Cha pte r 15: Phe no me na he re a c tio n A(a q ) + B(a q ) C(a q - - PowerPoint PPT Presentation

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Cha pte r 15: Phe no me na

Phe no me na : T he re a c tio n A(a q ) + B(a q )  C(a q ) wa s studie d a t two diffe re nt te mpe ra ture s (298 K a nd 350 K ). F

• r e a c h te mpe ra ture the re a c tio n wa s sta rte d

b y putting diffe re nt c o nc e ntra tio ns o f the 3 spe c ie s tha t ta ke pa rt in the re a c tio n into a n o the rwise e mpty c o nta ine r. T he re a c tio n ra te wa s the n me a sure d. Wha t pa tte rns do yo u no tic e a b o ut the re a c tio n ra te s? Ca n re a c tio n ra te s b e pre dic te d?

Da ta T a ke n a t 298 K E xp. [A] [B] [C] Ra te

1 1 M 1 M 1 M 10

• 2

1 M 0 M 1 M

• 3

1 M 1 M 0 M 10

• 4

0 M 1 M 1 M

• 5

1 M 2 M 1 M 10

• 6

1 M 3 M 0 M 10

• 7

2 M 1 M 1 M 40

• 8

4 M 1 M 1 M 160

• 9

2 M 2 M 2 M 40

• 10

0.5 M 6 M 3 M

Da ta T a ke n a t 350 K E xp. [A] [B] [C] Ra te

1 1 M 1 M 1 M 200

• 2

1 M 0 M 1 M

• 3

1 M 1 M 0 M 200

• 4

0 M 1 M 1 M

• 5

1 M 2 M 1 M 200

• 6

1 M 3 M 0 M 200

• 7

2 M 1 M 1 M 800

• 8

4 M 1 M 1 M 3200

• 9

2 M 2 M 2 M 800

• 10

0.50 M 6 M 3 M

Cha pte r 15 Che mic a l K ine tic s

• T

he rmo Re vie w

• Re a c tio n Ra te s
• Ra te L

a ws

• Co nc e ntra tio n a nd

T ime

• Re a c tio n Me c ha nisms
• E

xpla ining Re a c tio n Ra te F a c to rs

2

Big Ide a : T

he ra te s o f c he mic a l re a c tio ns a re de sc rib e d b y simple e xpre ssio ns tha t a llo w us to pre dic t the c o mpo sitio n o f a re a c tio n mixture a t a nytime . T he se e xpre ssio ns a lso sug g e st the ste ps in whic h the re a c tio ns ta ke s pla c e .

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Ra te s

 Ca ta lyst: A sub sta nc e

tha t inc re a se s the re a c tio n ra te witho ut b e ing c o nsume d in the re a c tio n.

 Homog e ne ous Ca ta lyst:

A c a ta lyst tha t is in the sa me pha se a s the re a c ta nts.

 He te rog e ne ous Ca ta lyst:

A c a ta lyst tha t is in a diffe re nt pha se tha n the re a c ta nts.

3

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Ra te s

 Re a c tion Ra te s: T

he c ha ng e in c o nc e ntra tio n o f

• ne o f the re a c ta nts o r pro duc ts divide d b y the

time inte rva l o ve r whic h the c ha ng e ta ke s pla c e .

4

R  P

Ave rage Rate o f Co nsumptio n o f R:

∆ ∆

No Note: Rates are always positive, therefore, since the reactants are consumed, a negative sign must be added to make the rate positive.

Ave rage Rate o f Pro duc tio n o f P:

∆ ∆

U nique Ave rage Rate (U AR)



1

• ∆

∆ 1

• ∆

∆ 1

• ∆

∆

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Ra te s

Insta nta ne ous Ra te of Re a c tion

 T

he b e st a ppro xima tio n to the ra te a t a sing le insta nt is o b ta ine d b y dra wing a line ta ng e nt to the plo t o f the c o nc e ntra tio n a g a inst time . T he slo pe o f the ta ng e nt line is c a lle d the insta nta ne o us ra te o f the re a c tio n.

