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International Journal of
Thermodynamics &
Chemical Kinetics
Jul–Dec 2016
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Manisha Dhoble
EDITORIAL BOARD MEMBERS
Dr. Chang-Yu SunState Key Laboratory of Heavy Oil Processing
China University of PetroleumBeijing, China
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Bundelkhand University India
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University, Visakhapatnam, India
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K. R. Puram Bangalore, India
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Department of Materials Science and Engineering National Taiwan University of
Science and Technology, Taiwan
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Azad National Institute of Technology, Bhopal, India
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Kalamassery, Kochi, Kerala, India
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Nehru National Institute of Technology (MNNIT), Allahabad, U. P., India
Dr. Niki Sweta JhaNational Institute of Technology (NIT)
Patna, Bihar, India
Dr. Ajaya Kumar SinghDepartment of Chemistry (DST-FIST
Sponsored) Govt. V. Y. T. PG. Autonomous College, Chhattisgarh, India
Dr. Vidyavathi A. ShastryDepartment of Chemistry, SEA College of Engineering & Technology, K. R. Puram,
Bangalore, India
Dr. Sandeep RaiDepartment of Chemistry/Polymer and Rubber,
Shroff S.R. Rotary Institute of Chemical Technology, Vataria, Ankleshwar, India
Dr. Kishore DasariNavin Fluorine International Limited,
India
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Ramakrishna RaoDepartment of Chemistry, GITAM School of Technology, GITAM University, Bangalore,
Karnataka, India
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Engineering College, Lakhanpur Sarguja University Ambikapur, Chattisgarh, India
Shaista AliDepartment of Chemistry, GC University,
Lahore, Punjab, India
EDITORIAL BOARD MEMBERS
Ranganathan SubramanianDepartment of Chemistry, Indian Institute of
Technology, Patna, Bihar, India
Dr. Annapurna NowduriDepartment of Engineering Chemistry, A. U.
College of Engineering (Autonomous), Andhra University,Visakhapatnam, Andhra Pradesh,
India
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University, Chennai, Tamil Nadu, India
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of Technology, Osmania University, Hyderabad, Andhra Pradesh, India
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University, Amritsar, Punjab, India
Dr. Suranani SrinathDepartment of Chemical Engineering,
National Institute of Technology, Warangal,Andhra Pradesh, India
From the Editor's Desk
Dear Readers,
We would like to present, with great pleasure, the inaugural volume of a new scholarly
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kinetics etc.
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It is our hope that this fine collection of articles will be a valuable resource for Thermodynamics and
Chemical Kinetics readers and will stimulate further research into the vibrant area of Thermodynamics and
Chemical Kinetics.
Puneet Mehrotra
Managing Director
1. The Decomposition of Tris-(Oxalato)-Manganate (III) Complex Ion as the Reaction Suitable for the Laboratory Practice on Chemical Kinetics Pavel Anatolyevich Nikolaychuk, Mariya Mikhaylovna Vayner 1
2. Kinetics and Mechanisms of the Reduction of Some Carbonyl Compounds with Sodium Dithionite in Aqueous Alkaline MediumP.O. Ukoha, F.N. Okafor 11
3. Kinetic and Mechanistic Study of Oxidation of Benzydamine Hydrochloride by Permanganate (VII) in Acidic MediumV. Shastry, B.C. Sateesh, S. Shashidhar, T.N. Padmini, K.S. Ravindra 20
4. A Note on: Thermodynamics in Our Daily LifeZeanut Akoijam 29
5. Chemical Composition in Atmosphere: An Introductory Approach for StudentsAmit Agnihotri 31
Contents
IJTCK (2016) 1–10 © JournalsPub 2016. All Rights Reserved Page 1
International Journal of Thermodynamics and Chemical Kinetics Vol. 2: Issue 2
www.journalspub.com
The Decomposition of Tris-(Oxalato)-Manganate (III) Complex
Ion as the Reaction Suitable for the Laboratory Practice on
Chemical Kinetics
Pavel Anatolyevich Nikolaychuk*, Mariya Mikhaylovna Vayner
Kafedra Analitičeskoj i Fizičeskoj Himii, Čelâbinskij Gosudarstvennyj Universitet, Brat'ev Kaširinyh,
Chelyabinsk, Russian Federation
ABSTRACT
The complex ion 3
2 4 3[Mn(C O ) ] is very photosensitive and rapidly decomposes at the
daylight even at ambient temperatures. Although the mechanism of this reaction is
complicated, its kinetic equation obeys the pseudo-first order. In addition, the tris-(oxalate)-
manganate ion has a low thermal stability, and the reaction of its decomposition is highly
affected by temperature. This makes this reaction very suitable for demonstrating the laws of
chemical kinetics to the students – both the first-order reaction kinetics and the dependency
of the rate constant on temperature. The kinetic studies of this reaction using a
photocolourimetric method were performed; the influence of the initial concentrations of the
reagents and temperature on the rate was studied. The didactic implementation of the
reaction was discussed. The methodical instruction for the organization of the laboratory
practice is provided.
