name_____________________________ - north · web viewif 36 grams of water are produced and 4...

Name_____________________________

Honors Chemistry

FINAL EXAM REVIEWFINAL EXAM DATES ndash THURSDAY JUNE 5 2014 and TUESDAY JUNE 10 2014 The final exam is worth 100 points and is multiple choice format Part 1 will assess Chapters 1 ndash 6

Part 2 will assess Chapters 7 - 13

FINAL REVIEW PRACTICEDIRECTIONS Complete on a separate sheet of paper Show all work

CHAPTER 1 AND 2 ndash INTRODUCTION TO CHEMISTRY AND MEASUREMENT1 Is the following set of data accurate precise both or neither if the actual value is 234 mL

204 mL 203 mL 201 mL 205 mL

The measurements are precise but not accurate

2 Indicate the number of significant figures in the following

a 1040 3 b 600 1 c 1240 4 d 000230 3 e 082 2

3 Solve each expression using correct number of significant figures and units

a 244g + 110g 130 g b 14530 mL ndash 128 mL 1325 mL

c 98 g 123 L 80 gL d 14500 cm x 255 cm x 15 cm 55 cm3

4 Solve the following using dimensional analysis (factor label method)

a Convert 235 yd3 to ft3 635 ft3

b A pound of coffee beans yields 50 cups (this number is obtained by counting) of coffee

How many milliliters of coffee can be obtained from 100 g of coffee beans (1 cup = 240mL)

264 mLg

c Convert 2350 ms2 to kmmin2 8460 kmmin2

5 Convert the following to the indicated temperatures

a -34 C to F -29 F b 213 K to C -60 C

6 Explain how a Bunsen burner works Gas and air are controlled by knobs on the burner The gas

and air mix resulting in a smokeless flame that produces very high temperatures

7 What is the most practical and accurate tool used to measure volume in a laboratory

Graduated Cylinder

8 Explain how you would set up a laboratory apparatus for

a heating a crucible of magnesium ndash ring stand with an iron ring supporting a clay triangle

b heating a beaker of copper II oxide and water ndash ring stand with an iron ring supporting a

wire gauze The beaker will be placed on the gauze and supported by a second iron ring

9 A student takes an object with an accepted mass of 20000 grams and masses it on his own

balance He records the mass of the object as 1965 g What is his percent error 175

10 What value does each of the following metric unit represent

a centi 01 or 1 x 10-2 b nano 000000001 or 1 x 10-9 c kilo 1000 or 1 x 10 3

d milli 001 or 1 x 10-3 e micro 000001 or 1 x 10-6

CHAPTER 3 ndash MATTER AND ENERGY1 Solve the following density problems using significant figures

a What is the density (gmL) of a block of metal 6cm x 10cm x 100cm that weighs 6820 dg

What would be the volume (in L) of 28 kg of the metal 245 L = 20 L

b A block of metal has a mass of 423 g It is placed in a graduated cylinder containing 560

cm3 of water If the final volume is 751 mL what is the density of the metal block 221 gmL

2 How would you separatehellip

a iron filings and pepper magnet b salt and sand dissolve the salt and filter the sand then

evaporate the water c methanol and water distillation

3 What is the specific heat of water 4184 Jg C

4 Which requires more heat to warm from 220 C to 850C if they have exactly the same mass a

sample of aluminum (c = 902 J g C) or a sample of water Explain It takes more energy to heat

one gram of water than 1 gram of aluminum because water has a higher specific heat

