This document discusses catalysis and provides definitions and examples of various types of catalysis. It defines catalysis as a process that increases the rate of a chemical reaction by adding a substance called a catalyst, which is not consumed in the reaction and can catalyze multiple reactions. It then describes the main types of catalysis as positive and negative catalysis, homogeneous and heterogeneous catalysis, autocatalysis, and enzyme catalysis. It provides examples and brief explanations of each type. Finally, it discusses two theories of catalysis - the intermediate compound theory and the adsorption theory.
CATALYSIS, TYPES OF CATALYSIS FOR CHEMISTRY STUDENTSShikha Popali
CATALYSIS IS A TYPE OF CHEMICAL REACTION. HERE IN THIS PREASENTATION THE CATALYSIS AND ITS TYPES ARE EXPLAINED IN DETAIL WITH ITS ADVANTAGES AND DISADVANTAGES.
Introduction
Basis
Importance
Classification
Homogeneous catalysis
Mechanism
Example
Heterogeneous catalysis
Mechanism
Examples
Promoters
Catalytic Poisoning
Autocatalysis
Enzyme catalysis
Enzymes
References
Catalyst: -
The substances that alter the rate of a reaction but itself remains chemically unchanged at the end of the reaction is called a Catalyst.
The process is called Catalysis.
prop-
A catalyst cannot start the reaction by itself.
Catalytic activity increases as surface area of catalyst increases.
Catalysts are thermolabile, this effect is very well pronounced in enzymes.
Catalytic activity is maximum at a catalyst’s optimum temperature.
A catalyst does not alter the position of the equilibrium, instead it helps in achieving the equilibrium faster.
Catalysis and its Types
Homogeneous Catalysis
Advantages of Homogeneous Catalysis
History of Homogeneous Catalytic Reactions
Examples of Homogeneous Catalytic Reactions
CATALYSIS, TYPES OF CATALYSIS FOR CHEMISTRY STUDENTSShikha Popali
CATALYSIS IS A TYPE OF CHEMICAL REACTION. HERE IN THIS PREASENTATION THE CATALYSIS AND ITS TYPES ARE EXPLAINED IN DETAIL WITH ITS ADVANTAGES AND DISADVANTAGES.
Introduction
Basis
Importance
Classification
Homogeneous catalysis
Mechanism
Example
Heterogeneous catalysis
Mechanism
Examples
Promoters
Catalytic Poisoning
Autocatalysis
Enzyme catalysis
Enzymes
References
Catalyst: -
The substances that alter the rate of a reaction but itself remains chemically unchanged at the end of the reaction is called a Catalyst.
The process is called Catalysis.
prop-
A catalyst cannot start the reaction by itself.
Catalytic activity increases as surface area of catalyst increases.
Catalysts are thermolabile, this effect is very well pronounced in enzymes.
Catalytic activity is maximum at a catalyst’s optimum temperature.
A catalyst does not alter the position of the equilibrium, instead it helps in achieving the equilibrium faster.
Catalysis and its Types
Homogeneous Catalysis
Advantages of Homogeneous Catalysis
History of Homogeneous Catalytic Reactions
Examples of Homogeneous Catalytic Reactions
KINETICS OF ESTERIFICATION REACTION USING ION-EXCHANGE RESIN CATALYSTJournal For Research
The reaction kinetics of esterification between n-butanol and acetic acid on acidic solid catalyst named SERALITE SRC-120 under atmospheric pressure was investigated in this work. Reaction experiments were carried out in a stirred batch reactor at temperature range of 353 to 356 K, under various catalyst loads and various starting reactants feed ratios. The experimental data were fitted to estimate the kinetic parameters for reaction mechanisms. The chemical equilibrium composition was measured and kinetic information was obtained at the same temperature range. The results show that the activation energy of n-butanol esterification reaction was found to be 622.28 KJ/mol. Finally the results of produced reaction mechanisms were compared with Experimental results to validate the reaction mechanism. Then it was conclude that the model results with the regressed kinetic parameters are in excellent agreement with the experimental results.
Phase Transfer Catalysis and Ionic liquids Gopika M G
Mechanism of Phase Transfer Catalysis, Examples of Phase Transfer Catalysts, Catalysis by Ionic Liquids, Examples of Ionic Liquids, Reactions involving Ionic Liquids.
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Environmental Catalysis Module: Students examines different types of catalytic systems, including heterogeneous and homogeneous catalysis. Depending on the knowledge they gained during activities, the students are then asked to design their projects.
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The Roman Empire A Historical Colossus.pdfkaushalkr1407
The Roman Empire, a vast and enduring power, stands as one of history's most remarkable civilizations, leaving an indelible imprint on the world. It emerged from the Roman Republic, transitioning into an imperial powerhouse under the leadership of Augustus Caesar in 27 BCE. This transformation marked the beginning of an era defined by unprecedented territorial expansion, architectural marvels, and profound cultural influence.
