Chemical kinetics deals with the study of reaction rates and their mechanisms. The rate of a reaction depends on factors like concentration, temperature, pressure, and presence of a catalyst. Rate laws relate the rate of reaction to the concentrations of reactants. The rate law is determined experimentally and cannot be predicted from the balanced chemical equation alone. Integrated rate laws allow determination of reaction order based on plots of concentration versus time data. Half-life is the time required for a reactant's concentration to reduce to half of its initial value and can be used to characterize reaction order.
The branch of chemistry, which deals with the study of reaction rates and their mechanisms, called chemical kinetics.
Thermodynamics tells only about the feasibility of a reaction whereas chemical kinetics tells about the rate of a reaction.
For example, thermodynamic data indicate that diamond shall convert to graphite but in reality the conversion rate is so slow that the change is not perceptible at all.
Chemical Kinetics & Rate of a chemical reaction.pptxDidarul3
Rate of reaction
✓Zero order reaction
✓1st order reaction
✓2nd order reaction
✓Theories of chemical reaction rate
Determination of order of reaction
Factors that influence reaction rates
Activation energy
Activation complex
The branch of chemistry, which deals with the study of reaction rates and their mechanisms, called chemical kinetics.
Thermodynamics tells only about the feasibility of a reaction whereas chemical kinetics tells about the rate of a reaction.
For example, thermodynamic data indicate that diamond shall convert to graphite but in reality the conversion rate is so slow that the change is not perceptible at all.
Chemical Kinetics & Rate of a chemical reaction.pptxDidarul3
Rate of reaction
✓Zero order reaction
✓1st order reaction
✓2nd order reaction
✓Theories of chemical reaction rate
Determination of order of reaction
Factors that influence reaction rates
Activation energy
Activation complex
9.2Physical Science SHS Measurement of Reaction Ra.pptxgoddesshera
It tells how fast or slow a certain chemical reaction occur.
There are two factors that can be used to determine reaction rates: concentration and rate constant.
It can simply be determined by measuring the changes in the concentrations of the reactants or products within a particular time frame.
Generally, a chemical reaction is represented in the following format.
As the chemical reaction takes place, the amount of reactants decrease as the amount of the products increase.
Δ[A], Δ[B], Δ[C], and Δ[D] are the measures of the change in respective concentrations over a period of time, Δt.
Reaction rates are always positive.
In terms of appearance of a product in a reaction, the expression is positive since the change in concentration is positive.
In term of disappearance of a reactant, the case is opposite; hence the expression is appended by a negative sign.
The rate law expresses the relationship of the rate of reaction to the rate constant and the concentration of the reactants raised to certain exponents.
The rate constant, k, is a constant of proportionality between the reaction rate and the concentration of the reactants.
Rate laws are always determined experimentally.
9.2Physical Science SHS Measurement of Reaction Ra.pptxgoddesshera
It tells how fast or slow a certain chemical reaction occur.
There are two factors that can be used to determine reaction rates: concentration and rate constant.
It can simply be determined by measuring the changes in the concentrations of the reactants or products within a particular time frame.
Generally, a chemical reaction is represented in the following format.
As the chemical reaction takes place, the amount of reactants decrease as the amount of the products increase.
Δ[A], Δ[B], Δ[C], and Δ[D] are the measures of the change in respective concentrations over a period of time, Δt.
Reaction rates are always positive.
In terms of appearance of a product in a reaction, the expression is positive since the change in concentration is positive.
In term of disappearance of a reactant, the case is opposite; hence the expression is appended by a negative sign.
The rate law expresses the relationship of the rate of reaction to the rate constant and the concentration of the reactants raised to certain exponents.
The rate constant, k, is a constant of proportionality between the reaction rate and the concentration of the reactants.
Rate laws are always determined experimentally.
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.
The empire's roots lie in the city of Rome, founded, according to legend, by Romulus in 753 BCE. Over centuries, Rome evolved from a small settlement to a formidable republic, characterized by a complex political system with elected officials and checks on power. However, internal strife, class conflicts, and military ambitions paved the way for the end of the Republic. Julius Caesar’s dictatorship and subsequent assassination in 44 BCE created a power vacuum, leading to a civil war. Octavian, later Augustus, emerged victorious, heralding the Roman Empire’s birth.
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.
The Roman Empire’s society was hierarchical, with a rigid class system. At the top were the patricians, wealthy elites who held significant political power. Below them were the plebeians, free citizens with limited political influence, and the vast numbers of slaves who formed the backbone of the economy. The family unit was central, governed by the paterfamilias, the male head who held absolute authority.