5 A 0234 kg sample of copper cools from 53 C to - 94 C What is the change in its energy if the

specific heat of copper is 387 Jg C - 570 J

6 Distinguish between a physical and chemical change A physical change is a change that results

in no change to the components of the substance A chemical change is a change that results in a

change to the components of the substance The identity of the substance will change due to a

physical change

7 Classify the following as either a physical or chemical change

a spoiling of milk C b softening glass to bend it into a new shape P

c burning a piece of paper C d rusting of a nail C

8 Identify the following as a pure substance heterogeneous mixture or homogeneous mixture

a copper Pure substance - element

b sweetened tea Homogeneous mixture - solution

c calcium carbonate Pure substance - compound

d sandy water ndash Heterogeneous mixture - suspension

9 What is the difference between an exothermic reaction and an endothermic reaction Relate each

reaction type to enthalpy Endothermic reactions absorb energy and the products have more energy

than the reactants The enthalpy change for an endothermic reaction is positive Exothermic

reactions release energy and the products will have less energy than the reactants Exothermic

reactions have a negative enthalpy change

10 Using the potential energy diagram above answer the following questions

a How much energy do the reactants have 200 kJ

b How much energy is needed to get the reaction started 250 kJ

c What type of reaction is this endothermic or exotherimic endothermic

CHAPTER 4 ndash CHEMICAL FOUNDATIONS1 What is the atomic mass of silver What is silverrsquos mass number 10787 amu 108

2 Determine the symbol for the atom ion and or isotope that fits the description below

a 16 p 18 e 16 n S-2 b 26 p 26 e 30 n Fe c 13 p 10 e 11 n Al+3

d 35 p 35 e 45 n Br

3 Determine the identity of an element with a mass number of 75 that contains 42 neutrons As

4 Determine the number of protons neutrons and electrons in the following

a Ar ndash 40 18p 22n 18 e b F-1 9p 10n 10e c 29 Al 13p 16n 13e

d Co 27p 32n 27e e 56 Fe 26p 30n 26e

26

5 Distinguish between an alpha and beta particle Alpha decay is the emission of a helium

nucleus (2 protons and 2 neutrons = alpha particle) Beta decay is the splitting of a neutron into a

proton and an electron = beta particle The proton is added to the nucleus of the atom changing the

identity of the atom

6 If 36 grams of water are produced and 4 grams of hydrogen are used in its production how many

grams of oxygen is needed What law is represented here 320 grams of O2 = Law of the

Conversation mass

7 What is the difference between the mass number for Carbon 14 and carbonrsquos average atomic

mass of 12011 amu Mass number gives the total number of protons and neutrons for one isotope

of carbon The average atomic mass is the calculated sum of all of the isotopes of carbon and their

abundance in nature

8 Calculate the atomic mass of lithium if one isotope has a mass of 60151 amu and a percent

abundance of 759 and a second isotope has a mass of 70600 amu and a percent abundance of

9241 698 amu

9 Describe the debate between Democritus and Aristotle in terms of the atom Democritus ndash small

pieces cannot be broken into smaller pieces forever ndash sooner or later a single particle so small that

cannot be broken down into anything further will remain He calls this end particle atomos He states

that all matter consists of a collection of atoms and if there was space between the atoms it contains

nothing Aristotle ndash he believes that it makes more sense to believe that everything can be broken

into smaller and smaller pieces forever He questions that if matter is composed of particles and

empty space what holds the particles together Due to Aristotlersquos fame and popularity he wins the

debate

10 List the five postulates to Daltonrsquos theory Explain two reasons why it is no longer accepted

1 All matter consists of tiny particles

2 Atoms of an element are unchangeable and indestructible

3 Elements are characterized by the mass of their elements

ndash All atoms of the same element have the same mass

ndash Atoms of different elements have different masses

4 When elements react their atoms combine in simple whole number ratios

ndash Different atoms combine in simple whole number ratios to form compounds

5 When elements react their atoms sometimes combine in more than one simple whole number

ratio

11 Compare and contrast Rutherford and Thomsonrsquos experiments and atomic models

Thomson ndash experiments using cathode ray tubes and discovers the electron His model is referred to

as the Plum Pudding Model where atoms are sphere shaped and composed of a space of positive

charge The negative electrons are found within this area of positive charge

Rutherford ndash experiments using sheets of gold foil and alpha particles and discovers that the alpha

particles are deflected back differently than what the plum pudding model would predict His model is

referred to as the nuclear model where the electrons are found in the empty space and the positive

charge or protons are found in the center of the atom in what he refers to as the nucleus