5

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

Ra te L

a w: An e q ua tio n e xpre ssing the

insta nta ne o us re a c tio n ra te in te rms o f the c o nc e ntra tio ns, a t a ny insta nt, o f the sub sta nc e s ta king pa rt in the re a c tio n.

 …

6

No Note: k is the rate constant and x ,y, … are the orders of reaction. No Note: This form of the rate law is called the differential rate law. No Note: The units of rate are always

• , therefore, the units of k will

differ depending on the overall reaction order.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

T hing s to know a bout the ra te la w:

 Ra te la ws c a n c o nta in pro duc ts, re a c ta nts,

c a ta lysts b ut usua lly o nly sta rting ma te ria l.

 Ra te la ws do no t c o nta in inte rme dia te s.  Ra te la ws c a n ONL

Y b e de te rmine d e xpe rime nta lly.

 Orde rs do NOT

c o rre la te with c o e ffic ie nts in b a la nc e d e q ua tio n!

 Orde rs c a n b e a n inte g e rs, ze ro s, fra c tio ns,

po sitive s, OR ne g a tive s!

 E

a c h spe c ie s ha s its o wn individua l re a c tio n

• rde r.

 T

he o ve ra ll re a c tio n o rde r is the sum o f the individua l o rde rs fo und in the re a c tio n.

7

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

How to find the units of k

Ste p 1: De te rmine the o rde r o f the

re a c tio n

Ste p 2: Sub tra c t 1 fro m the o ve ra ll o rde r Ste p 3: F

ind

• #

·

8

Ex Examples amples for rate=k[A][B]: Overall order 2 Ex Examples amples for rate=k[A][B]: 1 Ex Examples amples for rate=k[A][B]: 1

• ·
• ·

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Orde r 0th 1st 2nd

time Initia l Conc e n- tra tion Ra te L a w

Ra te L a ws

9 0 10 20 30 0 10 20 30 0 0.3 0.6 0.9

Ra te

0 2 4 6 0 2 4 6 0 2 4 6

[A]

0 2 4 6 0 10 20 30

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

De te rmine the ra te la w: A + B + C  2D

1)

Ge ne ra l Ra te L a w:

2)

Orde r with re spe c t to A:

3)

Orde r with re spe c t to B:

4)

Orde r with re spe c t to C:

10

E xpe rime nt [A]o (M) [B]o (M) [C]o (M) Initia l Ra te (

· )

1 1 6 4 20 2 2 6 2 80 3 2 3 2 40 4 1 6 2 20

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

De te rmine the ra te la w a nd k fo r

 2A + B  2C

11

E xpe rime nt [A]o (M) [B]o (M) Initia l Ra te (

· )

1 0.050 0.10 0.074 2 0.10 0.20 0.888 3 0.050 0.20 0.222

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

De te rmining Orde r (long wa y)

 Ste p 1: F

ind two e xpe rime nts in whic h the c o nc e ntra tio ns o f e ve rything , e xc e pt o ne spe c ie s, is he ld c o nsta nt.

 Ste p 2: Divide the ra te la ws fo r the se two

e xpe rime nts b y e a c h o the r.

 Ste p 3: So lve fo r o rde r.

