Test 4 Handouts

8/10/2019 Test 4 Handouts

1/23

BALANCING

CHEMICALEQUATIONS

Name

Rewrite

and

balance

the

equations

below.

. N

2

+ H

2

NH,

2. KCIO, KCI + C X

3. NaCI + F

2

-* NaF +CI

2

4.

H

2

+ O

2

H

2

O

5. AgNO

3

+ MgCI

2

AgCI+ Mg(NO

3

)

2

6.

AIBr

3

+

KjSO,

KBr + A I

2

(SO

4

)

3

7. CH,

+

O

2

-* CO

2

+

H

2

O

8.

C

3

H

8

+ O

2

-*

CO

2

+

H

2

O.

9. C

8

H

18 +

0

2

10

2

+H

2

0

10. FeCL

+ NaOH

Fe(OH)

3

+

NaCI.

11.

P+

O,

12. Na +

H

2

O

NaOH +

13.

Ag

2

O

-

Ag

+

O

2

14. S

8

+0

2

- S0

3

.

O A. 0

15. C0

2

+

H

2

0

0

16. K

+ MgBr

2

17,

HCI + CaCO,

KBr + Mg

CaCI

2

+ H

2

O +CO

2

.

Chemistry IF8766

58

Instructional


2/23

EQUATIONS

Name

theword

equations

belowaschemical equationsandbalance.

zinc

+

lead(II) nitrate yield

zinc

nitrate

+

lead

2

aluminumbromide +chlorine yield aluminum chloride +bromine

3 ,

sodiumphosphate

+

calcium chlorideyieldcalcium phosphate

+

sodium

chloride

4. potassiumchloratewhenheatedyields potassiumchloride + oxygen gas

5 . aluminum

+

hydrochloricacidyield aluminum chloride

+

hydrogen

gas

6 .

calcium hydroxide

+

phosphoricacid yieldcalciumphosphate

+

water

7 .

copper

+ sulfuricacid

yield copper (II)sulfate

+

water

+

sulfur dioxide

8 .

hydrogen +nitrogen monoxide yield water + nitrogen

i

nc

Chemistry IF8766

59 Instructional

Fa i r ,

in


3/23

TYPES OF REACTIONS

Thereare 5main typesofreactions.

1. Direct CombinationCompositionSynthesis:

Two ormore elements orcompounds A and B)combine toforma

more complex substance. ABoneproduct)

A + B AB

Examples:

Write equationsshowing

the

direct combination

of the

elements below:

a. Sodium

and

iodine

b. calciumandoxygen

c. hydrogen and chlorine

d.

hydrogen

and

carbon monoxide

and

oxygen

to

form carbonic

acid

e. nitrogenandhydrogentoform ammonia

2. DecompositionAnalysis:

^ Reverse

of

direct combination.

A

complex compound

ABone

reactant)

isbroken down intotwo ormore simpler substances.

Aand B,elements and/or compounds)

AB *

A + B

Examples: Write equations showing

the

decomposition

of

each

of

the

following substances:

a. Water

b. silver chloride

c.

aluminum oxide

d. lithium phosphate to form

lithium,

phosphorous and oxygen

e.

sulfuric acid to form hydrogen, sulfur and oxygen

3. Single Replacement:

Onesubstance isreplaced from-itscompound byanother

substance.

Element + compound -^ element + compound

A + BC

*

B + AC


4/23

Note: Cationic single

replacement: is

when metals replace

metals andhydrogen. +ion)

AnionicSingle replacement: is when nonmetals replace

nonmetals.

-

ion)

To see if a

reaction takes place

use

Table

J. A

more active

metal replacesaless active metalor amore active nonmetal

replaces

a

less active nonmetal.

If

this

is not the

case

a

reaction will not occur.

Examples: Decideif thefollowing reactions will occur. If

they

dotake place determinetheproductsofeach reaction.

a.

zinc and nitric

acid

b. iron andcopper IIsulfate

c. sodium and water

d. magnesium chlorideandfluorine

e. sodium chloride and bromine

4. Double Replacement:

Twocompounds combine toformtwo newcompounds.

AB + CD

*

AD + CB

Note: +

ions switch places.

These equations are also known as ionic equations. Ionic

equations have

two

possibilities:

a. Reactions go to completion stops): When ions in a solution

combine to form a productthatleaves the scene of a

reaction. There are three types of products that leave the

scene of a

reaction.

