KINETIKA REAKSI-

8/17/2019 KINETIKA REAKSI-

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KINETIKA KIMIA

BAMBANG WIDIONO


2/77

KINETIKA KIMIA ? "how fast do reactionsgo?"

Untu a!a ? #anfaat $ Mata u%iah ter ait ? #ate#ati a&

stoi io#etri& ' $


3/77

Understanding how chemical reactors work lies at the heart ofalmost every chemical processing operation.

Design of the reactor is no routine matter, and many alternatives can be proposed for a process. Reactor design uses information,

knowledge and experience from a variety of areas -thermodynamics, chemical kinetics, fluid mechanics, heat and masstransfer, and economics .

CR is the synthesis of all these factors with the aim of properlydesigning and understanding the chemical reactor.

What is Chemical Reaction Engineering(CRE) ?

(he#ica%

!rocess

)aw

#ateria%

*e!aration

+rocess

*e!aration

+rocess

+roducts

B, !roducts


4/77


5/77


6/77

T,!ica% (he#ica% +rocess

+h,sica%treat#entste!s

(he#ica%treat#entste!s

+h,sica%treat#entste!s

)aw#ateria%s

- !re.treat#ent - se!arations

- !urifications

+roducts

)EA(TION ENGINEE)ING

Unit O!erations


7/77

Boo

- O.Levenspiel: / (he#ica% )eactionEngineering 0

- S.Fogler: /E%e#ents of (he#ica%)eaction Engineering0

- 1 M *#ith 2 / (he#ica% Engineering

Kinetics /- *tan%e, M Wa%as 2 / (he#ica% )eaction

Engineering 3and4oo 0


8/77

!ersa#aan rea si tida da!at#en5awa4 6 isu !enting

78 *e4era!a ce!at rea si 4er%angsung98 Bagai#ana onsentrasi rea tan dan !rodu

saat rea si se%esai68 A!a ah rea si 4er5a%an dengan sendirin,a

dan #e%e!as an energi& atau ah ia

#e#er%u an energi untu 4erea si?


9/77

Kineti a i#ia

- *tudi tentang ece!atan rea si i#ia danfa tor.fa tor ,ang #e#!engaruhin,a serta#e anis#e rea si


10/77

(%assification of )eactions

Man, wa,s of c%assificationMost usefu% . according to nu#4er : t,!es of !hases

3o#ogeneous2 reaction ta es !%ace in 7 !hase3eterogeneous2 reaction )E;UI)E* at %east 9 !hases

+hase < unifor# +&T& (o#!osition

According to the use = not use of cata%,stNoncata%,tic(ata%,tic


11/77

(%assification of )eactions

3o#ogeneous

3eterogeneous

Noncata%,tic (ata%,tic

Most gas.!hase reactions Most %i>uid.!hase r s

@ast reactions such as4urning of a f%a#e

) s in co%%oida% s,ste#s

En ,#e and #icro4ia% r s

Burning of coa%

Attac of so%ids 4, acids

Gas.%i>uid a4sor!tionwith reaction

A##onia s,nthesisO idation of a##onia!roduce to nitric acid


12/77

Menge s!resi an a5u )ea si

t x

t t x x

∆∆=−

−==!"

!"

waktu#erubahan posisi#erubahan

$erak%a&u

t t t ∆∆−=−

−−=

='()onst*')onst')onst

waktu#erubahan'ikonsentras#erubahanreaksi%a&u

!"

!"

[ ] [ ]t

Bt

A Laju

∆∆=∆

∆−=


13/77

3ow can reaction rate 4ee !ressed ?

- *e%ect one reaction co#!onent forconsideration and define the rate in ter#sof this co#!onent& i 8

- If the rate of change in nu#4er of #o%es ofthis co#!onent due to reaction is dN i /dt &then the rate of reaction in its Cariousfor#s is defined as fo%%ows2


14/77

)eaction )ate Definition

- the rate at which a s!ecies %ooses its che#ica% identit, !er unit Co%u#e

@or f%uid s,ste#s . 4ased on unit Co%u#e of f%uid = unit Co%u#e of reactor

(time) fluid)of (volume formed imoles

dt dN

V r ii ==

!(time)reactor)of (volume

formed imolesdt

dN V

r ir

i==′ !