12

No Note: This will cancel out k and all other variables except for the order that you are trying to determine. Math No Math Note: It is sometimes useful to take the log of both sides of the equation. The log(xy)=ylog(x). Math No Math Note:

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Student Question

Ra te L a ws

T he ra te la w fo r the fo llo wing re a c tio n 2NO(g ) +O 2(g )  2NO 2(g ) wa s e xpe rime nta lly fo und to b e in the fo rm ra te =k[NO]x[O 2]y I t wa s a lso fo und tha t whe n the NO c o nc e ntra tio n wa s do ub le d, the ra te o f the re a c tio n inc re a se s b y a fa c to r o f 4. I n a dditio n, whe n b o th the O 2 a nd the NO c o nc e ntra tio n we re do ub le d, the ra te inc re a se s b y a fa c to r o f 8. Wha t is the re a c tio n

• rde r o f O 2?

a ) 0th b ) 1st c ) 2nd d) 3rd e ) No ne o f the a b o ve

13

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Ra te L a ws

De te rmine the ra te la w a nd k fo r

 A + B  2C  Pse udo Orde r Re a c tion: A re a c tio n in whic h

the ra te la w c a n b e simplifie d b e c a use a ll b ut

• ne o f the spe c ie s ha ve virtua lly c o nsta nt

c o nc e ntra tio ns.

14

E xpe rime nt [A]o (M) [B]o (M) Initia l Ra te (

· )

1 5.0 0.010 5.0 2 5.0 0.020 10.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

Ze ro Orde r Inte g ra te d Ra te L

a w

15

k Rate  ) 1

   

 

 

t A A

dt k dA ) 4



   

A kt A   



kdt dA   ) 3 k dt dA   ) 2



  const x dx

   

kt A A   



) 5

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

F

irst Orde r Inte g ra te d Ra te L a w

16

 

kdt dA A   1 ) 3

   

kt A A   



ln ln ) 5

   

ln ln A kt A   



 

A k dt dA   ) 2

 

A k Rate  ) 1



  const x dx x ln 1

 

   

 

 

t A A

dt k dA A 1 ) 4



Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

Se c ond Orde r Inte g ra te d Ra te L

a w

17

 

kdt dA A  

2

1 ) 3

   

kt A A    



1 1 ) 5

   

1 1 kt A A  



 

2

) 2 A k dt dA  

 

2

) 1 A k Rate 



   const x dx x 1 1

2

 

   

 

 

t A A

dt k dA A

2

1 ) 4



Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

T

he ra te la w fo r A+B  C + D wa s o nly fo und to b e de pe nde nt o n A. Using the fo llo wing da ta de te rmine the ra te la w a nd k.

18

T ime (s) [A] (M)

5.4 20. 0.15 40. 0.077 60. 0.052

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

19

1 2 3 4 5 6 20 40 60 80

[A] T ime

• 4
• 3
• 2
• 1

1 2 20 40 60 80

ln[A] T ime

5 10 15 20 25 20 40 60 80

[A]^- 1 T ime

T ime

(s)

[A]

(M) 5.4 20. 0.15 40. 0.077 60. 0.052

ln[A]

1.7

• 1.9
• 2.6
• 3.0

[A]- 1

(M

• 1

)

0.19 6.7 13 19

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

Ca lc ula te the c o nc e ntra tio n o f N2O a fte r the first o rde r de c o mpo sitio n: 2N2O(g )  2N2(g ) + O 2(g ). T he ra te o f de c o mpo sitio n o f N2O = k[N2O]. T he re a c tio n ha s c o ntinue d a t 780ºC fo r

• 100. ms, a nd the initia l c o nc e ntra tio n o f

N2O wa s 0.20 M a nd k = 3.4

.

20

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

 Ha lf L

ife : T

ime it ta ke s fo r the c o nc e ntra tio n to dro p to ha lf the initia l a mo unt

21

0th Orde r

   

A kt A   

 

12

2 A t k 



     



A A kt ln ln 2

1 2 1

  

   

A A

2 1



 

A kt

2 1 2 1

  

1st Orde r

   

A kt A ln ln   

 

12

ln 2 t k 

   



A kt A   

2 1 2 1

     



A kt A ln ln

2 1 2 1

  

   

 

 

 

2 ln ln ln

2 1 2 1

2 1

    

 

A A

kt

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

22

2nd Orde r

   

A kt A 1 1  

 

12

1 t k A 



   



A kt A 1 1

2 1 2 1

 

     

 

A A A kt 1 1 2

2 1

  

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Co nc e ntra tio n a nd T ime

23

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Me c ha nisms

Re a c tion Me c ha nism: T

he ste ps b y whic h a re a c tio n ta ke s pla c e .

