MECHANISM OF PROPANE-BUTANE FRACTION DECOMPOSITION PROCESS INTO LOW MOLECULAR SATURATED AND UNSATURATED HYDROCARBONS

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A

BSTRACT

The decomposition of propane-butane fractions into low molecular weight saturated and unsaturated
hydrocarbons is a key process in petrochemical production. This study explores the kinetic parameters
and reaction mechanisms using reactors designed for impulse and continuous flow operations. The results
indicate that the decomposition reactions follow first-order kinetics under specific experimental
conditions. Conducted at temperatures ranging from 400°C to 700°C with catalysts, the experiments reveal
that the process occurs at two distinct active catalytic sites (Z and Z). The mechanism involves the
formation of surface radical complexes (C-Z), which govern the reaction pathways. Depending on the
stability of these complexes, the process proceeds through either sequential hydrogen detachment, leading
to carbon formation on the catalyst surface, or hydrogen recombination from the gas phase with the C-Z
complex, resulting in methane production. This study provides valuable insights into the decomposition
mechanisms of propane-butane fractions and lays the groundwork for optimizing catalytic processes to
enhance the yield of desired low molecular weight hydrocarbons.

K

EYWORDS

Propane-butane fractions, hydrocarbon decomposition, catalytic process, kinetic parameters, active
catalytic sites, surface radical complexes, first-order kinetics, methane formation, carbon deposition,
impulse reactors, continuous flow reactors, petrochemical production.

Journal

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Copyright:

Original

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Research Article

MECHANISM OF PROPANE-BUTANE FRACTION
DECOMPOSITION PROCESS INTO LOW MOLECULAR
SATURATED AND UNSATURATED HYDROCARBONS

Submission Date:

December 15,

2024,

Accepted Date:

December 20, 2024,

Published Date:

December 30, 2024

Crossref doi:

https://doi.org/10.37547/ijasr-04-12-52

Sanjar H. Saidqulov

Laboratory Assistant, Department of Polymer Chemistry and Chemical Technologies, Institute of
Biochemistry, Samarkand State University named after Sharof Rashidov, Samarkand, Uzbekistan

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336-348

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I

NTRODUCTION

Unsaturated hydrocarbons of the ethylene series

are among the most critical products in primary

organic synthesis. They serve as key

intermediates in numerous organic synthesis

processes and form the foundation for producing

high-tonnage polymers [1

–

7]. Products derived

from these hydrocarbons are widely utilized

across various branches of the chemical industry.

One of the primary industrial applications of light

unsaturated ethylene hydrocarbons, such as

ethylene and propylene, is the production of

polyethene and polypropylene, as well as their

oxides. Due to the rapid growth in the demand for
ethylene and propylene, there is a constant search

for reliable sources of inexpensive raw materials

and more efficient production technologies [8

–

14].

The primary industrial method for producing

propylene involves the thermal decomposition of

liquid hydrocarbon raw materials, such as

naphtha. However, the predominant product of

naphtha

thermal

cracking

is

ethylene.

Additionally, a growing share of global ethylene

production comes from the thermal cracking of

ethane, which is derived from natural gas. This

shift highlights the increasing urgency to develop

targeted processes for producing propylene from

more affordable and accessible gas-based raw

materials [15

–

19].

Breaking carbon-carbon bonds in light alkanes

through homogeneous selective oxidation is

considered a promising direction for the

development of targeted propylene production

processes [20

–

27]. Catalytic oxidation of carbon-

carbon bonds offers significant advantages over

non-catalytic methods [28

–

31]. Interestingly, the

potential for enhancing propane’s thermal

decomposition efficiency by adding unsaturated

compounds like ethylene has not been

extensively studied [32

–

38]. Experimental results

show that during the co-oxidation of propane and

ethylene, the yield of propylene significantly

increases compared to the oxidation of propane

alone [39

–

43].

This process can be organized to enable a highly

efficient direct production of propylene from

propane. These findings suggest a promising

potential method for producing propylene and

other unsaturated hydrocarbons of the ethylene

series [44

–

47].

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VOLUME

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Experimental part

According to the theory of thermal decomposition

of hydrocarbons, the decomposition of saturated

hydrocarbons under the influence of heat in the

absence of air and propane-butane mixture under

the influence of high temperature in the absence

of air with the presence of a reactor designed to

carry out the process of breaking the C

–

C and C

–

H bonds corresponds to the process.