1. Slightlyionizedwater

2.

Gases escape Cf)

3. Precipitates settle

to the

bottom 4*)

Precipitates are solid substances formed by a physical

orchemical change in a liquid medium. It separates

from the liquid by settling to thebottom.Precipitates

are insoluble compounds see table F.

b. If a reaction does not go to completion they are said to be

Reversible. 5). Areversible reactionis one inwhichthe

products can themselves react to form the reactants.

Examples: For each reaction write themolecular,ionic and

Netionic equations:

a. silver nitrateandzinc chloride


5/23

b.

copper

IIhydroxideandacetic acid

c.

iron II

sulfate

andammonium sulfide

5. Complete Combustion:

When

a

hydrocarbon compound composed

of

onlycarbon

and

hydrogen) or acarbohydrate compound composed ofcarbon,

hydrogen andoxygen) react with oxygentoform carbon dioxide

andwater.

Example: Write anequationfor thecomplete combustion ofeach

ofthe

following

organic substances:

a.

b. CH

4

c

C

2

H

2

d.

C

6

Hi

2

0

6


6/23

Name

Date

Class

CHAPTERS REVIEW

ACTIVITY

TtxtReferenct:Section-13

Chemical Changes

Choose word*fromtrwlistto fill In the blanks in the paragraphs.

WordUat

analysis

arrow

chemical equation

chemicalreaction

coefficient

delta

doublereplacement

electrolysis

endothermic

exothermic

ionic equation

precipitate

product

reactant

single

replacement

spectator

synthesis

Another name for a chemical change is

a(n)

LD Such a change can

be

represented

by means of a written statement called a(n)

(

2

)

. The

symbol

for the

word yields

in

such

a

statement

is

a(n) GD

Any

substancewrittento the leftof thissymboliscalled

a(n)

.

W

_ .Any

substancewritten to the right ofthis

symbolis

called

a(n)

GJ) A

number written

just

to the

left

of a formula is called a(n)

()

A

chemjMf

changeinwhich energy is absorbed is called a(n) (?)

reaction.

One in which energy is released iscalled a(n) (8) reaction.

Some chemical

changes

involve charged particles. Anequation that

showsthe

reaction

or

production

of

such

paniclesis

called

a(n)

C O

.

Any

charged

particle

that

is

present

but that

does

not change or react

during areaction isusually omitted from theequation; it iscalled

a(n)

(IP)

A

chemical change

in

which

two or

more substances combine

to form

a more complex substance is called a(n) (H) reaction. A change in

which

asubstanceisbroken down into

simpler

substancesiscalleda(n)

(12) reaction.Any such change that is caused by the flow of anelectric

current is called a(n) (13) . If the change iscausedby heat supplied to

the reaction, the Greek symbol

(H) isoften

written above the yields

symbol

in the

equation.

A chemical change

in

which

a

free

element replaces and releases

another

element

in acompoundiscalleda(n) (15) reaction. Achemical

change inwhich there isanexchangeofions betweentw ocompoundsis

called

a(n)

(*6) reaction. Asolid substance producedbysucha reac-

tion

inaliquid

medium

is

called a(n)

(

17

) .

1.

2.

3.

4.

5.

.

7.

g.

9.

10.

11.

12.

13.

14.

IS.

16.

17.

9 4 CHEMIST1Y:

Th

StudyofMattar

COPYRIGHTbyPrtotic*Hall,Inc

Reproductionofthil matter u

rvttrkltd

toduplicationfixd*uroomUM only.


7/23

Name

Date

Class

CHAPTERS

REVIEW ACTIVITY

Text Reference:Section9-12

Categories of Chemical Reactions

State whether each of thefollowingequations represents a synthesis

i),analysis a),single replacement sr),

or

doublereplacement dr)

reaction.

1.

CO

2

-*

C +

O,

1.

2.

NaCl

+ AgNOa

-

NaNO,+

AgCl

2.

8. S + CU

-+

SCU 3.

4.

BaClt

+

2NaOH

-*

2NaCl

+

BaTOH),

4.

5.

Zn

+

CuSO

4

-*ZnSO

4

+ Cu 5.

6.

CH*

-*

C +

2H

2

6.

7.

PbCNO,)s

+

Mg-*Pb

+

MgCNOsk

7.

