(+(.234(L(=((

(

( (

20.((100,000(g(÷(10.0(g(=((

(

( (

(

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Decimal Present or Absent

Number of Sig Figs

1) 0.03092

2) 3092

3) 309.200

4) 392

5) 1020

6) 1200

7) 1200.

8) 1200.00

9) 0.00120

10) 18

11) 152.3

12) 4.000

13) 0.0205

14) 8.40

15) 22.200 g

16) 657 m

17) 0.000711 kg

18) 876.223 mg

19) 52.345 g

20) 0.3609 mL

21) 500000 m

22) 86000. mg

23) 8955.0 g

24) 87200 mL

25) 520 mL

26) 3.092 x 103

27) 520 mL

28) 0.001 cm

29) 0.451 Pa

30) 0.0102 g

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Lesson 7

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Density Problems: Show all work and express answer in proper number of sig figs.

1. You are given the following information: mass = 48 g, volume = 24 cm3. What is thedensity?

2. Bob, who weighs 150 pounds, found a rock. What is the density of the rock if its mass is36 g and its volume is 12 cm3?

Percent Error Practice Problems: Show all work.

1. There are 140 calories in one can of Coke. In an experiment you determine that thereare 210! You are a bit off, but what is your percent error for the experiment?

2. There are 35 mg of sodium in a can of Coke. You determine it to be 15 mg. What isyour percent error?

3. There is 3.5 grams of fat in a granola bar. You determine the fat content to be 4.0 g inthe lab. What is the percent error?

4. Working in the laboratory, a student finds the density of a piece of pure aluminum tobe 2.85 g/cm3. The accepted value for the density of aluminum is 2.699 g/cm3.

5. A student experimentally determines the specific heat of water to be 4.29 J/g x Co.He then looks up the specific heat of water on a reference table and finds that it is4.18 J/g• Co. What is his percent error?

6. A student takes an object with an accepted mass of 200.00 grams and masses it on hisown balance. He records the mass of the object as 196.5 g. What is his percent error?

Lesson 7

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Review/Study!Guide!

METRIC!

1.(Using(tables(on(page(one(of(your(reference(table(you(should(be(able(to(identify,(which(unit(is(used(to(

measure(each(quantity(and(you(should(be(able(to(convert(between(units(using(the(prefixes.(((Locate(the(

prefix(assigned(to(the(measurement(unit(that(you(are(starting(with(and(then(find(the(prefix(that(you(want(

to(convert(to.(Count(the(number(difference(between(the(factors(and(then(move(your(decimal(that(many(

places.(

( a.(Identify(the(unit(used(for(each(quantity:(

( ( (1)(mass( _________( ( (4)(temperature(( __________(

( ( (2)(volume( _________( ( (5)(length( ( __________(

( ( (3)(energy(( _________( ( (6)(time( ( __________(

( b.(Convert(the(following:(

( ( (1)((568(mL(to(L(( ___________________(

( ( (2)(0.00897(g(to(mg( ___________________(

( ( (3)(45700(mm(to(km(( ___________________(

2.(Density(is(the(measurement(of(mass(divided(by(volume.(A(substance’s(density(can(help(identify(it.(For(example,(water’s(density(is(1.00g/mL.(Substances(float(in(water(of(they(have(low(densities,(and(sink(when(

their(densities(are(greater(than(1.00(g/mL.((

( a.(Calculate(the(density(of(5.00(gram(sample(of(an(unknown(substance,(which(has(a(volume(of(((((

(((((((((((((((((((5.15mL.(

( b.(Using(table(S,(identify(the(unknown(substance(in(question((a)(above.(__________________________(

( c.(Calculate(the(mass(of(a(substance(with(a(density(of(2.50(g/mL(and(a(volume(of(23.0mL.(

( d.(Calculate(the(volume(of(a(metal(rectangle(with(a(height(of(2.0cm,(a(length(of(3.0cm,(and(a(width((

(((((((((((((((((((of(1.0cm.(

( e.(If(the(metal(in(question((d)(above(is(iron,(calculate(the(mass.((Hint:(density(is(on(table(S)(

(

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Lesson 1- 7

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METRIC

1. Using tables on page one of your reference table you should be able to identify which unit is used to measureeach quantity and you should be able to convert between units using the prefixes. Locate the prefix assigned to the measurement unit that you are starting with and then find the prefix that you want to convert to. Count the number difference between the factors and then move your decimal that many places.

a. Identify the unit used for each quantity:

(1) mass _________ (4) temperature __________

(2) volume _________ (5) length __________

(3) energy _________ (6) time __________

b. Convert the following:

(1) 568 mL to L ___________________

(2) 0.00897 g to mg ___________________

(3) 45700 mm to km ___________________

2. Density is the measurement of mass divided by volume. A substance’s density can help identify it. Forexample, water’s density is 1.00g/mL. Substances float in water of they have low densities, and sink when their densities are greater than 1.00 g/mL.

a. Calculate the density of 5.00 gram sample of an unknown substance, which has a volume of5.15mL.

b. Using table S, identify the unknown substance in question (a) above. __________________________

c. Calculate the mass of a substance with a density of 2.50 g/mL and a volume of 23.0mL.

d. Calculate the volume of a metal rectangle with a height of 2.0cm, a length of 3.0cm, and a widthof 1.0cm.

e. If the metal in question (d) above is iron, calculate the mass. (Hint: density is on table S)