For kinetic studies, the use of reactors designed

for the implementation of a pulsed process
determines that the equation for determining the

kinetic parameters is applicable only for first-

order reactions (valid for the ideal displacement

regime).

When calculating the abstract rate constant of the

decomposition of hydrocarbon raw materials in

the reactor, the following formula (1) was used

for the ideal compression mode of products into

the reaction zone in the reactor designed for the
process with the pulsed introduction of raw

materials and the reactor designed for the flow

process.

1

1

1

,

1

ef

i

k

ln

c

x



−

=

−

(1)

Here,

𝑥

𝑖

−

is the degree of modification of the

initial hydrocarbon,

τ

–

is the contact time determined by the ratio of

the volume of the reactor designed for the

implementation of the process and the volume

velocity of the flow passing through the reactor

designed for the implementation of the process.

The thermal effect of the reaction of the

decomposition reaction with the breaking of C

–

C

and C

–

H bonds in the absence of air and under the

influence of heat and the propane-butane mixture
under the influence of high temperature in the

absence of air was determined according to the

following formula (2):

3

290.5(

6 8

1

) 2

.

i

i

H

x



+

=

−

(2)

Here,

i

x

is the degree of modification of the initial

hydrocarbon.

The activation energy was estimated from the

experimental data using the least squares method

(3). For this, the Arrhenius equation was used in
logarithmic form:

ef

а

ef

E

lnk

lnA

RT

=

−

(3)

where A is an old-exponential multiplier;

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ef

а

E

- effective activation energy;

R

is the universal gas constant (8.31 J/mol∙K).

Solving the problem of linear regression in

coordinates -

1

ef

lnk

Т

−

, A and

ef

а

E

R

parameters

found.

R

ESULTS AND

D

ISCUSSION

Development of a physicochemical model of

the pyrolysis process.

To explain the observed

changes in hydrogen and methane concentrations

in the reaction products, it is necessary to have an

idea about its intermediate stages, which take

place in the presence of active centres in a catalyst

with high catalytic activity and productivity.

Based on the obtained experimental data, it can

be assumed that the decomposition of
hydrocarbons in the presence of catalysts in the

temperature range of 400-700

℃

occurs in two

types (Z and Z) of active catalytic centres. This

process is observed by the formation of surface

radical complexes C-Z. Depending on the

dominance of the resulting C-Z (active centre -

carbon), either the sequential separation of
hydrogen atoms through the formation of carbon

on the surface of the catalytic particle or the

joining of active hydrogen atoms from the gas

phase to C-Z with the formation of methane can

occur. Decomposition of hydrocarbons can occur

due to the breaking of C-C bonds with the

formation of CH

x

complexes on the surface of

catalyst particles. In the same work, it was shown
that subsequent dehydrogenation of surface CH

x

complexes can lead to the formation of hydrogen

and carbon. The hypothesis of two different types

of active sites present on the surface of a catalyst

with high catalytic activity and productivity is

stated for the first time in the present thesis work.

Depending on the strength of C-Z (active centre -

carbon) bonds, two parallel (competitive)

processes can occur in C-Z complexes. With the
formation of carbon on the surface of the catalytic

particles in the Z centres with stronger C-Z bonds,

sequential separation of hydrogen atoms occurs

in the gas phase:

3

2

2

•

•

•

•

•

•

•

•

• •

Z CH

Z CH

Н

Z CH

Z CH

Н Z C

Z

C

Z CH

Z C

Н

→

+

→

+

→

+

→

+

The carbon formed on the surface of the catalytic

particle dissolves in its volume and separates on

the opposite side according to the carbide cycle

mechanism. Molecular hydrogen is formed by the

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interaction of active hydrogen atoms with each

other or with the initial hydrocarbon molecules:

3

8

2

3

7

2

•

•

• •

Н

С Н

Н

С Н

Н

Н

Н

+

→

+

+

→

At Z centres with less strong C-Z bonds, hydrogen

atoms can bond to form methane from the gas

phase:

2

2

3

3

3

8

4

3

7

3

4

•

•

•

•

•

•

•

•

•

•

Z CH

Н

Z CH

Z CH

Н

Z CH

Z CH

С Н

Z

СН

С Н

Z CH

Н

Z

CH

+

→

+

→

+

→

+

+

+

→

+

So, the total reaction looks like this:

3

8

4

2

2

2

С Н

С

СН

Н

→

+

+

The proposed scheme of the catalytic reaction is

confirmed by the evidence that nickel catalysts

with high catalytic activity and productivity are

the most active for methanation reactions. It is for

this reason that the selectivity of the process of

propane to hydrogen conversion is strongly

dependent on the degree of deactivation of the

catalyst with high catalytic activity and

productivity during the reaction.