12 What significance does each subatomic particle have in regards to an elementrsquos properties

Protons ndash used to identify an individual atom

Neutrons ndash effect the average atomic mass of an atom

Electrons ndash determine an atomrsquos chemical behavior

13 Radioactive strontium (Sr - 90) has a half life of 29 years If you had a 100 gram sample how

many years will it take you to get 25 grams of sample

100 grams 50 grams = 29 years 50 grams 25 grams = 29 years TOTAL = 58 years

14 What element undergoes alpha decay to form lead-208 Explain

When a radioactive element undergoes alpha decay it emits an alpha particle that is 2 protons and 2

neutrons (Helium nucleus) The element is Po ndash 212

CHAPTER 5 ndash MODERN ATOMIC THEORYQUANTUM MECHANICS1 What is the wavelength (in m) of a photon of light containing 319 x 10-13 J of energy

623 x 10 -13 m

2 How much energy in Joules will a photon of light with a wavelength of 3450 nm possess

5762 x 10-19 J

3 What is the maximum number of electrons that can occupy the following

a 3d 10 b 3rd energy level 18 c 4s 2 d one orbital 2

e 4th energy level 32

4 Draw the orbital diagrams for the following elements

a argon b copper

c nitrogen

5 Write the electron configuration for the following elementsions

a calcium 1s22s22p63s23p64s2 b arsenic 1s22s22p63s23p64s23d104p3

c molybdenum 1s22s22p63s23p64s23d104p6 5s14d5

d magnesium ion 1s22s22p6 e sulfur ion 1s22s22p63s23p6

6 Write the noble gas configuration for the following elements

a Tin [Kr] 5s24d105p2 b Gold [Xe] 6s1 4f14 5d10 c Chromium [Ar] 4s13d5

7 Answer the following questions about the electron configuration of aluminum

a What does the 3 in 3s2 mean Third energy level

b What does the 2 in 3s2 mean Two electrons in sublevel

c How many valence electrons does this atom have 3

d How many electrons will an atom of aluminum (lose or gain) to form an ion Lose 3

e What orbitals will aluminum lose its electrons from 3s and 3p

8 What is needed for an electron to move from one energy level to a higher energy level

A quanta of energy must be absorbed

9 What can be determined from an atomrsquos atomic emission spectra The

wavelengthfrequencyenergy of light emitted by an atom when electrons return to ground state

10 What happens when an electron falls back to its ground state It emits light of a specific

wavelengthfrequencyenergy

CHAPTER 6 ndash THE PERIODIC TABLE1 Write the symbol of the element that fits each description

a alkali metal in period 3 Sodium b alkaline earth metal with 5 energy levels

Strontium

c the only metalloid chalcogen (oxygen group) Tellurium (Polonium is acceptable too)

d halogen with four energy levels Bromine

2 How many valence electrons does each of the following possess What ion does each form

a calcium 2 Ca+2 b silver 1 Ag+1 c phosphorus 5 P-3 d lead 24 Pb+2Pb+4 e

carbon 4 C-4

3 Which is smaller

a Ca or Ca+2 b P or O c N or F d Sulfur ion or Aluminum ion

4 Does each of the following trends increase or decrease down a family or across (left to right) a

period

Down a Family Across a Period

Electronegativity Decreases Increases

Ionization Energy Decreases increases

Atomic Radius Increases decreases

5 Define electron affinity Which elements have a negative value for electron affinity Why

Electron affinity is the energy change that occurs when a neutral atom acquires an electron The

more negative the value the greater the amount of energy that is released Elements that readily

gain electrons like the halogens will have the most negative values because little energy is required to

force an atom to acquire the electron

Metals such as the alkaline earth metals will have positive values Metals wish to lose electrons not

gain them In order to add electrons to a metal energy must be added forcing the addition of the

electron

6 Draw the Lewis dot diagrams for the following elements

a b c

7 Why are the alkali metals one of the most reactive families of elements They have low ionization

energy

8 Which groups make up the representative or main group elements 1 2 13 14 15 16 17 and

18

9 Give three physical properties that differ between metals and nonmetals Metals will lose

electrons are good conductors of electricity and heat have luster exist as solids high boiling points

and melting points Nonmetals will gain electrons are poor conductors of electricity and heat lack

luster are normally found as gases or solid are brittle low boiling points and melting points