E

le me nta ry Re a c tion: One o f the

re a c tio n ste ps in a n o ve ra ll re a c tio n.

24

No Note: RATE LAWS CAN BE DETERMINED FROM ELEMENTARY REACTIONS. No Note: In order to be a valid mechanism the sum of the elementary reactions must equal the overall reaction.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Me c ha nisms

Me c ha nism 1:

E le me nta ry Re a c tio n(s):

Me c ha nism 2:

E le me nta ry Re a c tio n(s):

25

No Note: Different elementary reactions usually give different rates. No Note: In order to be a valid mechanism the rate law derived from the elementary reactions must match the experimentally determined rate law.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Me c ha nisms

Re a c tion Inte rme dia te : A spe c ie s tha t

pla ys a ro le in the re a c tio n b ut do e s no t a ppe a r in the re a c tio n.

Mole c ula rity: T

he numb e r o f re a c ta nt mo le c ule s/ a to ms ta king pa rt in a n e le me nta ry re a c tio n.

26

Ex Examples amples: → Molecularity of 1 → 2 Molecularity of 2

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Student Question

Re a c tio n Me c ha nisms

Use the e xpe rime nta lly fo und ra te la ws g ive n b e lo w to de te rmine whic h re a c tio n is mo st like ly to o c c ur in a sing le ste p.

a )

2NO 2(g )+F

2(g )2NO 2F

(g )

• b )

H

2(g )+Br 2(g )2HBr(g )

⁄

c )

2NO(g )+2O 2(g )2NO 2(g ) + O 2(g )

d)

NO 2(g )+CO(g ) NO(g ) + CO 2(g )

27

E xpe rime nta lly F

• und Ra te L

a ws

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Student Question

Re a c tio n Me c ha nisms

Co nside r the fo llo wing hypo the tic a l re a c tio n: A + 2B  E . T he me c ha nism fo r this re a c tio n is: (1) A + B  C (slo w) (2) B + C  D (fa st) (3) D  E (fa st) T he ra te la w c o nsiste nt with this me c ha nism is:

a ) ra te =k[A][B] b ) ra te =k[A]2[B] c ) ra te =k[A]2 d) ra te =k[A][B]2 e ) No ne o f the a b o ve

28

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Student Question

Re a c tio n Me c ha nisms

T he re a c tio n 2NO + Cl

2  2NOCl wa s e xpe rime nta lly

fo und to ha ve the ra te la w: ra te = k[Cl

2][NO]2. Whic h

me c ha nism c o uld not b e the c o rre c t me c ha nism?

a )

Cl

2 ⇌ 2Cl (fast e quilibrium)

2Cl + 2NO  2NOCl (slo w)

b )

2NO + 2Cl

2  2NOCl 2 (slo w)

2NOCl

2 ⇌ NOCl 3+NOCl (fast e quilibrium)

NOCl

3 ⇌ NOCl + Cl 2 (fast e quilibrium)

c )

2NO + Cl

2  2NOCl

d)

2NO ⇌ N2O 2 (fast e quilibrium) N2O 2 + Cl

2  2NOCl (slo w)

e )

All o f the a b o ve a re po ssib le me c ha nisms

29

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Me c ha nisms

E quilibrium Consta nt

• Ra te Consta nt
• 30

    

1 1

C k K A B k  

1 1

k K k 

 Re la ting the Ra te a nd E

quilibrium Consta nts

A+B

• ⇌
• C

At E q uilib rium (Ra te fo rwa rd = Ra te re ve rse)

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Re a c tio n Me c ha nisms

Multi Ste p Re a c tions With Unknown Spe e ds

 Ste p 1: Write a n e xpre ssio n fo r the ra te o f

fo rma tio n o f o ne o f the fina l pro duc ts (so me time s the pro duc t o f inte re st is spe c ifie d). I f po ssib le se le c t a pro duc t tha t is o nly in 1 ste p.