Decay of propane into lower molecular

saturated and unsaturated hydrocarbons

with the breaking of C

–

C and C

–

H bonds.

Figure

1 shows the experimental results obtained in a
laboratory

reactor

with

a

volumetric

consumption of hydrocarbons of 1 l/h on the

composition of propane decomposition reaction

products without the presence of a catalyst with

high catalytic activity and productivity. The

temperature must be much higher than 700

℃

to

obtain much higher concentrations of hydrogen
by breaking down the thermal C

–

C and C

–

H bonds

of propane into lower molecular saturated and

unsaturated hydrocarbons.

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Picture 1. Temperature dependence of the concentrations of the decomposition products into lower

molecular saturated and unsaturated hydrocarbons with the breaking of S3N8 thermal C

–

C and C

–

H

bonds in a laboratory reactor

When alkanes break down into lower molecular

saturated and unsaturated hydrocarbons with

the breaking of C

–

C and C

–

H bonds, the initial

formation of the chain occurs due to the breaking

of CC bonds, which are more blunt than S-N bonds

in the gas phase.

The process of thermal decomposition of propane

(Fig. 1) can be described by the following

simplified scheme. Initially, under the influence of

temperature, with the formation of primary free

radicals (chain initiation), the breaking of the CC

bond occurs:

3

8

3

2

5

•

•

С Н

СН

С Н

→

+

Resistant to decomposition, but extremely

reactive methyl (-

СН

3

) and ethyl (-

С

2

Н

5

) radicals

react with the initial molecules of propane,
removing a hydrogen atom from them:

2

5

3

8

2

6

3

7

3

3

8

4

3

7

•

•

•

•

С Н

С Н

С Н

С Н

СН

С Н

СН

С Н

+

→

+

+

→

+

As a result, methane, ethylene and propyl radicals

(-

С

3

Н

7

) are formed. Large, relatively unstable

radicals spontaneously form more stable methyl
radicals (-

СН

3

) and ethylene molecules (when C-

C bonds are broken) or hydrogen atoms (-N) and

propylene molecules (when C-H bonds are

broken) according to the β

-rule decomposes with:

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3

7

2

4

3

3

7

3

6

•

•

•

•

С Н

С Н

СН

С Н

С Н

Н

→

+

→

+

For the ethyl radical, decomposition according to

the β

-rule is impossible, this radical can

decompose with the separation of a hydrogen

atom and the formation of ethylene:

2

5

2

4

•

•

С Н

С Н

Н

→

+

Atomic hydrogen, in turn, is reduced to molecular

hydrogen by removing another hydrogen atom

from the original propane molecule:

3

8

2

3

7

•

•

Н

С Н

Н

С Н

+

→

+

There is also the possibility of interaction of

hydrogen atoms with each other or with methyl

radicals (radical recombination) with the

formation of molecular hydrogen and methane:

2

3

4

• •

• •

Н

Н

Н

Н

СН

СН

+

→

+

→

In the disproportionation reaction of methyl and
ethyl radicals, the formation of methane along

with ethylene is not an exception:

3

2

5

4

2

4

•

•

СН

С Н

СН

С Н

+

→

+

Thus, at the time of low feedstock in the reactor,

with the breaking of thermal C

–

C and C

–

H bonds

of propane, decomposition into lower molecular

saturated and unsaturated hydrocarbons occurs

with the formation of hydrogen, methane,

ethylene and small amounts of ethane and

ethylene in the gas phase. The mechanism of

hydrogen formation includes several stages. The

process of methane formation goes parallel to the
hydrogen formation process. It should be noted

that at temperatures above 600

℃

, with the

breaking of the thermal C

–

C and C

–

H bonds of

propane, during decomposition into lower

molecular

saturated

and

unsaturated

hydrocarbons, pyro-carbons begin to separate

from the gas phase, which settles in the form of
solids on the walls of the reactor. After the

experiments, the inner surface of the reactor is

completely covered with pyro-carbon.