10 What is a metalloid List each of them Elements that behave as both a metal and a nonmetal

Boron Silicon Germanium Arsenic AntimonyTellurium Polonium and Astatine

CHAPTER 7 ndash CHEMICAL BONDING1 What is the difference between an ionic and a covalent bond

An ionic bond is a bond commonly formed between a metal and a nonmetal The electronegativity

difference is normally greater than 18 causing a transfer of electrons from one atom to the other A

covalent bond is a bond commonly formed between two nonmetals The electronegativity difference

is less than 18 causing the electrons to be shared (and not transferred) from one atom to the other

2 Would the following pairs most likely form an ionic or molecular compound

a Mg and Cl - ionic b I and F - molecular c P and Cl - molecular

b d Sn and O - ionic e Ag and S - ionic

3 Draw a Lewis dot diagram for each of the following

a b c d e

4 Using electronegativity values write the ranges for a polar covalent non polar covalent and ionic

bonds What is the significance of these electronegativity differences

18 and greater ndash ionic 4 ndash 17 polar covalent 0 - 3 nonpolar covalent ndash the electronegativity

difference determines whether or not the electrons are able to be transferred or shared

5 Describe the three types of intermolecular forces Give one example of each

Intermolecular forces are weak attractive forces between MOLECULES in a molecular compound

Dispersion force ndash weak force between nonpolar molecules Any diatomic molecule like

F2

Dipole ndash dipole force ndash force between oppositely charged ends of two polar molecules

The more polar the molecule the stronger the force SCl2

Hydrogen bond ndash especially strong attraction between the hydrogen end and a fluorine

nitrogen or oxygen atom on the other dipole Water

6 Draw the Lewis structures for each of the following compounds

i Identify the total number of valence electrons for each

ii What is the molecular shape (linear bent trigonal pyramidal trigonal planar

tetrahedral)

iii What is the bond angle for each shape

iv Polar or nonpolar covalent bonds

v Polar or nonpolar molecule

a N2 - 10 linear 180 nonpolar nonpolar

b O3 ndash 18 Bent less than 120 nonpolar nonpolar

RESONANCE STRUCTURES

c H2S ndash 8 Bent less than 1095 polar polar

d NCl3 ndash 26 trigonal pyramidal less than 1095 slightly polar polar

e SiF4 ndash 32 tetrahedral 1095 polar nonpolar

CHAPTER 8 ndash NOMENCLATURE1 Name each of the following

a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4

q Hg3(PO3)2 (CLASSIC)

r Na2O2ME

s LiC2H3O2

t FeCl3 ∙ 6 H2O (CLASSIC)

u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)

a Barium Cyanideb Cobalt (II) Bromidec Phosphorus (V) Oxided Sodium Hydridee Magnesium Iodidef Calcium Arsenateg Hydrogen Chlorideh Tin (IV) Sulfatei Sulfur Dioxidej Barium Sulfitek Zinc Perchloratel Beryllium Hypobromite

m Nitric Acidn Aluminum Hydroxideo Perbromic Acidp Potassium Permanganateq Mercuric Phosphiter Sodium Peroxides Lithium Acetatet Ferric Chloride Hexahydrateu Carbon Tetrachloridev Silver Nitratew Nitrogen (III) Oxidex Lead (II) Nitride