8.

Mg

+

2HC1- MgCU

+

Hi

8.

9. HjSO

4

-*

H

2

+S +20

2

9.

10.

2Oj+

N

s

-*N

A 10.

11.

3CaBr

2

+ 2Na

s

P-

Ca

s

ft +

6NaBr

11.

12. 2KI

-l - Br

2

-2KBr

+

I

2

12.

18.

CflHtfO,,

- 6C +

6HzO

13.

14.

2NaF

- 2N a+ R 14.

15.

Si +

O

2

-

SiO

2

15.

16. 2NaI -t -

Pb(NO

8

)2

-2NaNO

3

- f Pb I

2

16.

17.

N al+ Cs-*

Csl

+ Na

17.

18. H

2

+ CO

+O

2

-

H

2

CO

3

18.

19. LJaPO

4

-3Li

+

P + 2O

2

19.

20. CSz +

2FJ

-

CF

4

+ 2S 20.

J

COPYRIGHT

by Prtntic*

Hll.

Inc.

Rtproduction of

thu

mrtr

(rttridd

to duplication for

eUwoom

UM

only.

CHEMISTRY:ThStudyofMatter 9 3


8/23

CLASSIFICATIONOF

Nome

CHEMICAL REACTIONS

Classify

thereactions belowas

synthesis,

decomposition,singlereplacement

(cationic

anionic) or

double

replacement,

2H

2

+

O

2

- 2H

2

O

2. 2H

2

O - 2H

2

+ O

2

3.

Zn +

H,SO,

ZnSO. + H

2 4

2

4. 2CO

O

2

- 2CO

2

5.

2HgO -*

2Hg

O

2

6. 2KBr + CI

2

- 2KCI +

Br

2

7.

CaO + H

2

O

-

Ca(OH)

2

8. AgNO

3

+ NaCI

AgCI

+ NaNO

3

9. 2H

2

O

2

2H

2

O +

O

2

10.

Ca(OH),

+ H

2

SO

4

~- CaSO,, 2H,O

'H .

:

, t r, '8766

50 Inotfjctionai

f f j i f . m


9/23

Name

predict

theproductsof thereactions below. Then, writethe

balanced

equationand

c l a s s i f y

the reaction.

^

magnesium

bromide

chlorine

2 aluminum + iron (III) oxide

3 .

silvernitrate + zinc chloride

PREDICTING

PRODUCTS

CHEMICAL REACTIONS

4 hydrogen peroxide (catalyzed by manganese dioxide)

5 zinc

hydrochloricacid

6

sulfuricacid

+

sodium hydroxide

sodium

+

hydrogen

Qceticacid + copper


10/23

PROBLEMS

INVOLVING EQUATIONS

The

coefficients used

in

balancing

a

chemical equation

represent

moles.

Instoichiometric problems involving

equations it isassumed thatthereactionis the single

reaction

with

noside reactions),thatthereaction goes

tocompletion

and the

reactants

are

completely reacted.

Every stoichiometric problem involvesthefollowing

three basic

steps.

Stepl: Find

the

moles

of the

substance

you are

given

information

about.

Moles

=

g/gfm Moles=1/22.4 Moles

= ftp/6.02 x

10

23

Step 2: Set up amole ratio.

Actual moles from step1) = Actual moles

unknown)

Theoretical moles fromcoefficients)Theoretical moles

Step 3: Find

the

grams, liters

or

particles

of

your

unknownusingone of thethree mole equations from step1.

Type 1: Mass-Mass Problems:

A

balanced equationshows

the

moleproportions

of

products

f toreactants. It ispossibletodeterminethemassof one

substance that reacts withor isproduced fromagiven mass

of

another substance.

Examples:

1.

How

many grams

of

sodium chloride

are

needed

to

react

toproduce 35.5 gramsofchlorinegas?

2. How manygramsofhydrogenareproduced by theaction

ofwateron 100.gramsofsodium?

3.

What massof

oxygen

will combinewith3. 0

grams

of

hydrogen

to

produce water?


11/23

4.

Given

the

reaction:

N

2

+

0

2

-

2NO. What

is the

total

number

of

grams

of

oxygen needed

to

react completely

with

2. 0

moles

of

nitrogen?