@or gas.so%id s,ste#s . 4ased on unit Co%u#e of so%id

(time) solid)of (volume formed imoles

dt dN

V r i

S i

== !++


15/77

)eaction )ate Definition

@or 9 f%uid s,ste#s = gas.so%id s,ste# . 4ased on unit interfacia% surface

(time)(surface)

formed imoles

dt

dN

S r iS i ==

!

@or f%uid.so%id s,ste#s . 4ased on unit #ass of so%id

(time) solid)of (mass

formed imoles

dt

dN

W

r iwi ==!

+++ir iS

S i

wii r V r V Sr Wr V r ====


16/77

*!eed of (he#ica% )eactions

ce%%u%ar r s8

watertreat#ent !%ants

hu#anat rest

wor inghard

gases in !orouscata%,st !artic%es

7 . 7 .6 7 .9 87 7 7 7

roc etengines

r i''

= moles of i disappearing(m 3 of thing) (s)


17/77

)eaction )ate F e a#!%e 7

The roc et engine2

- 4urning a stoichio#etric #i ture of fue% %>8 h,drogen : o ,gen$

- (,%indrica% co#4ustion cha#4er2 < Hc#& D< c#- +roduces 7 J g=s e haust gases

)eaction rate ofh,drogen and o ,gen?


18/77

)eaction rate F e a#!%e 7

dt

dN

V r H H

"

"

!=−

dt dN

V r OO

"

"!=−

3m L D

V "!"!.(.*/

(0.*/

""

=== π π

O H O H """ "! →+

smol mol !

s! O H

s

! 10

(1*!2

(1*! 2! 2 " ==

?

smol

used H 03"

smol

used O 43"

smmoles

smol

r H ⋅

×==−4

/!2."0

"!"!.!

" smmoles

smol

r O⋅

×==− 4/!/!.!

4"!"!.!

"


19/77

)e%ationshi! 4etween rates of

reaction F e a#!%e 9The reaction carried out in a reactor2

If at a !articu%ar !oint& the rate of disa!!earance of A is 7 #o%=d# 6=s& what

are the rates of B and (?

" B A 4" →+

4"

" B A r r r =−=− sdm

mol sdm

mol r r A B

⋅=

⋅=−=− 44 !"

!4

"4

sdmmol

sdmmol r

r A" ⋅

=⋅

=−=− 44 ""!

"


20/77

Kece!atan rea si- Kece!atan rea si die s!resi an 2

To increase the rate 2- increasing the surface area of so%ids$.this a%%ows for #ore co%%isions and giCes

#ore #o%ecu%es the right geo#etr,

- increasing the te#!erature .this giCes #ore #o%ecu%es the right energ, a%soca%%ed the actiCation energ,& Ea$

- increasing the concentration of gases and so%utions$.this a%%ows for #oreco%%isions and #ore correct geo#etr,

- using a cata%,st .he%!s #o%ecu%es achieCe the correct geo#etr, 4, !roCiding adifferent wa, to react

- The !h,sica% state so%id& %i>uid or gas$ of a reactant

- Nature of reactants . Na is #ore reactiCe than (a it #ore easi%, %oses its outere%ectron$

rate


21/77

Luas Permukaan Sentuhan- *uatu rea si #ung in 4an,a #e%i4at an

!erea si da%a# 4entu !adatan- Menga!a e!ingan ,ang %e4ih ha%us 4erea si

%e4ih ce!at? +ada ca#!uran !erea si ,angheterogen& rea si han,a ter5adi !ada 4idang

4atas ca#!uran ,ang se%an5utn,a ita se4ut4idang sentuh8 O%eh arena itu& #a in %uas4idang sentuh #a in ce!at 4erea si8 1adi #a inha%us u uran e!ingan at !adat #a in %uas!er#u aann,a8

- Artin,a #a in eci% u uran& #a in %uas!er#u aann,a& #a in 4an,a tu#4u an& #a ince!at ter5adin,a rea si

h ff f


22/77

The effect of increasing te#!erature

- When the te#!erature is raised the added heat energ,shows itse%f in the for# of increased !artic%e inetic energ,8In the gra!h a4oCe& two distri4ution curCes are shown for a%ower=higher te#!eratures& T7=T9& and it is assu#ed that thearea under the who%e curCe is the sa#e for 4othte#!eratures i8e8 the sa#e nu#4er=!o!u%ation of #o%ecu%es8