Write the formula for each of the following

a Diboron Hexahydride

b Ammonium Chloride

c Iron (III) Nitrate

d Phosphoric Acid

e Titanium (IV) Bromide

f Cuprous Phosphide

g Selenium (VI) Fluoride

h Sodium Cyanide

i Hydroselenic Acid

j Phosphorus Triiodide

k Barium Chloride Dihydrate

l Potassium Hydroxide

m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide

p Calcium Hypochlorite

q Lead (II) Phosphate

r Magnesium Sulfate Heptahydrate

s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate

x Manganese (III) Sulfite

a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3

k BaCl2 middot 2H2Ol KOH

m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2

r MgSO4 middot 7H2Os SiO2

t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3

CHAPTER 9 ndash THE MOLE1 What is the molar mass of each of the following

a Al(C2H3O2)3 20413 gmol b Ammonium chloride 5350 gmol

c Potassium bromate 16700 gmol

2 I know that 8401 x 1024 atoms of a certain element has a mass of 3918 g

What element is this Silicon

3 How many Sulfide ions are present in 1224 mg of potassium sulfide 6683 x 1019 ions

4 How many carbon atoms are in 100 mole of dicarbon hexahydride 120 x 1024 carbon atoms

5 How many grams are 234 x 1023 molecules of C6H10OS2 631 grams

6 How many molecules can be found in a sample of 847 grams of carbon dioxide

116x 1022 molecules

7 Determine the percent composition of all of the elements found in the following compounds

a Sodium chlorate NaClO3 4510 O 3330 Cl 2160 Na

b Cuprous sulfide Cu2S 2015 S 7915 Cu

8 What is the difference between an empirical and molecular formula The empirical formula shows

the most simplified ratio of the elements in a compound The molecular formula shows the actual

ratio of the elements in the compound

9 Determine the empirical formula for a compound using the following information

a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O

10 What is the molecular formula of a compound with an empirical formula of CHOCl (chlorine) and

a molecular weight of 129 grams C2H2O2Cl2

11 What are the 7 diatomic elements Br2 I2 N2 Cl2 H2 O2 F2

12 Determine the molecular formula for a compound containing 770 carbon 130 hydrogen

and 8190 iodine Its molar mass is 281 gmol C2H4I2

13 If you take 208 g of hydrated aluminum oxide and heat it to remove all of the water what is the

formula of the original hydrate if the mass of the remaining solid after heating is 154 g Al2O3 2H2O

14 100 mol of Al2S3 consists of how many total mol of ions 500 mol (200 mol Al and 300 mol S)

CHAPTER 10 ndash CHEMICAL REACTIONS1 For each of the following

a Indicate the type of the reaction

b Predict the products by name

c Write the equation for the complete reaction If the reaction does not occur write NR

d For DD reactions include the states

e Balance the reaction only if it occurs

a silver nitrate + cupric chloride DD (precipitate) ndash silver chloride and cupric nitrate

2AgNO3(aq) + CuCl2(aq) 2AgCl(s) + Cu(NO3)2(aq)

b copper (II) + aluminum sulfate NO REACTION

c sodium nitrite + ammonium sulfate NO REACTION

d iodic acid D4 - diiodine pentoxide and water

2HIO3 I2O5 + H2O

e hydrochloric acid +barium hydroxide DD (neutralization)-water and barium chloride

2HCl(aq) + Ba(OH)2(aq) BaCl2(aq) + H2O(l)

f sodium + chromium (II) chlorate SD ndash sodium chlorate and chromium

2Na + Cr(ClO3)2 2 NaClO3 + Cr

g cupric oxide D2 ndash copper (II) and oxygen

2CuO 2Cu + O2

h C4H8 + oxygen (complete) C ndash carbon dioxide and water

C4H8 + 6O2 4CO2 + 4H2O

i dibromine pentoxide + water S4 ndash bromic acid

Br2O5 + H2O 2HBrO3

j iron (II) oxide + carbon dioxide S5 ndash iron (II) carbonate

FeO + CO2 FeCO3

k chlorous acid + magnesium hydroxide

DD (neutralization) ndash water and magnesium chlorite

2HClO2(aq) + Mg(OH)2(s) Mg(ClO)2(aq) + 2H2O(l)

l aluminum carbonate D5 ndash aluminum oxide and carbon dioxide

Al2(CO3)3 Al2O3 + 3CO2

m Sodium sulfide + hydrochloric acid

DD (gaseous) ndash sodium chloride and hydrogen sulfide gas

Na2S + 2HCl(aq) 2NaCl (aq) + H2S(g)