Type 2: Mass-Volume

Problems:

A

mole 6.02

X 10 ) of

molecules

of any gas

occupies

a

volume

of22.4 litersat STP. This numerical valueis

called themolarvolume. It has amass equalto the

molecular mass expressed in

grams.

In abalanced equation

where

the

mole unit serves

to

relate

the

quantities

of

products andreactants,it ispossibletodetermine

quantitative

resultsindesired units, whichmay not

necessarily

be the

same

as the

original units.

Examples:

1. Howmany gramsofzinc metalareneededtoreact with

hydrochloric acidtoproduce 11.2 litersofhydrogen

gas at

STP.

2. Howmany gramsofcarbon dioxideat STP are produced

by the

complete combustion

of C

2

H

e

?


12/23

Type 3: Volume- Volume Problems:

Since

one

mole

of any gas

occupies

the

samevolume

as one

mole of any other gas, at the same temperature and

pressure,

the

volumes

of

gases involved

in a

reaction

are

proportional to the number of moles indicated by the

numerical coefficients in a balanced equation.

Examples:

1. In the

reaction N

2

+

H

2

->

2NH

3;

calculate

the

volume

of

hydrogen

gasrequired toform100. litersofammonia?

2. What volume of carbon dioxide will beformed fromthe

complete combustion of 21.2 liters of camphene Ci

0

H

6

)?


13/23

STOICHIOMETRY:

MOLE-MOLE

PROBLEMS

Name

4.

N

2

+ 3H

2

-* 2NH

3

Howmany moles

of

hydrogen

are

needed

to

completely react with

twomoles

of

nitrogen?

2. 2KCIO,

2 K C I +

3O,

Howmanymoles of oxygen areproducedbythe'decompositionof sixmoles

ofpotassium chlorate?

3. Zn + 2HCI -

ZnCI

2

+ H

2

Howmany molesofhydrogenareproducedfromthereactionofthree moles

ofzincwithan

excess

ofhydrochloric acid?

C

3

H

5CL

3C0

4H

2

0

. _ 2 2

Howmany

molesof

oxygen

are

necessary

to

react completely with fourmoles

of

propane(C

3

H

8

)?

5.

K

3

P0

4

+

AI(N0

3

)

3

-*

3KN0

3

+

AIPO

4

Howmanymolesofpotassium nitrateareproduced whentwomolesofpotassium

phosphate

react withtwomolesofaluminum nitrate?

Chemistry IF8766

62

Instructional

Fair,


14/23

STOICHIOMETRY:

MASS-MASS PROBLEMS

Name

1 .

2KCIO,

2KCI

+ 3O

0

Howmany gramsofpotassium chlorideareproducedif 25 g ofpotassium chlorate

decompose?

2.

N

2

+

3H

2

- 2NH

3

Howmany

grams

ofhydrogenarenecessary toreact completelywith50.0g of

nitrogenintheabove reaction?

3.

How

manygrams

of

ammonia

are

produced

in the

reaction

in

Problem

2?

4. 2AgN0

3

+ BaCI

2

- 2AgCI + Ba(NO

3

)

2

How

many grams

of

silver chloride

are

produced

from5.0 g ofsilver

nitratereacting

withanexcess ofbarium chloride?

5. How much barium chlorideis necessary to reactwiththe silver nitratein Problem4?

Chemistry

IF8766

64

InstructionalFa ir,

nc


15/23

5TOICHIOMETRY:

VOLUME VOLUME PROBLEMS

Name

N, + 3 H

2

2NH,

What

volume

ofhydrogenis

necessary

toreact with fiveliters ofnitrogentoproduce

ammonia?

(Assume

constant temperatureandpressure.)

2.

What volume of ammonia is produced in the reactionin Problem1?

3. C

3

H

8

+50

2

3CO

4H

2

O

If

20

liters

o f oxygena re consumedin the above reaction,how many

liters

of carbon

dioxide are produced?

4. 2H

2

0 2H

2

+0

2

If

30ml ofhydrogenareproducedin theabove reaction,howmanymilliliters of

oxygen are

produced?

5.

2CO + O

2

-* 2CO

2

How

many liters of carbon dioxidea re produced if 75 liters of carbon monoxide

a re

burned

in

oxygen?

How

many

liters

of

oxygen

a re necessary?

Chemistry IF8766

63

Instructional Fa i r , Inc.