Degradation of normal butane into lower

molecular

saturated

and

unsaturated

hydrocarbons with the breaking of C

–

C and C

–

H bonds.

Similar results were obtained in the

study of the thermal decomposition of butane

under the same conditions. As in the case of
propane, the products of the decomposition

reaction of butane are hydrogen, methane,

ethylene, ethylene and propylene. The curve of

the change of propylene concentration will have a

similar appearance as for the decomposition of

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propane into lower molecular saturated and

unsaturated hydrocarbons with the breaking of

C

–

C and C

–

H bonds. The difference is that the

decomposition of the butane molecule begins at a

lower temperature (450

℃

) with the formation of

hydrogen and propylene. The concentration of

ethylene also exceeds the concentration of ethane

in all considered ranges of temperatures. The

concentration, however, is low and does not

exceed 11 vol.% even at 750

℃

.

Figure 2. Temperature dependence of the concentrations of the decomposition products of n-butane

into lower molecular saturated and unsaturated hydrocarbons with the breaking of thermal C

–

C and

C

–

H bonds in a laboratory reactor

The distribution of butane cracking reaction

products depicted in Fig. 2 can also be explained
following the rules of the theory of the radical-

chain mechanism of hydrocarbon decomposition

mentioned above. Initially, primarily free radicals

are formed due to the breaking of C-C bonds in the

weakest place (methyl, ethyl and propyl):

4

10

2

5

2

5

4

10

3

3

7

•

•

•

•

С Н

С Н

С Н

С Н

СН

С Н

→

+

→

+

Then the process develops in two possible

directions. Unstable propyl radicals decompose
to form more stable methyl and ethyl radicals or

hydrogen atoms and the corresponding

molecules of alkenes according to the reactions

described above. Free methyl and ethyl radicals

and active hydrogen atoms interact with the

original butane molecules and remove hydrogen

atoms from them, resulting in the formation of

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hydrogen, methane, ethane and secondary butyl

(-

С

4

Н

9

) radicals:

3

4

10

4

4

9

2

5

4

10

2

6

4

9

4

10

2

4

9

•

•

•

•

•

•

СН

С Н

СН

С Н

С Н

С Н

С Н

С Н

Н

С Н

Н

С Н

+

→

+

+

→

+

+

→

+

Butyl radicals, being more unstable than propyl

radicals, can cleave both through C-C and through

C-H bonds. In the first case, methyl and ethyl

radicals are formed together with ethylene and

propylene, and in the second case - hydrogen

atoms and butylene molecules:

4

9

2

4

2

5

4

9

3

6

3

4

9

4

8

•

•

•

•

•

•

С Н

С Н

С Н

С Н

С Н

СН

С Н

С Н

Н

→

+

→

+

→

+

Since butylene was not detected in the reaction
products (Fig. 2), it can be suggested that the

•С

4

Н

9

→ С

4

Н

8

+• Н

reaction almost does not occur,

because the butyl radicals were mainly

decomposed by the much weaker C-C bond under

these conditions. Indeed, in butyl radicals, the

homolysis energy of the C-H bond (364 kJ/mol)

significantly exceeds the homolysis energy of the
C-C bond (264 kJ/mol).

C

ONCLUSIONS

Thus, at the time of low feedstock in the reactor,
with the breaking of thermal C

–

C and C

–

H bonds

of propane, decomposition into lower molecular
saturated and unsaturated hydrocarbons occurs
with the formation of hydrogen, methane,
ethylene and small amounts of ethane and
ethylene in the gas phase. The mechanism of
hydrogen formation includes several stages. The
process of methane formation goes parallel to the
hydrogen formation process. It should be noted
that at temperatures above 600

℃

, with the

breaking of the thermal C

–

C and C

–

H bonds of

propane, during decomposition into lower
molecular

saturated

and

unsaturated

hydrocarbons, pyro-carbons begin to separate
from the gas phase, which settles in the form of
solids on the walls of the reactor. After the
experiments, the inner surface of the reactor is
completely covered with pyro-carbon.

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