3

n hydrobromic acid + calcium carbonate

DD (gaseous) -calcium bromide carbon dioxide and water (carbonic acid breaks down)

HBr(aq) + CaCO3(s) CaBr2(aq) + CO2(g) + H2O(l)

2 What is the difference between oxidation and reduction Oxidation is a loss of electrons by one

reactant Reduction is a gain of electrons by one reactant

3 Write the net ionic equations for the reaction of

a hydrochloric acid + barium hydroxide H+(aq) + OH-

(aq) H2O(l)

b chlorous acid + sodium hydroxide HClO2(aq) + OH-(aq) H2O(l) + ClO2 -

(aq)

c strontium sulfide + hydrochloric acid 2H+(aq) + S -

(aq) H2S(g)

d silver nitrate + cupric chloride Ag+(aq) + Cl -

(aq) AgCl (s)

4 What are the four main signs that a chemical reaction has occurred Evolution of a gas

temperature change precipitate color change

5 Balance the following redox reaction in a basic environment

MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O

CHAPTER 11 ndash STOICHIOMETRY1 If you react 254 g of bromine with an excess of sodium iodide and you produce 2320 mg of

iodine what is the percent yield of iodine 575

2 How many grams of potassium sulfate are produced if 100 g of sulfuric acid and 70000 mg of

potassium hydroxide are mixed together What is the limiting reactant LR = KOH 10872 g

3 How many moles of chloric acid are required to react completely with 205 g of sodium carbonate

0387 mol

4 The reusable booster rockets of the US space shuttle employ a mixture of aluminum and

ammonium perchlorate for fuel The balanced equation is

3Al(s) + 3NH4ClO4 Al2O3(s) + 3NO(g) + 6H2O(l) NH3(g)

What mass of ammonium perchlorate should be used in a fuel mixture for every 100 kg of

aluminum used 436 kg

5 How many grams of magnesium chloride are produced if 420 cm3 of chlorine gas reacts with 148

g of Magnesium at STP 18 g MgCl2

6 If the following reaction produces 6840 J of energy how many grams of CrO3 is used 127 g

CrO3 + H2O H2CrO4 + 54 kJ

7 How much heat is absorbedreleased when 193 g of ammonium bromide react according to the

following equation

NH3 + HBr NH4Br ΔH = 18832 kJ

371 kJ released (enthalpy is reversed because reaction is reversed

CHAPTER 12 ndash SOLUTIONS

1 If 960 g of sodium hydroxide are used to prepare 16000 mL solution What is the molarity of the

solution 15 M

2 If we add 15 L of a 602M HCl solution and some water to a beaker creating a 242 M HCl

solution what is the volume of the new solution 37L

3 A 234 M solution contains 10 g of acetic acid What is the volume of the solution in mL 71 mL

4 What mass of sodium oxide is consumed if it reacts with 123 mL of a 345 M HCl solution 132g

5 How many grams of 67 M KClO3 are needed to prepare 100 Liters of solution 82 g

6 Describe how 100 ml of a 10 M solution of sodium hydroxide would be made Fill a volumetric

flask approximate 23 full of water Add 4 grams of sodium hydroxide to the flask Swirl the flask

Add remaining 13 of water to the solution until meniscus is at the line on the flask Mix

7 Using the pH scale define an acid and a base An acid is a substance with a pH value of 0 ndash 699

and a base is a substance with a pH value of 701 - 14

8 Calculate the pH when [H+] = 39 x 10 -5 441 Calculate the [H+] when the pH value is 957

27 x 10-10

9 Which solution is a poor conductor of electricity 1M NaCl 1MHC2H3O2 (weak acids do

notpartially ionize) 1M NaOH 1M HCl

10 What volume of 31M H2SO4 will neutralize 250 mL of 30 M Al(OH)3 360 mL

CHAPTER 13 ndash GASES1 Describe the conditions that allow a liquid to boil The vapor pressure is equal to the atmospheric