23/77

- (o#!aring lower temperature T1 with higher temperature T2 & ,ou can see that asthe te#!erature increases & the !ea for the #ost !ro4a4%e KE is reduced& and #oresignificant%, with the rest of the KE distri4ution& #oCes to the right to higher Ca%ues so#ore !artic%es haCe the highest KE Ca%ues 8

- Now& if we consider an acti ation energ! Ea & the #ini#u# KE the !artic%es #ust haCeto react Cia e8g8 4ond 4rea ing& the fraction of the !o!u%ation a4%e to react at T1 isgiCen 4, the "lue area 8

- 3oweCer& at the higher te#!erature T2 & the fraction with enough KE to react is giCen 4,the co#4ined "lue area plus the re# area 8

- Therefore& 4ecause of the shift in the distri4ution at the higher te#!erature T9& agreater fraction of !artic%es has the #ini#u# KE to react and hence a greater chanceof a fruitfu% co%%ision ha!!ening i8e8 reactant #o%ecu%e 4onds 4rea ing en route to!roduct for#ation8

- In the diagra#& for the sa e of argu#ent& a te#!erature rise fro# T7 to T9 resu%ts inthe fraction of !artic%es with a KE of L


24/77

The e%%ect o% a catal!st

-

- A cata%,st s!eeds u! a reaction& 4ut it #ust 4e

inCo%Ced che#ica%%,&howeCer te#!orari%, & inso#e wa,& and is continua%%, changed andrefor#ed as the reaction !roceeds8


25/77

- (ata%,sts wor 4, !roCiding an a%ternatiCe reaction !athwa, of %oweractiCation energ,& e8g8 it can assist in endother#ic 4ond 4rea ing!rocesses

- If ,ou consider the KE distri4ution curCe a4oCe& at a fi edte#!erature& the green area shows the #o%ecu%es which haCesufficient KE to react and oCerco#e the actiCation energ, Ea1 forthe un.cata%,sed reaction8

- 3oweCer& in the !resence of a cata%,st & the lower actiCation energ,Ea2 & a%%ows a #uch greater !ro!ortion of the #o%ecu%es to haCeenough energ, to react at the sa#e te#!erature8

- This is shown 4, the co#4ined green area plus the purple area

and this increased fraction of #o%ecu%es increased area$considera4%, increases the chance of a fruitfu% co%%ision %eading to!roduct for#ation& so s!eeding u! of the reaction8

C t l! i


26/77

Catal!sis Catal!st 2 a su4stance that increases the

rate of a reaction and can 4e recoCeredche#ica%%, unchanged at the end of thereaction8

- Kata%is da!at 4e er5a dengan #e#4entusen,awa antara atau #enga4sor!si at,ang direa si an8

' catalyst

%ower the activation energy


27/77

&cti ation energies o% catal!se#reactions

Reaction

""" # H H# +→

Catalyst E a / kJ mol -1

""4 4" H N NH +→

5one

'u

#t

5one

6

!2/

!

! 7

6 HD

7 I9


28/77

ON*ENT)A*I

- Bi%a onsentrasi !erea si di!er4esarda%a# suatu rea si& 4erarti era!atann,a4erta#4ah dan a an #e#!er4an,a

e#ung inan ta4ra an sehingga a an#e#!erce!at %a5u rea si8

- Bi%a !arti e% #a in 4an,a & a i4atn,a %e4ih4an,a e#ung inan !arti e% sa%ing4ertu#4u an ,ang ter5adi da%a# suatu%arutan& sehingga rea si 4erta#4ah ce!at8


29/77

MEKANI*ME )EAK*I

- serang aian rea si taha! de#i taha! ,angter5adi 4erturut.turut se%a#a !roses!eru4ahan rea tan #en5adi !rodu 8


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32/77

- *etia! taha! #e anis#e rea si diatas&#e#!un,ai %a5u tertentu8 Taha! ,ang!a%ing lam"at dise4ut tahap penentu la'ureaksi & aren taha! ini #eru!a an!engha%ang untu %a5u rea si secara

ese%uruhan8


33/77

The )ate E>uation = *toichio#etr,

aA + bB → cC + dD

dt dN

V r A

A!