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Under Augustus, the empire experienced the Pax Romana, a 200-year period of relative peace and stability. Augustus reformed the military, established efficient administrative systems, and initiated grand construction projects. The empire's borders expanded, encompassing territories from Britain to Egypt and from Spain to the Euphrates. Roman legions, renowned for their discipline and engineering prowess, secured and maintained these vast territories, building roads, fortifications, and cities that facilitated control and integration.
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Read| The latest issue of The Challenger is here! We are thrilled to announce that our school paper has qualified for the NATIONAL SCHOOLS PRESS CONFERENCE (NSPC) 2024. Thank you for your unwavering support and trust. Dive into the stories that made us stand out!
1. CATALYSIS Dr. V. Sreeja,
Assistant Professor of Chemistry,
TKMM College Nangiarkulangara,
Alappuzha, Kerala, India
2. CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
CONTENTS
1
2
3
4
5
WHAT IS CATALYSIS?
TYPTES OF CATALYSIS
CHARACTERISTICS OF
CATALYTIC REACTIONS
THEORIES OF CATALYSIS
ENZYME CATALYSIS
3. WHAT IS CATALYSIS?
Catalysis is the process of increasing the rate of a chemical reaction by adding a
substance known as a catalyst, which is not consumed in the catalyzed reaction and
can continue to act repeatedly.
A substance that alters the reaction rate of a chemical reaction chemically unchanged at the end of
the reaction
CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
4. TYPTES OF CATALYSIS
TYPES OF CATALYSIS
POSITIVE
CATALYSIS
NEGATIVE
CATALYSIS
HOMOGENEOUS
CATALYSIS
HETROGENEOUS
CATALYSIS
BIOCATALYSIS
AUTO-CATALYSIS
CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
5. POSITIVE CATALYSIS
The catalyst which increases the rate of a chemical reaction is called positive
catalyst and the phenomenon is known as positive catalysis
Examples
(j) 2KClO3 2KCl + 3O2
(ii) H2O2 H2O + [O]
MnO2
Pt
The catalyst which decreases the rate of reaction is called negative catalyst and
phenomenon is called negative catalysis.
Example
(j) H2O2 H2O + [O]
NAGATIVE CATALYSIS
Acetanilide
CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
6. HOMOGENIOUS CATALYSIS
CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
Homogeneous catalysis refers to reactions where the catalyst is in the same phase as the
reactants, principally in solution
e.g. 2SO2 (g) + O2 (g) 2SO3
NO(g)
HETEROGENIOUS CATALYSIS
The catalytic process in which the reactants and the catalyst are in different
phases is known as heterogeneous catalysis
e.g. 2SO2 (g) + O2 (g) 2SO3
Pt(s)
8. CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
AUTO-CATALYSIS
In certain reactions, one of the product acts as a catalyst. In the initial stages the reaction
is slow but as soon as the products come into existences the reaction rate increases. This
type of phenomenon is known as auto- catalysis
Example
The rate of oxidation of oxalic acid by acidified potassium permanganate increases as the
reaction progresses. This acceleration is due to the presence of ions which are formed
during reaction. Thus ions act as auto-catalyst.
5H2C2O4 + 2KMnO4 + 3H2SO4 2MnSO4 + K2SO4 + 10CO2 + 8H2O
2MnO4- + 16H+ + 5C2O4
2- 2Mn2+ + 8H2O+ I0CO2
9. CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
ENZYME CATALYSIS
Numerous reactions occur in the bodies of animals and plants to maintain the life
process. These reactions are catalysed by enzymes. The enzymes are thus,
termed as bio-chemical catalysts and the phenomenon is known as bio-chemical
catalysis
C12 H22O11 + H2O C6 H12O6 + C6 H12O6
Invertase
10. CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
CHARACTERISTICS OF CATALYTIC REACTIONS
1
6
5
4
3
2
A catalyst remains unchanged in mass and chemical
composition at the end of the reaction
A small quantity of the catalyst is generally
sufficient to catalyzes almost unlimited
reactions
The catalyst can not initiate the reaction
The catalyst can not change the position of
equilibrium
The catalyst is generally specific in nature
Change of temperature alters the rate of chemical
reaction
11. CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
THEORIES OF CATALYSIS
Intermediate compound formation theory
Adsorption theory
INTERMEDIATE COMPOUND THEORY OF CATALYSIS
According to this theory, the catalyst reacts with one of the reactants to give
an intermediate, which reacts with another reactant to yield products and the
catalyst
12. CATALYSIS & PHOTOCHEMISTRY Dr. V. Sreeja
A + B AB
A + C AC (Intermediate compound)
AC + B AB + C
(Product) (Catalyst)
Example:
2SO2 (g) + O2 (g) 2SO3
2NO + O2 2NO2
2NO2 + 2SO2 2SO3 + 2NO
(C)