pressure allowing the liquid to evaporate

2 Compare the particles within a solid liquid and a gas The particles of a solid are close together

and fixed in place liquid the particles can slide past each other and a gas the particles are spread

out to move freely and randomly

3 Relate the intermolecular forces within a solid liquid and gas The intermolecular forces within

solid water are much stronger than liquid water The intermolecular forces within water vapor are

minimal

4 Identify and define the different phase changes of matter

a Sublimation ndash solid to gas

b Deposition ndash gas to solid

c Condensation ndash gas to liquid

d Evaporation ndash liquid to gas

e Freezing ndash liquid to solid

f Melting ndash solid to liquid

5 What is vapor pressure The force exerted by a vapor that has been released by a liquid

6 A balloon at 22 degC holds 200L of oxygen If the gas in the balloon is heated to 90deg C what

volume will the balloon be 25 L

7 What is the temperature of 70 moles of a gas that occupies 470 mL at a pressure of 150 kPa

12 K

8 5000 mL of O2 gas is collected over water Atmospheric pressure is 1010 kPa The temperature

of the water is 22 degC What is the pressure of the gas You will need a chart from your notes to

complete this problem 7378 mmHg

9 A gas is at 133 atm of pressure and a volume of 682 mL What will the pressure be if the volume

is reduced to 0419 L 216 atm

10Nitrogen gas is being held in a 143 m3 tank at a temperature of 62oC What will the volume be

when the temperature drops to 24oC 126 m3

11A gas storage tank is a 172 atm and 35oC What temperature is the gas at if the pressure

increases to 200 atm 358 K

12A gas with a volume of 100 L is at 135oC and 844 mm Hg What is the volume if the conditions

change to 14o C and 748 mm Hg 794 L

13Calculate the mass of 162 L of chlorine gas measured at STP 512 g

14Find the pressure in mm Hg produced by 235 g of carbon dioxide in a 500 L flask at 18oC

194 mmHg

15How many grams of carbon monoxide must be placed into a 400 L tank to develop a pressure of

965 mm Hg at 23oC 585 g

16At what Celsius temperature will argon have a density of 103 gL and a pressure of 643 atm

306 degC

10 What value does each of the following metric unit represent

a centi 01 or 1 x 10-2 b nano 000000001 or 1 x 10-9 c kilo 1000 or 1 x 10 3

d milli 001 or 1 x 10-3 e micro 000001 or 1 x 10-6

CHAPTER 3 ndash MATTER AND ENERGY1 Solve the following density problems using significant figures

a What is the density (gmL) of a block of metal 6cm x 10cm x 100cm that weighs 6820 dg

What would be the volume (in L) of 28 kg of the metal 245 L = 20 L

b A block of metal has a mass of 423 g It is placed in a graduated cylinder containing 560

cm3 of water If the final volume is 751 mL what is the density of the metal block 221 gmL

2 How would you separatehellip

a iron filings and pepper magnet b salt and sand dissolve the salt and filter the sand then

evaporate the water c methanol and water distillation

3 What is the specific heat of water 4184 Jg C

4 Which requires more heat to warm from 220 C to 850C if they have exactly the same mass a

sample of aluminum (c = 902 J g C) or a sample of water Explain It takes more energy to heat

one gram of water than 1 gram of aluminum because water has a higher specific heat

5 A 0234 kg sample of copper cools from 53 C to - 94 C What is the change in its energy if the

specific heat of copper is 387 Jg C - 570 J

6 Distinguish between a physical and chemical change A physical change is a change that results

in no change to the components of the substance A chemical change is a change that results in a

change to the components of the substance The identity of the substance will change due to a

physical change

7 Classify the following as either a physical or chemical change

a spoiling of milk C b softening glass to bend it into a new shape P

c burning a piece of paper C d rusting of a nail C

8 Identify the following as a pure substance heterogeneous mixture or homogeneous mixture

a copper Pure substance - element

b sweetened tea Homogeneous mixture - solution

c calcium carbonate Pure substance - compound

d sandy water ndash Heterogeneous mixture - suspension

9 What is the difference between an exothermic reaction and an endothermic reaction Relate each

reaction type to enthalpy Endothermic reactions absorb energy and the products have more energy