=− rate of disa!!earance of A

dt dN

V r " "

!= rate of a!!earance of (

d r

cr

$r

ar D" B A ==−=−

)e%ationshi!4etween rates ofreaction

) ) d )


34/77

)eaction )ates and )eaction*toichio#etr,

- oo at the reaction

O 6 g$ NO g$ → NO 9 g$ O9 g$

[ ]

dt

]Od[ +=

dt

]NOd[ +=

dt

d[NO]-=

dt

Od-=rate 223


35/77

Another E a#!%e

9 NO(% g$ → 9 NO 7 (% 9 g$

[ ] dt d[Cl+=dt d[NO]21 =dt NOCld21-=rate2 ]+

WHY? 2 moles of NOCldisappear for every 1 mole Cl 2 formed.


36/77

(onc8 = Te#!8 de!endenc, ter#s

.(.,* tem%co&c f r =

,...(8,*(89*9 B A A " " f ' r =−)eaction rate

constant$(oncentrationde!endent ter#s


37/77

+ersa#aan u#u#2aA 4B 888 ....L gG h3 88888

- the reaction rate can 4e ca%cu%ated 4,2)eaction rate < A # Bn 8888

Dengan2- A & B & etc8 are the concentrations of the reactants is the rate constant or rate coefficient& a Ca%ue

de!endent on te#!erature8 units of < units of rate= units of concentration$ reaction order

- #&n& etc8 are e !onents which corres!ond to a& 4& etc8The concentration is raised to the !ower of its coefficientin the 4a%anced e>uation8

http://www.shodor.org/UNChem/glossary.htmlhttp://www.shodor.org/UNChem/glossary.html


38/77

)ate constant $

,...(8,*9 B A A " " f r =−

Di#ensions Car, with order of reaction n$2&io&co&ce&trat time −− !! (*(*

)eaction order

#o%=#6$

( A

#o%=#6$

#o%=#6$

#o%=#68s$

#o%=#68s$

#o%=#68s$

.r A )ate %aw

#o%=#6$=s r A =− A A " r =−"

A A " r =−

7=s

# 6=#o%$=s

ero

7 st

9nd


39/77

&rrhenius E uation


40/77

Temperature* Rates + the&rrhenius E uation

- ,ne can calculate the rate constant %or a reaction using the&rrhenius e uation-

- A is a constant representing the %raction o% collisions "etweenmolecules ha ing the correct orientation to react when thereactants ha e a concentration o% 1 ./ 0t is generall! not known/

- ut A can "e %actore# out i% one ratios the e uation at twotemperatures/ ,ne t!picall! uses this mo#i%ie# &rrheniuse uation to either calculate E a alues %rom rate constants#eri e# %rom e periments at #i%%erent temperatures* or a rateconstant at a #i%%erent temperature i% one has alrea#!#etermine# E a/

/ E RT a Ak e


41/77

2

1 1 2

2

1

1 2

1 1ln

ln

1 1

a

a

k

k R T T

k R

k

T

E

T

E

÷ ÷

÷


42/77

Problem:

- 3ow much will the rate increase i% a r nhas a E a 4 56k7 an# the temperatureincreases %rom 8669 to :669?

- & reaction has k 4 1/; < 16=> s =1 at;66 9/ When the temperature is

increase# to 566 9 the new measure# k 4 ;/8; < 16=8 s =1/ Calculate the E a alue%or this reaction/


43/77


44/77

E%e#entar, = Non.e%e#entar,)eactions

E%e#entar, reactions F iff stoichio#etric coefficients are the sa#e as theindiCidua% reaction order of each s!ecies

Non.e%e#entar, reactions F stoichio#etr, does not #atch the inetics

D" B A +→+

B A A " " r =−

stoichio#etric coeff2 !==== d c$a

!== β α

B A A " " r "=− "=α

!=β

C ! % l


45/77

Common t!pes o% rate laws-78 @irst Order )eactions - In a first order reaction the rate is !ro!ortiona% to the concentration

of one of the reactants8 That is&v < rate < k B & 7$

- where B is a reactant8 If we haCe a reaction which is nown to 4efirst order in B& such as

B other reactants Q !roducts&- we wou%d write the rate %aw as&

v < rate < k B & 9$- The constant& k & in this rate e>uation is the first order rate constant8

98 *econd Order )eactions - In a second order reaction the rate is !ro!ortiona% to concentration

s>uared8 @or e a#!%e& !ossi4%e second order rate %aws #ight 4ewritten as)ate < k B9 6$

or as)ate < k A B 8 $


46/77

@irst Order )eaction

A → !roduct)ate < C < . d A =d t < A

3ow does the concentration of thereactant de!end on ti#e?

kt A

A

o −=

ln

k has units of s -1


47/77

- 1adi !ersa#aan hu4ungan onsentrasi Adengan wa tu 2

- Atau 4isa din,ata an hu4ungan antaraonCersi dengan wa tu 2

t

A

A e" " −=

t

A A e" " −

=

,

t A A A

e" ) " −=−,, (!*

t

Ae ) −−= !