Keywords: activation energy, Arrhenius equation, chemical kinetics, decomposition, first-
order reaction
INTRODUCTION
Complex compounds of manganese (III)
with various ligands have a very high
chemical reactivity. The redox chemistry
of Mn+3
is very diverse and was studied
thoroughly.[1–4]
One of such species of
interest is the complex of tervalent
manganese with oxalate-ion. A tris-
(oxalate)-manganate (III) complex ion is
formed in a solution according to the
reaction[5,6]
:
(1)
or in ionic form:
(2)
IJTCK (2016) 11-19 © JournalsPub 2016. All Rights Reserved Page 11
International Journal of Thermodynamics and Chemical Kinetics Vol. 2: Issue 2
www.journalspub.com
Kinetics and Mechanisms of the Reduction of Some Carbonyl
Compounds with Sodium Dithionite in Aqueous Alkaline Medium
P.O. Ukoha, F.N. Okafor*
Department of Pure and Industrial Chemistry, University of Nigeria, Nsukka, Enugu State, Nigeria
ABSTRACT
Kinetics of the reduction of some carbonyl compounds (acetophenone, benzophenone,
benzaldehyde, and salicylaldehyde) with sodium dithionite was studied at 28± 0.5oC and
basic concentration in the range of 0.01 to 0.05 mol dm-3
(NaHCO3). Under these conditions,
the reaction rates were found to be first order with respect to sodium dithionite as plot of log
kobs versus log [S2O42-
] showed linearity to about 95% extent of reaction, however, the
overall reaction rate was second order at constant [OH-]. Furthermore, order of reactions
with respect to acetophenone, benzophenone, salicylaldehyde, and benzaldehyde was unity as
the plot of log(A∞-At) versus time showed about 90% linearity. Reaction rates increased with
ionic strength and addition of chloride ions of varying concentration. Michaelis–Menten plot
of 1/kobs versus 1/[S2O42-
] were linear and have small intercepts on y-axis. Increase in pH
(from 1-13) also showed remarkable increase in the reaction rates. Kinetic investigations
showed that an outer-sphere reaction mechanism was operational and plausible mechanisms
have been proposed for these reactions.
The rate laws for the reactions conform to the equations:
Rate = {k3K1 + k2 [OH-]
2} [S2O4
2-] [RCHO]
where RCHO = benzaldehyde and salicylaldehyde
Rate = {k3K1 + k2 [OH-]
2} [S2O4
2-] [RCOR
1]
where RCOR1
= benzophenone and acetophenone
Keywords: carbonyl compounds, dithionite ions, kinetics, mechanism, reduction
INTRODUCTION
Over the years, a lot of interests have been
devoted to the study of redox reactions
using sodium dithionite[1–3]
due to its
strong reducing ability, the kinetic study of
these redox processes have also been
shown[4]
but not to a large extent.