 Ste p 2: Use the ste a dy sta te a ppro xima tio n to

so lve fo r the c o nc e ntra tio n o f inte rme dia te s.

 Ste p 3: Plug b a c k into o ve ra ll ra te e q ua tio n.

31

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

Student Question

E xpla ining Re a c tio n Ra te F a c to rs

T he ra te c o nsta nt fo r the se c o nd-o rde r g a s- pha se re a c tio n HO(g ) + H

2(g )  H 2O(g ) + H(g )

va rie s with the te mpe ra ture a s sho wn he re : De te rmine the a c tiva tio n e ne rg y. a ) 2.4×10-5

• b ) 4.0×103
• c ) 4.2×104
• d) No ne o f the a b o ve

32

T e mpe ra ture (K) Ra te Consta nt (

· )

373 1.1×10-9 473 1.8×10-8 573 1.2×10-8 673 4.4×10-7

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

E xpla ining Re a c tio n Ra te F a c to rs

Collision T he ory (Ga se s Only)

 Ra te = Co llisio n F

re q ue nc y × F ra c tio n with Suffic ie nt E ne rg y

33

How would we g e t c ollision fre que nc y

 Size o f the mo le c ule s/ a to ms  Ave ra g e ve lo c ity o f the

mo le c ule s/ a to ms

 Co nc e ntra tio n o f mo le c ule s/ a to ms

How would we g e t fra c tion with suffic ie nt e ne rg y?

 Bo ltzma nn distrib utio n  4

• ⁄

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

E xpla ining Re a c tio n Ra te F a c to rs

 Proble m: Altho ug h the ra te ha s the rig ht fo rm

(Arrhe nius) it pre dic ts a la rg e r re a c tio n ra te tha n is fo und.

 Solution: Ste ric s ne e d to b e ta ke n into a c c o unt.

34

• E

a = Minimum e ne rg y

ne e de d fo r re a c tio n to o c c ur. A = T a ke s into a c c o unt numb e r o f c o llisio ns a nd ste ric s.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

E xpla ining Re a c tio n Ra te F a c to rs

Ac tiva te d Co mple x T

he o ry (So lutio ns)

35

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

T a ke Awa y F ro m Cha pte r 15

 Big Ide a : T

he ra te s o f c he mic a l re a c tio ns a re de sc rib e d b y simple e xpre ssio ns tha t a llo w us to pre dic t the c o mpo sitio n o f a re a c tio n mixture a t a nytime . T he se e xpre ssio ns a lso sug g e st the ste ps in whic h the re a c tio ns ta ke s pla c e .

 T

he rmo Re vie w

 K

no w the diffe re nc e b e twe e n the rmo a nd kine tic s

 T

he rmo dyna mic s a llo ws us to pre dic t if a re a c tio n will o c c ur.

 K

ine tic s a llo ws us to pre dic t ho w fa st a re a c tio n will o c c ur.

 Be a b le to dra w re a c tio n c o o rdina te s a lo ng with la b e ling

re a c ta nts, pro duc ts, inte rme dia te s, tra nsitio n sta te s, a nd a c tiva tio n e ne rg y. (87,88)

 Re a c tion Ra te s

 Be a b le to e xpla in ho w a c a ta lyst c a n inc re a se re a c tio n ra te .

(90)

36

Numb e rs c o rre spo nd to e nd o f c ha pte r q ue stio ns.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

T a ke Awa y F ro m Cha pte r 15

 Re a c tion Ra te s (Co ntinue d)

 Be a b le to c a lc ula te the a ve ra g e ra te o f re a c tio n o f 1 spe c ie s

g ive n the a ve ra g e ra te o f re a c tio n o f a no the r spe c ie s.