48/77


49/77


50/77

T @&S 1

- *uatu %arutan A dengan onsentrasi 7g#o%= da%a# reactor 4atch denganCo%u#e %arutan 9&H 4erea si #e#4entuB dengan !ersa#aan rea si A 6B&rea si #eru!a an rea si order 7 dengan

ece!atan rea si rA< (A& dengan ni%ai

< & 9 7=#enit 4era!a onsentrasi A&onCersi A serta onsentrasi B&( #au!un

D sete%ah 6 #enit

The 3a%f %ife of a @irst Order


51/77

The 3a%f.%ife of a @irst Order)eaction

- @or a first order reaction& the ha%f.%ife t 7=9is ca%cu%ated as fo%%ows8

k 6930

t 21.

=


52/77


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54/77

- EXAMPLE: @i en the %ollowing e perimental kinetic #ata* #etermine the kineticrate e pression an# o erall or#er o% reaction/

- 23gCl 2 $ C 2 , : 2= ====== 3g2 Cl 2 $ 2C, 2 $ 2Cl =

- ,ur tentati e rate e pression %or this reaction is- rate 4 k A3gCl 2 B x AC2 , : 2=By

- We nee# to #etermine what the e ponents ( orders ) x an# y are on the reactantconcentrations/ Then we can sol e %or the rate constant k /- Step 1- %in# two e periments where the concentration o% one o% the reactants

sta!s the same/ Since the rate constant k is a constant an# the concentrationo% one o% the components is not changing (also a constant %or this comparison)*we onl! ha e to worr! a"out the one reactant that is changing/

E p A3gCl 2B AC2, :2=

B 0nitial Rate 7 6/16 . 6/1> . 2 16 => 9 6/16 . 6/86 . D 16 =>

6 6/6> . 6/86 . : 16=>


55/77


56/77

Step 2- Repeat %or the other reactantconcentration terms in the rate e uation-

R a t e( e p 2 )

D 1 6= >

: 1 6= >

R a t e( e p 8 )4

4

4

A Be x p # 2 &

A Be x p # 3&

x

x

x

6 / 1 6

6 / 6 >

2 ( 2 ) x 4 1


57/77

ow that we ha e sol e# %or the or#ers o% thekinetic rate e pression* we can write out the

rate e uation-

- rate 4 k A3gCl 2BAC2, : 2=B2

- The overall order o% the rate e pression is thesum o% the in#i i#ual or#ers ( x $ y )- 1 $ 2 4 8/So this is calle# a thir# or#er r n or rate law/

- ote that the or#ers F, ,T correspon# to thecoe%%icients on the chemical e uation/ .an!times the! #o* "ut 'ust as man! times the!wonGt/ There is , H,R.&L C, ECT0, II


58/77

Step 8- Calculate the rate constant (i% aske# %or)/ Wenow 'ust plug in the e perimental #ata %rom an! one o%the e periments an# rearrange an# sol e %or k * the rate

constant/ Hor this e ample we will use the #ata %rome periment 1/

r a t e 2 4 A 3 g C l B A C ,=B2 2 :2k

A 3 g C l B A C ,=B2 2 :2 2k 4

k 4

k 4

r a t e

2 1 6? = >

2 1 6? = >

2 / 2 > 1 6? = 8

k 4 D / D D 1 6? = 8

( 6 / 1 6 . ) ( 6 / 1 > . )2

. s e c= 1

. s e c= 1

. 8

. s e c= 2 = 1

Pro"lem- Consi#er the %ollowing reaction an#


59/77

Pro lem Consi#er the %ollowing reaction an#kinetic #ata/ What is the kinetic rate

e pression? - i(C,) : $ C C3 8 i(C,) 8(C C3 8) $ C,

E p A i(C,) : B AC C3 8B 0nitial Rate(.sec =1)

7 6/6: 6/6; 6/2 16 =>

9 6/6: 6/12 6/2 16 =>

6 6/6D 6/6; 6/: 16=>

6/6D 6/12 6/: 16 =>

P "l C i# h % ll i i #


60/77

Pro"lem- Consi#er the %ollowing reaction an#

kinetic #ata/ What is the rate constant? - C,( g ) $ 3 2 ,( g ) C, 2 (g ) $ 3 2 (g )