Dithionite ion is used to reduce carbonyls
to their corresponding alcohols,[5]
and the
reduction, monitored kinetically.[6]
It is a
white crystalline powder with a weak
sulfurous odor,[7]
readily available
inexpensive reducing agent that is capable
of reducing a variety of functional groups
e.g. nitro, nitroso, oximes, aldehydes,
ketones, diazonium salts, imines and
haloketones.[8]
Its reducing power is
known to be generally enhanced in basic
pH.[9]
Though stable under most
conditions, it gets decomposed in hot
water and acidic solutions.[10]
It produces
sulphonyl anion, SO2- by reversible
dissociation;
(1)
This anion is a stronger reducing agent
than S2O42-
as shown by its redox
potential.[11]
Redox reactions of dithionite
IJTCK (2016) 20–28 © JournalsPub 2016. All Rights Reserved Page 20
International Journal of Thermodynamics and Chemical Kinetics Vol. 2: Issue 2
www.journalspub.com
Kinetic and Mechanistic Study of Oxidation of Benzydamine
Hydrochloride by Permanganate (VII) in Acidic Medium
V. Shastry1*, B.C. Sateesh
2, S. Shashidhar
1, T.N. Padmini
3, K.S. Ravindra
1
1Department of Chemistry, South East Asian College of Engineering & Technology, Bangalore, India
2Department of Chemistry, Shri Pillappa College of Engineering, Bangalore, India
3Department of Chemistry, Shri Krishna Institute of Technology, Bangalore, India
ABSTRACT
The kinetics and mechanism of Permanganate (Mn (VII)) oxidation of Benzydamine
hydrochloride (B.HCl) in acidic medium has been studied at 26 ± 0.1°C. The reaction shows
first order dependence in [Mn (VII)], less than unit order in [B.HCl] and fractional order
dependence in [H2SO4]. Variation of ionic strength by the addition of KCl has no significant
effect on the rate. The stoichiometry of the reaction is found to be 1:4 and the main oxidative
products were toluene, dimethyl aza propionic acid and benzoic acid. A mechanism involving
formation of complex has been proposed and the reaction constants involved in the different
steps of mechanism are calculated. Activation parameters with respect to slow step of the
mechanism are calculated and tabulated. The rate constant of reaction is found to be 1.960 ×
10−3
s-1
.
Keywords: benzydamine hydrochloride, oxidation, potassium permanganate
INTRODUCTION
The nonsteroidal anti-inflammatory drug,
Benzydamine hydrochloride (B.HCl)
shows local anaesthetic and analgesic
action by stabilizing the cellular membrane
and inhibiting prostaglandin synthesis.[1]
Benzydamine hydrochloride has a
tendency of increasing therapeutic effect;
hence it is used as an adjunct to other
therapy.
It is also used in the treatment of Strains,
Bursitis, Sprains, Synovitis, Myalgice,
Tendinitis and Periathritis
(musculoskeletal disorders).[2]
Benzydamine shows prominent invitro
antibacterial activity and also shows
synergic property in combination with
many antibiotics especially tetracyclines,
against antibiotic resistance strains of
Staphylococcus aureas and Pseudomonas
aeruginosa (Figure 1).[3,4]
N
NO N
CH3
CH3
Fig. 1. Structure of benzydamine.
In general anti-inflammatory drugs are
organic acids but benzydamine is a base
and available as its hydrochloride salt.
Benzydamine is fluorescent (exeitation
306nm: emission 362nm) and is detected
fluorometrically in HPLC assay. In over
dosage it acts as deliriant and CNS
stimulant.[5]
Potassium permanganate [Mn (VII)] will
oxidize a wide variety of inorganic and
IJTCK (2016) 29–30 © JournalsPub 2016. All Rights Reserved Page 29
International Journal of Thermodynamics and Chemical Kinetics Vol. 2: Issue 2
www.journalspub.com
A Note on: Thermodynamics in Our Daily Life
Zeanut Akoijam* Department of Chemistry, Manipur University, Manipur, India
ABSTRACT
Thermodynamics plays crucial role in our day-to-day life. Almost all the activities that we do
or observe are all based on the principles of thermodynamics. Here, some of the common
routine activities are brought into limelight that is explained by the phenomenon of
thermodynamics.
Keywords: energy, entropy, heat transfer, thermodynamics
BACKGROUND
Thermodynamics is the field of science
that deals with relationships between heat,
work and energy. The term
thermodynamics is actually a combination
of two words viz., thermo (meaning
thermal energy or heat) + dynamics
(meaning study of forces or motion). This
field of science involves various cyclic
transformations between heat and energy.
Because of this, some define
thermodynamics as the study of energy
and its various interconversions from one
to another form [1]. It is applicable to
various scientific fields including physics,
biology and chemistry. Scientists argue
that everything that occurs in our day-to-
day activities like the driving of vehicles
(cars, motorbikes, airplanes, ships), jet-
engines, spark-ignition engines etc., is
entirely because of thermodynamics.
The study of thermodynamics is based on
different laws: first law of
thermodynamics, second law of
thermodynamics and third law of
thermodynamics. Also, there is the zeroth
law of thermodynamics, Boyle’s law,
Charles law etc., which explains numerous
activities occurring in nature. The first law
of thermodynamics states that the total
energy always remains conserved. It
means that the energy can neither be
created nor destroyed but can only be
converted from one form to another [2, 3].