 Be a b le to c a lc ula te the uniq ue a ve ra g e ra te o f a re a c tio n.

 Ra te L

a w

 K

no w tha t ra te la ws must b e de te rmine d e xpe rime nta lly.

 Be a b le to de te rmine the o rde r o f a re a c tio n a nd e a c h

individua l spe c ie s.

 Be a b le to c a lc ula te ra te la w fro m e xpe rime nta l da ta . (18,19,

20,21,22,23)

 Do ub le c o nc e ntra tio n a nd ra te sta ys the sa me : 0th o rde r  Do ub le c o nc e ntra tio n a nd ra te do ub le s: 1st o rde r  Do ub le c o nc e ntra tio n a nd ra te q ua druple s: 2nd o rde r  I

f no ne o f the se use the ma th tric k

 Be a b le to de te rmine the units o f the ra te c o nsta nt (14,15)  T

he units o f c o nc e ntra tio n a re c o nsta nt (M)

 T

he units o f ra te a re c o nsta nts

• ·

37

Numb e rs c o rre spo nd to e nd o f c ha pte r q ue stio ns.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

T a ke Awa y F ro m Cha pte r 15

 Ra te L

a w (Co ntinue d)

 K

no w tha t ra te pro b le ms c a n b e simplifie d whe n the c o nc e ntra tio n o f 1 spe c ie s is hig h a nd e sse ntia lly unc ha ng ing (pse udo o rde r re a c tio ns). (36,39,54)

 Conc e ntra tion a nd T

ime

 Be a b le to use the inte g ra te d ra te la w to pe rfo rm c a lc ula tio ns.

(43,47,48,52)

 0th o rde r: °  1st o rde r: ln °  2nd o rde r:

°

 Be a b le to ide ntify the o rde r o f the re a c tio n b y plo tting da ta .

(30,31,32,33,35,38)

 [A] vs. t line a r 0th o rde r, slo pe = -k  ln[A] vs. t line a r 1st o rde r, slo pe = -k  [A]-1 vs. t line a r 2nd o rde r, slo pe = k  Be a b le to c a lc ula te ha lf-life / 2nd ha lf-life / e tc ..

38

Numb e rs c o rre spo nd to e nd o f c ha pte r q ue stio ns.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

T a ke Awa y F ro m Cha pte r 15

 Re a c tion Me c ha nisms (56)

 Be a b le to write a ra te la w o f a n e le me nta ry re a c tio n. (59)  Be a b le to de te rmine the ra te la w o f multi ste p re a c tio ns.

(60,61)

 Be a b le to e limina te inte rme dia te s fro m multi ste p re a c tio ns.  E

q uilib rium (63,65,68)

 Ste a dy sta te a ppro xima tio n (69,70)

 E

xpla ining Re a c tion Ra te F a c tors

 Co nc e ntra tio n  Ca ta lyst (94)  Be a b le to dra w po te ntia l e ne rg y dia g ra m o f re a c tio ns  T

e mpe ra ture

 K

no w tha t mo st re a c tio ns fo llo w Arrhe nius b e ha vio r. (8,72,79,80,81,84,86)



• 

ln

• ln
• 39

Numb e rs c o rre spo nd to e nd o f c ha pte r q ue stio ns.

Chapt Chapter 1 r 15: : Chemic Chemical Kine Kinetic tics

T a ke Awa y F ro m Cha pte r 15

 E

xpla ining Re a c tion Ra te F a c tors (c ontinue d)

 Surfa c e Are a  K

no w the ide a s b e hind c o llisio n the o ry (g a se s).

 K

no w the ide a s b e hind a c tiva te d c o mple x the o ry (so lutio ns).

40

Numb e rs c o rre spo nd to e nd o f c ha pte r q ue stio ns.