16/23

I

STOICHIOMETRY:

MASS-MASS PROBLEMS

Name

\

1. 2KCIO,

2KCI + 3CX

How

many

gramsofpotassium

chloride

are

produced

if 25 g of

potassium chlorate

decompose?

2. N

2

+

3H

2

- 2NH

3

How

many

gramsof

hydrogen

arenecessaryto

react completelywith50.0

g of

nitrogen

inthe

above reaction?

3.

How

manygrams

of

ammonia

are

produced

in the

reaction

in

Problem

2?

Ba(NO

3

)

2

.

2AgNO

3

+

BaCI

2

-

2AgCI

How

many

grams

ofsilver

chloride

are

produced

from5.0 g ofsilvernitrate

reacting

with

anexcessof

barium chloride?

5.

How

much barium chloride

is

necessary

to

react with

the

silvernitrate

in

Problem

4?

Chemistry

IF8766

64

InstructionalFa ir, nc


17/23

STOICHIOMETRY:

Name

VOLUME VOLUME PROBLEMS

1. N

2

+ 3H

2

- 2NH

3

Whatvolume

of

hydrogen

is

necessa ry

to

react withfive liters

of

nitrogen

to

produce

ammonia?

(Assume

constant temperatureandpressure.)

2.

What volume

of

ammonia

is

produced

in the

reaction

in

Problem1

?

3.

C

3

H

8

+ 5O

2

- 3CO

2

+ 4H

2

O

If20liters ofoxygenareconsumedin theabovereaction,howmanyliters ofcarbon

dioxide are produced?

4. 2H

2

0

2H

2

+0

2

If

30

mL

of

hydrogen

are

produced

in the

above reaction,

how

manymilliiiters

of

oxygen

are

produced?

5.

2CO + O

2

->

2CO

2

Howmany liters ofcarbon dioxideareproducedif 75

liters

ofcarbon monoxide

are

burned

in

oxygen?

How

many

liters

of

oxygen

arenecessary?

Chemistry IF8766

63 InstructionalFa ir, Inc.


18/23

llOICHIOMETRY:

MIXED PROBLEMS

Name

N

2

+ 3H

2

- 2NH

3

What

volume

of

NH

3

at

STP

is

produced

if

25.0

g of

N

2

is

reacted with

an

excess

ofH,?

2.

2KCIO

3

-* 2KCI

+

3O

2

If5.0 g ofKCIO

3

isdecomposed, what volumeof O

2

isproducedat STP?

3, Howmany gramsof

KCI

areproducedinProblem2?

4. Zn +

2HCI -

ZnCI

2

+

H

2

What

volumeofhydrogenat

STP

isproduced when2.5

g

of zincreact withan

excessofhydrochloric acid?

5.

H

2

SO

4

+ 2NaOH

-* H

2

O

+

Na

2

SO

4

How

many moleculesof water areproducedif 2.0 g ofsodiumsulfate are

produced

in the

abovereaction?

6.

2AICI

3

-

2AI +

3CI2

If

10.0

g ofaluminum chloridearedecomposed,howmany moleculesof CI

2

are

produced?

w

Chemistry

IF8766

65

Instructional Fa i r , Inc.


19/23

STOICHIOMETRY:

LIMITING

REAGENT

Name

f onaj -fopfc)

. N

2

3 H

2

2NH,

Howmany

gramsofNH

3

can be

produced

fromthereactionof 28 g of

N

and

25g ofH

2

?

2. Howmuchof the excess

reagent

in

Problem

1 s

eft over?

3.

Mg +

2HCI

-

MgCI

2

+

H

2

What volume

of

hydrogen

at STP isproduced

from

the

reaction

of

50.0

g of M

theequivalentof 75 g of HCI?

4. How much of the excess reagent in Problem3 is leftover?

5. 3AgNO

3

+

Na

3

PO

4

-

Ag

3

P O

4

+ 3NaNO

3

Silvernitrate and sodium phosphate arereactedinequalamounts of 200. g

ea

How

manygrams

of

silver phosphate

are

produced?

6.

How

much

of the excess

reagent

in

Problem

5 is

eft?

ChemistryIF8766

66

Instructiona


20/23

N a m e

IL

Class

Mass-Mass Problems

Solving

mass-mass

p roblems usual ly involves these steps:

1.

Convertgiven masses in gramsto moles.

2.

U se coefficients in the balanc ed equ ation to establish mo le

ratios

between

the substances involved in the problem.

