Hydrogen Peroxide Decomposition- Batch1

8/19/2019 Hydrogen Peroxide Decomposition- Batch1

1/13

CHP 305

PROCESS CONTROL AND REACTION ENGINEERING

LABORATORY

CRE 3: To determine the kineti! o" the h#dro$en

%ero&ide deom%o!ition in ' ('th re'tor)

S*(mitted B#:

Yash Kumar Bhati 2012BB50048Atul Verma 2012BB50012


2/13

Aim: To determine the kinetics of the hydroen !ero"ide decom!osition in a #atch

reactor$

A!!aratus: %&necked round #ottom flask' condenser' as (olume measurin unit at

atmos!heric !ressure' constant tem!erature #ath' thermometer' sto!)atch$

*hemicals: +ydroen !ero"ide' ,otassium iodide$

Theory and calculations:

-eaction : 2+2.2 2+2. / .2

A B .

t is re!orted that the reaction is irre(ersi#le and first order$

The rate e3uation #ecomes'

&d*Adt K$*A

nteratin and sol(in for *A' )e et

*A*Ao$ e&Kt

6rom the e"!ression' the ra!h #et)een *A and t )ill #e e"!onential in nature$

7o) calculations from the e"!erimental data:

nitial concentration of the hydroen !ero"ide solution:

*+2.2 V.292 224009V+2.2 m moleml

These are the m moles of hydroen !ero"ide in 1 ml of the sam!le$

o concentration of hydroen !ero"ide in the initial reaction mi"ture is:

*Ao *+2.2 9V+2.2 V+2. / V+2.2

The concentration of hydroen !ero"ide in the reaction mi"ture at any i(en time

is i(en #y:

*A V; < Vt V; 9 *Ao

=here Vt is the (olume of o"yen li#erated at any time t$


3/13

*alculatin (alues from a#o(e relations:

At tem!erature T4%$4 deree and usin +2.2 (olume %ml

V.2 250 ml

V+2.23 ml

*+2.2 0.0074

*Ao 0.00022

t

vt

v*-

vt

v*-

vt/v*

Ca

0 0 250 1 0.00022

8 25 225 0.9

0.00019

8

13 50 200 0.8

0.00017

6

15 70 180 0.72

0.00015

84

20 110 140 0.56

0.00012

32

25 140 110 0.44

0.00009

68

30 165 85 0.34

0.00007

48

35 190 60 0.24

0.00005

28

40 210 40 0.16

0.00003

52

50 230 20 0.08

0.00001

76

60 250 0 0 0

,lottin Vt (s t


4/13

,lottin *A (s t$

imilarly calculatin (alues at Tem!erature T 4%$4 deree and 5ml +2.2 (olume

V.2 420 ml

V+2.2 5 ml

*+2.2 0.0075


5/13

*Ao 0.00036


6/13

To determine the rate constant of the reaction

=e ha(e seen that

*A*Ao$ e&Kt

o *A*Ao e&Kt

Takin lo on #oth sides' )e et>

&ln*A*Ao Kt

o on !lottin this cur(e the slo!e of the line )ill i(e rate constant$

*alculatin *A*Ao (alues$

At tem!erature T4%$4 deree and % ml +2.2 (olume


7/13

,lottin &ln*A*Ao (s t$

lo!e 2$52&0$1 50 &8

0$05?


8/13

imilarly for T4%$4 deree and 5ml +2.2$

,lottin &ln*A*Ao (s t$

lo!e : 1$?@&0$18 24&8

0$1


9/13

To determine the order of reaction

The rate e3uation'

&d*Adt K$*An

Takin lo on #oth sides>

=e et>

ln&d*Adt lnk/nln*A

o a !lot #et)een ln&d*Adt and ln*A )ill cur(e )hose slo!e )ill #e e3ual to

the order of the reaction$

*alculation for T4%$4 deree and (olume 0f +2.2 % ml

T *a &d*adt ln*a ln&d*adt

15

0.000158

4 8.8E-06

8.750387

08

11.64075

88

20

0.000123

2

0.000007

04

9.001701

51

11.86390

24

25

0.000096

8

0.000005

28

9.242863

56

12.15158

45

30

0.000074

8

0.000004

4

9.500692

67

12.33390

6

35

0.000052

8

0.000004

4

9.848999

37

12.33390

6

40

0.000035

2

0.000003

52

10.25446

45

12.55704

96

50

0.000017

6

0.000001

76

10.94761

17

13.25019

67


10/13

lo!e of ra!h :1%$25&11$410$@4&8$?5

1$12$1@

0$?%

imilarly calculatin for T4%$4 deree 5ml +2.2$

T *a &d*adt ln*a ln&d*adt

8

0.0003

04

1.39286

E-05

7.929406

527

11.181

57

11

0.0002

53

1.71429

E-05

8.097543

448

10.973

93

150.0001

81.82143

E-058.282685

88110.913

3

18

0.0001

33

1.57143

E-05

8.622553

707

11.060

94

22

7.71E-

05

1.39286

E-05

8.926236

121

11.181

57

24

0.0000

6

8.57143

E-06

9.469851

567

11.667

08

28

1.71E-

05

1.07143

E-05

9.721165

996

11.443

93


11/13

30 0

8.57143

E-06

10.97392

896

11.667

08

lo!e of ra!h :

11$? < 10$@1 @$4?&8$28

0$?1$1@

0$4


12/13

Results

• 6rom the !lots of *A (s t )e see that the nature of the cur(es is

e"!onential in nature )hich is in accordance )ith the rate

e3uationtheory$

• 6rom the !lots of &ln*A*Ao (s t the slo!e of the cur(es are:

lo!e T%4$ de 0$05?

lo!e T44 de 0$1

o rate constant (alues:

K T%4$'e"!erimental 0$05?

K T44$0'e"!erimental 0$1

• 6rom the !lots of ln&d*Adt (s ln*A

lo!e T%4$ de 0$?%

lo!e T44 de 0$4

o order of reaction:

n T%4$ 0$?%n T44 0$4


13/13

ources of error:

• The tu#e drainin the )ater out of the o(erflo) lass #ottle must #e

shaken at reular inter(als to ensure !ro!er drainae of the )ater and

no air #lockae$

• Tem!erature of the reaction must #e kee! at an o!timum le(el say

around %5&40 de$$ o)er tem!eratures )ould retard the reaction rate

and hiher tem!erature )ould enhance the reaction rate to such an

e"tent that the initial rates are too difficult to measure$ =hen the

reaction rate is ma"imum$

• The three )ay sto! cock must #e !ro!erly closed to ensure !ro!er

trans!ort of o"yen$

S'"et# %re'*tion!:

As e(en traces of alkali e$$ leachin from lass can initiate decom!osition' +2.2is stored in )a"&coated #ottles' or !lastic containers' )ith the addition of a

sta#iliCer e$$ urea$ D(en a trace of dust can lead to e"!losi(e decom!osition$ The

handlin of the )ater&free com!ound' or concentrated solutions thereof' should

therefore #e carried out under dust&free conditions and )ith the e"clusion of metal

ions$

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Hydrogen Peroxide Decomposition- Batch1