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SCIENTIFIC NOTATION

3. Scientific Notation is used to represent very small or very large numbers. Convert the following to scientificnotation:

a. 0.00000345 ____________________________

b. 1098000000 ____________________________

c. 0.000345 ____________________________

d. 0.000005677 ____________________________

SIGNIFICANT FIGURES

4. All whole numbers 1-9 count. Preceding zeros never count, trapped zeros always count, and trailing zeroscount IF THERES A DECIMAL before the zero. Count the number of significant figures:

5678 0.09809 0.00345 0.0712

0.0987 10000 10200 102.0986

5. When rounding, your answer can only be as precise as your least precise measurement. When adding orsubtracting numbers, round your answer to the lowest decimal place given. When multiplying or dividing, round your answer to the least number of significant figures. Calculate and round to the correct number of significant figures:

a. 4.567 + 1.2 = _____________ d. 67065/87.2 = ________________

b. 678.345-234.98 = ______________ e. (54.0-32.34)/1.202 = ________________

c. 45 x789 = _____________ f. 3.108*(98.70-8.20) = __________________

ELEMENTS, COMPOUNDS, AND MIXTURES

6. Matter is anything that has a mass and takes up space. An element is the simplest form of matter, whichcannot be broken down any further. Elements are listed on Table S and the periodic table. Their symbols start with an uppercase letter.

a. Which of the following is not matter? _____________________

Magnesium Calcium Carbonate Salt water Heat

b. Which of the above is an element? _____________________

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7. Compounds are composed of two or more elements. They can only be decomposed chemically. Elementsand compounds are also known as substances.

a. Which of the choices in number one was a compound? ________________________

b. How can compound be broken down? __________________________________________________

c. Which of the choices in question one are substances? ______________________________________

8. Mixtures are physical combinations of two or more substances (elements and/or compounds). Mixtures canbe homogeneous (completely mixed, cannot see the parts) or heterogeneous (unevenly mixed, can see the parts). Mixtures can be separated by physical means. Label each as homogeneous or heterogeneous:

Sand: ____________________ Brass: ______________________________

Milk: ____________________ Oil and water: ________________________

9. Compounds must be separated chemically but mixtures can be separated easily using physical methods.

a. Match each method with its name.

Distillation Separated by differences in particle size Filtration To pour off the top layer of an uneven mixture Decant Separated by differences in boiling point. Chromatography Just a test for purity

b. Which of the above processes only work if the mixture is heterogeneous? _____________________

10. Mixtures are composed of solutes that dissolve and solvents that do the dissolving. The solute should be thesmaller quantity.

a. In iced tea, what is the solute? ___________________ solvent? ________________________

b. In air, name a solute: _________________

c. Do all solvents have to be water? Explain. _______________________________________________

SOLIDS, LIQUIDS, AND GASES

11. A solid has a definite shape and volume. Solids are arranged in a geometric pattern. Liquids have a definitevolume but take the shape of the container they are in. Gases have an indefinite shape and volume; they take the shape and volume of the container. Gases are easily compressed.

a. Draw particle diagrams for a solid, liquid, and a gas using at least 5 particles:

b. Which has a definite shape?

32

HCl(g) H2O(l) Cu(s)

c. Which has a definite volume?LiF(g) Br2(l) Mg(s)

12. Vapors are the gas phase of substances that are normally solid or liquid at room temperature. Which can bea vapor?

Carbon dioxide ______ Water _____ Oxygen _____

13. Phase changes occur when heat is given to or taken from a sample. For each of the following, give thephases involved and if it is endothermic or exothermic.

Evaporation ___________________________ __________________________

Melting ___________________________ __________________________

Deposition ___________________________ __________________________

Boiling ___________________________ __________________________

Condensation ___________________________ __________________________

Sublimation ___________________________ __________________________

CHANGES IN THE LAB

14. Physical changes are changes where the substance retains its properties. Chemical changes will makesubstances change into new substances and change properties.

a. Label the following as physical (P) or chemical (C) properties:

Texture ____ flammability ____ boiling point: ____

Odor ____ color ____ chemical composition: ____

b. Label the following as physical (P) or chemical (C) changes:

Corrosion: ____ melting: ____ mixing: ____

Freezing: ____ cutting: ____ decaying: ____

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!

SCIENTIFIC!NOTATION!

3.(Scientific(Notation(is(used(to(represent(very(small(or(very(large(numbers.(Convert(the(following(to(

scientific(notation:(

( a.((0.00000345( ____________________________(

( b.(1098000000( ____________________________(

( c.(0.000345( ( ____________________________(

( d.(0.000005677( ____________________________(

SIGNIFICANT!FIGURES!

4.(All(whole(numbers(1e9(count.(Preceding(zeros(never(count,(trapped(zeros(always(count,(and(trailing(

zeros(count(IF(THERES(A(DECIMAL(before(the(zero.(Count(the(number(of(significant(figures:(

( 5678( ( ( 0.09809( ( 0.00345( ( 0.0712(

( 0.0987(( ( 10000(( ( 10200(( ( 102.0986(

5.(When(rounding,(your(answer(can(only(be(as(precise(as(your(least(precise(measurement.(When(adding(

or(subtracting(numbers,(round(your(answer(to(the(lowest(decimal(place(given.(When(multiplying(or(

dividing,(round(your(answer(to(the(least(number(of(significant(figures.(Calculate(and(round(to(the(correct(

number(of(significant(figures:(

( a.((4.567(+(1.2(=(( _____________( ( d.(67065/87.2(=(( ________________(

( b.(678.345e234.98(=(______________( ( e.((54.0e32.34)/1.202(=(________________(

( c.(45(x789(=( ( (_____________( ( f.(3.108*(98.70e8.20)(=(__________________(

!

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(