3.

Calculate th e numb er of moles of the required substance.

4. Convert

that

number of moles to mass in grams.

Examples

How many moles

of

F

2

are

there

in

60.0s

o fF,?

(F

= 19.0

g/mole)

mole

mass

of F

2

= 2 x 19.0

g/mole

= 38.0

g/mole

60.0 g

38.0

g/mole

=

1.58 moles

In the

followingreaction,

ho w

many moles

of F

2

are

needed

to

produce 1.5

moles

of HF?

H

2

2HF

mole ratio ofF

2

to HF = 12

1:2= ?:1.5 ? = .75

How many grams of HF is .75 moles of HF? (H = 1.0 g/mole)

mole mass of HF = 1.0 g/mole + 19.0g/mole= 20g/mole

.75 moles x 20g/mole= 15 g

c

o

I Solve the

following problems. Show

your

work.

| 1.

Given

the

equat ion

N

2

(g)+

3H

2

(g)-

2N H

3

(g)

answerthe

fol-

lowing questions.

a. How many moles of N

2

are there in 200 g ofN,?

(N

= 14.0

g/mole)

la.

Date

o

b.

H ow

many moles

of

NH

3

could

be

produced

from the

above amount

of

N

2

?

c.

How many grams ofNH

3

would

this

be?

(H =

1.00 g/mole)

c.

11-3


21/23


22/23

Name

Class

Volume-Volumeand Mass-Volume Problems

Date

Volume-volume problems involve direct comparisonof the

coef-

ficients

in abalanced

equation.

The

reason

is

that equal volumes

of gases at the same temperature and pressure contain equal

numbers of moles and molecules. Also involved is thefactthat at

STP the volumeof a gas isequalto22.4L /mole.Calculationof

numbers

of

molecules involves

the use of Avogadro's

number,

6.02 x

10

23

molecules/mole.

Examples

Howmanylitersof HC1 gas can beproducedfrom 10 L ofC1

2

gas

by the reaction H

2

+C1

2

-*2HC1?

1:2=

10L:?L

? = 20 L

Howmany gramsofhydrogen gas (H

2

) areneeded toproduce

5.00

L ofwater vapor, measuredatSTP, accordingto the reac-

tion

2H

2

+O

2

-2H

2

O? (H = 1.00 g/mole; O = 16.0g/mole)

5.00

L

=.223 molesof

H

2

O

vapor

22.4

L/mole

2:2

= ?

moles

H

2

:.223

molesH

2

0

? =

.223 molesH

2

.223

moles

x

2.00g/mole

=

.446

g

H

2

Howmany H

2

molecules aretherein .223 molesof H

2

atSTP?

.223

moles

x

6.02

x

10

23

molecules/mole

= 1.34 x

io

23

molecules H

2

Solve

thefollowing problems. Show yourwork

1. Howmany

liters

of

CO

2

can beproduced

from

14.5L of C

2

H

2

by

the reaction

2C

2

H

2

(g)

+

50

2

(g)

-

4C0

2

(g) +

2H

2

0(g)

2. Howmanylitersofoxygenarereleased

from

thedecomposi-

tionof 3.6 L of hydrogen peroxide gas

(H

2

O

2

)

to produce

water vaporandoxygen? (Writethe

balanced

equation for

the

reaction

as

part

of

your work.)

2H

2

0

2

(g)-+2H

2

0(g) +0

2

(g)

2.

< ~ H F M T S T R Y

Review Activity

11 5


23/23

Name

Class

Volume-Volumeand

Mass-Volume

Problems Continued)

3. How many grams of zinc (Zn = 65.4g/mole) arerequired to

produce

67.2

L of

hydrogen

gas at

STP, according

to the reac-

tion

2HCl-ZnCl

2

+

H

7

3.

Date

4. a. How manyliters of

C1

2

gas

at STP can be produced by

decomposing 70.0g of HC1

gas?

(H = 1.00 g/mole;

Cl

=

35.5g/mole) (Includeabalanced equa tioninyour work.)

4a.

b. How many

C1

2

molecules would be produced?

5. How many liters of H

2

O vapor could be produced by the

reaction

of

9.03

x

10

23

m olecules

of

O

2

,according

to the re-

action

2H

2

(g)

+

0

2

(g)

-*

2H

2

0(g)

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