The second law is the law of entropy.
According to this, systems always try to
maintain their state of thermodynamic
equilibrium. Also, referred as the state of
maximum entropy, second law of
thermodynamics describes that the heat
energy flows from a state of low
temperature to a state of higher
temperature. The topic of entropy is
further extended to the third law of
thermodynamics. It states that at
temperature of absolute zero, entropy
remains zero. Absolute zero is the
temperature at which the motion of an
average atom or an average molecule is
zero [2, 3]. Several examples of our daily
activities can be described on the basis of
these laws. These are [2–4]:
All types of vehicles that we used to
see running on-roads every day, such
as cars, motorbikes, trucks, or those
that fly in air i.e., aeroplanes, or the
ships that run on water; all work on the
basis of the second law of
thermodynamics.
IJTCK (2016) 31-32 © JournalsPub 2016. All Rights Reserved Page 31
International Journal of Thermodynamics and Chemical Kinetics Vol. 2: Issue 2
www.journalspub.com
Chemical Composition in Atmosphere: An Introductory
Approach for Students
Amit Agnihotri Department of Chemical Engineering, ITM, Gwalior, India
Our atmosphere is divided into different
strata above the earth’s surface. The
region closest to earth’s surface is the
troposphere that is extended upto 10–16
km above the surface. This layer or strata
is followed by stratosphere which extends
upto nearly 50 km.[1]
Above it is the
mesosphere region, which covers about
50–85 km from surface of the earth.
Beyond the mesosphere lies the
thermosphere which goes from 85–500
km away from the earth’s surface.[1]
The chemical composition in these layers
varies considerably and so does the
chemical reactions.
Fundamentally, atoms in the lithosphere
undergo reduction reaction over time,
while those in upper atmosphere are more
prone to be oxidized. This is because
atmospheric density decreases as we move
up from ground level. Higher density at
ground level means that there is more
number of molecules available per unit
volume of gas to interact with each other.
Also, the temperature of gaseous
substances transforms from room
temperature to very cold and then to very
hot and then very cold while moving from
surface of the earth towards thermosphere.
During this, the entire composition of gas
change. The gaseous molecules experience
change in their velocity and hence kinetic
energy and undergo several collisions
amongst each other.[2]
This is why we find
stable molecules at the surface and highly
charged atoms or ions at the top (towards
thermosphere).
Troposphere largely consists of gases viz.,
nitrogen and oxygen, carbon dioxide, and
water vapor. Oxides of nitrogen and
Sulphur, methane and some other trace
gases are also found in this layer. The
stratospheric region consists of less dense
composition and is more exposed to
radiation from the Sun. The molecules of
this region therefore have more velocity
and kinetic energy. The composition is
rich in nitrogen and their oxides, oxygen,
and ozone.[2,3]
The third layer above the ground level is
the mesosphere which consists of ions of
molecules that were found in the layer
beneath it i.e., stratosphere. This layer
receives intense solar radiation and
therefore the molecules here get ionized
and exist as small ionized molecules,
positive ions and electrons.
The topmost layer, thermosphere, receives
even more intense radiations of the Sun.
The molecules exist as mixture of highly
charged ions and atoms.
Chemical reactions in the atmospheric
layers can occur in any forms: gas phase
collisions between the molecules, surfaces
of particulate matter or in water droplets
(aqueous phase).[1]
As we move away from the earth’s
surface, there is variation in the altitude,
pressure and temperature. As we go up,
temperature decreases till the end of
troposphere, after which it begins to
increase as the stratosphere arrives. With
the further rise in altitude, temperature
Mechanical Engineering
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Architecture
Office No-4, 1 Floor, CSC, Pocket-E,Mayur Vihar, Phase-2, New Delhi-110091, India
E-mail: [email protected]
¬ International Journal of Thermal Energy andApplications
¬ International Journal of Production Engineering¬ International Journal of Industrial Engineering
and Design¬ International Journal of Manufacturing and
Materials Processing¬ International Journal of Mechanical Handling and
Automation
« International Journal of Radio Frequency Design« International Journal of VLSI Design and Technology« International Journal of Embedded Systems and Emerging
Technologies« International Journal of Digital Electronics« International Journal of Digital Communication and Analog
Signals
« International Journal of Housing and Human SettlementPlanning
« International Journal of Architecture and InfrastructurePlanning
« International Journal of Rural and Regional PlanningDevelopment
« International Journal of Town Planning and Management
Applied Mechanics
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