than the reactants The enthalpy change for an endothermic reaction is positive Exothermic

reactions release energy and the products will have less energy than the reactants Exothermic

reactions have a negative enthalpy change








d 35 p 35 e 45 n Br




d Co 27p 32n 27e e 56 Fe 26p 30n 26e

26







Conversation mass




abundance in nature



9241 698 amu








debate










ratio




















623 x 10 -13 m


5762 x 10-19 J





a argon b copper

c nitrogen





















Strontium





carbon 4 C-4

3 Which is smaller



period












electron


a b c


energy


18
















a b c d e








F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC








d 35 p 35 e 45 n Br




d Co 27p 32n 27e e 56 Fe 26p 30n 26e

26







Conversation mass




abundance in nature



9241 698 amu








debate










ratio




















623 x 10 -13 m


5762 x 10-19 J





a argon b copper

c nitrogen





















Strontium





carbon 4 C-4

3 Which is smaller



period












electron


a b c


energy


18
















a b c d e








F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC




abundance in nature



9241 698 amu








debate










ratio




















623 x 10 -13 m


5762 x 10-19 J





a argon b copper

c nitrogen





















Strontium





carbon 4 C-4

3 Which is smaller



period












electron


a b c


energy


18
















a b c d e








F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC












623 x 10 -13 m


5762 x 10-19 J





a argon b copper

c nitrogen





















Strontium





carbon 4 C-4

3 Which is smaller



period












electron


a b c


energy


18
















a b c d e








F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC

















Strontium





carbon 4 C-4

3 Which is smaller



period












electron


a b c


energy


18
















a b c d e








F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC





electron


a b c


energy


18
















a b c d e








F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC






F2








tetrahedral)











a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC



a Ba(CN)2

b CoBr2

c P2O5 (STOCK)

d NaH

e MgI2

f Ca3(AsO4)

g HCl

h Sn(SO4)2

i SO2 (CLASSIC)

j BaSO3

k Zn(ClO4)2

l Be(BrO)2

m HNO3 (aq)

n Al(OH)3

o HBrO4 (aq)

p KMnO4


r Na2O2ME

s LiC2H3O2


u CCl4

v AgNO3

w N2O3 (STOCK)

x Pb3N2 (STOCK)





b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC


b Ammonium Chloride


d Phosphoric Acid


f Cuprous Phosphide


h Sodium Cyanide

i Hydroselenic Acid




m Mercuric Sulfate

n Auric Bromide

o Cadmium Oxide




s Silicon Dioxide

t Sulfuric Acid

u Aluminum Chlorate

v Magnesium Sulfide

w Plumbous Acetate


a B2H6

b NH4Clc Fe(NO3)3

d H3PO4

e TiBr4

f Cu3Pg SeF6

h NaCNi H2Sej PI3


m HgSO4

n AuBr3

o CdOp Ca(ClO)2

q Pb3(PO4)2


t H2SO4

u Al(ClO3)3

v MgSw Pb(C2H3O2)2

x Mn2(SO3)3










116x 1022 molecules








a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC







a 5800 Rb 950 N 3250 O RbNO3

b 4962 C 1082 H 3956 O C5H13O




















2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC












2HIO3 I2O5 + H2O






2CuO 2Cu + O2


C4H8 + 6O2 4CO2 + 4H2O


Br2O5 + H2O 2HBrO3


FeO + CO2 FeCO3









3








(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC







(aq) H2O(l)


(aq)


(aq) H2S(g)


(aq) AgCl (s)




MnO4- + SO2 SO4 -2 + Mn+2

4OH - + 5SO2 + 2MnO4 - 2Mn+2 + 5SO4-2 + 2H2O






0387 mol











following equation





solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC


solution 15 M












27 x 10-10











minimal












12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC




12 K














194 mmHg


965 mm Hg at 23oC 585 g


306 degC

name_____________________________ - north · web viewif 36 grams of water are produced and 4...

Documents