E p AC,B A32,B 0nitial Rate (.sec =1)

7 1/> 1/> &99 1/> :/> &

6 8/6 :/> 7&9

1/> 6/5> &7

H 8/6 8/6 &J


61/77


62/77

+seudo.first Order contVd$- *ince the concentration of 3 9 O is

essentia%%, constant

C < (36

I constant< (3 6 I where < 39 O

- The reaction is !seudo first order since ita!!ears to 4e first order& 4ut it is actua%%,a second order !rocess8


63/77

*ing%e = Mu%ti!%e )eactions

*ing%e reaction F 7 e>uation : 7 sing%e rate e>uation

Mu%ti!%e reactions F #ore than 7 rate e>uation needed

*eries reactions2 S * A →→

+ara%%e% reactions2 * B A →+S B * →+

A *

S

* A →S B →

D" B A +→+

co#!etitiCe side 4, side series : !ara%%e%

Physicalh

Reaction


64/77

Chemistry Homogeneous Catalysis

has been set e=ual to !.(

88989989

4" −+= Br O H HOOH ,

dt Od

Kinetics

PhysicalCh i Types of Homogeneous

ReactionKi i


65/77

Chemistry Types of HomogeneousCatalysis

:eterogeneous catalysis normally depends on at least one reactant being adsorbed *usually chemisorbed( and modified to a form inwhich it readily undergoes reaction.

:omogeneous catalysis

'cid catalysis

?ase catalysis

−+ +→+ A H) HA ) reacts

+− +→+ BH ) B )H reacts

[email protected] acid

[email protected] base*many organic reactions(

Autocatalysis


66/77

Chemistry Autocatalysis - A →

x A A −= 8989 x - - += 89898899 - A r =

( )( ) x - x A dt dx +−= 8989

( )( )

++−×+=+− x - x A - A x - x A 89!

89!

8989!

8989!

Antegration by partial fractions, using

( )( )

t x A -

A x - - A

=

−+

+ 89898989ln

8989!

at

at

$e

e - x

+

−=!

!89

(898*9 - A a +=8989

A -

$ =

't what time is the reactionrate a maximumB

Homewo

rk No. 1


67/77

Chemistry Unimolecular Reactions#he $indemann-%inshel&ood 'echanism


68/77



69/77


89898989

"4

"4!C4 A

A A dt - d +== >

898989

"

4! A A

dt - d ==

"

4!

=

4" 89 A


70/77

Chemistry mpro!ements of theTheory

!!(' 'echanism


71/77


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KATA I* 3ETE)OGEN


76/77

KATA I* 3ETE)OGEN-

Ban,a %oga# ,ang da!at #engi at cu u!4an,a #o%e u%.#o%e u% gas !ada!er#u ann,a& #isa%n,a Ni& +t& +d dan X8 Ga,atari #enari antara ato# %oga# dengan#o%e u% gas da!at #e#!er%e#ah i atan oCa%en!ada #o%e u% gas& dan 4ah an da!at#e#utus an i atan itu8 A i4atn,a #o%e u% gas,ang terad4or!si !ada !er#u aan %oga# ini#en5adi %e4ih rea tif dari!ada #o%e u% gas ,angtida tera4sor4si8 +rinsi! ini ada%ah er5a dari

ata%is heterogen& ,ang 4an,a di#anfaat anuntu #eng ata%isis rea si.rea si gas8

)EAK*I KATA I*


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)EAK*I KATA I*- at A dan at B ,ang direa si an #e#4entu at AB

dengan at ( se4agai ata%is8 AB A B YYF rea si %a#4at$- Bi%a tan!a ata%is di!er%u an energi !enga tifan ,ang

tinggi dan ter4entu n,a AB %a#4at8 Na#un& denganadan,a A( rea si ce!at$8 ata%is (& #a a ter5adi%ah

rea si2 A (Y- Energi !enga tifan diturun an& A( ter4entu ce!at danse eti a itu 5uga A( 4erea si dengan B #e#4entusen,awa AB(8

A( B AB( re YYa si ce!at$

- Energi !enga tifan rea si ini rendah sehingga dengance!at ter4entu AB( ,ang e#udian #engurai #en5adi AB dan (8

AB AB( YYF ( rea si ce!at$

KINETIKA REAKSI-

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