Culturally, the Romans were eclectic, absorbing and adapting elements from the civilizations they encountered, particularly the Greeks. Roman art, literature, and philosophy reflected this synthesis, creating a rich cultural tapestry. Latin, the Roman language, became the lingua franca of the Western world, influencing numerous modern languages.
Roman architecture and engineering achievements were monumental. They perfected the arch, vault, and dome, constructing enduring structures like the Colosseum, Pantheon, and aqueducts. These engineering marvels not only showcased Roman ingenuity but also served practical purposes, from public entertainment to water supply.
The Art Pastor's Guide to Sabbath | Steve ThomasonSteve Thomason
What is the purpose of the Sabbath Law in the Torah. It is interesting to compare how the context of the law shifts from Exodus to Deuteronomy. Who gets to rest, and why?
Instructions for Submissions thorugh G- Classroom.pptxJheel Barad
This presentation provides a briefing on how to upload submissions and documents in Google Classroom. It was prepared as part of an orientation for new Sainik School in-service teacher trainees. As a training officer, my goal is to ensure that you are comfortable and proficient with this essential tool for managing assignments and fostering student engagement.
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
In this webinar you will learn how your organization can access TechSoup's wide variety of product discount and donation programs. From hardware to software, we'll give you a tour of the tools available to help your nonprofit with productivity, collaboration, financial management, donor tracking, security, and more.
The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
For more information, visit-www.vavaclasses.com
Operation “Blue Star” is the only event in the history of Independent India where the state went into war with its own people. Even after about 40 years it is not clear if it was culmination of states anger over people of the region, a political game of power or start of dictatorial chapter in the democratic setup.
The people of Punjab felt alienated from main stream due to denial of their just demands during a long democratic struggle since independence. As it happen all over the word, it led to militant struggle with great loss of lives of military, police and civilian personnel. Killing of Indira Gandhi and massacre of innocent Sikhs in Delhi and other India cities was also associated with this movement.
How to Make a Field invisible in Odoo 17Celine George
It is possible to hide or invisible some fields in odoo. Commonly using “invisible” attribute in the field definition to invisible the fields. This slide will show how to make a field invisible in odoo 17.
2. • The branch of chemistry, which deals with
the study of reaction rates and their
mechanisms, called chemical kinetics.
• Thermodynamics tells only about the
feasibility of a reaction whereas chemical
kinetics tells about the rate of a reaction.
• For example, thermodynamic data indicate
that diamond shall convert to graphite but in
reality the conversion rate is so slow that the
change is not perceptible at all.
3. • Kinetic studies not only help us to determine
the speed or rate of a chemical reaction but
also describe the conditions by which the
reaction rates can be altered.
• The factors such as concentration,
temperature, pressure and catalyst affect the
rate of a reaction.
4. • The speed of a reaction or the rate of a
reaction can be defined as the change in
concentration of a reactant or product in unit
time. It can be expressed in terms of:
• (i) the rate of decrease in concentration of
any one of the reactants, or
• (ii) the rate of increase in concentration of
any one of the products.
5. Consider a hypothetical reaction, assuming that the volume of
the system remains constant
R → P
One mole of the reactant R produces one mole of the product
P. If [R]1 and [P]1 are the concentrations of R and respectively
at time t1and [R]2 and [P]2 are their concentrations at time t2
then,
Δt = t2 – t1
Δ[R] = [R]2 – [R]1 Δ [P] = [P]2 – [P]1
&
The square brackets in the above expressions are used to express molar
concentration.
6. • Rate of disappearance of R
= Decrease in concentration of R = − Δ [R]
Time taken Δt
Rate of appearance of P
= Increase in concentration of P = + Δ [P]
Time taken Δ t
Since, Δ[R] is a negative quantity (as concentration of reactants is
decreasing), it is multiplied with –1 to make the rate of the reaction a
positive quantity.
7. The Rate of a Chemical Reaction
2 Fe3+(aq) + Sn2+ → 2 Fe2+(aq) +Sn4+(aq)
t = 38.5 s [Fe2+] = 0.0010 M
Δt = 38.5 s Δ[Fe2+] = (0.0010 – 0) M
Rate of formation of Fe2+= = = 2.6x10-5 M s-
Δ[Fe2+]
Δt
0.0010 M
38.5 s
Consider the following chemical reaction -
9. a A + b B → c C + d D
Rate of reaction = rate of disappearance of reactants
=
Δ[C]
Δt
1
c
=
Δ[D]
Δt
1
d
Δ[A]
Δt
1
a
= -
Δ[B]
Δt
1
b
= -
= rate of appearance of products
Δ[A]
Δt
1
a
= -
Δ[B]
Δt
1
b
-
=
Δ[C]
Δt
1
c
=
Δ[D]
Δt
1
d
or
Eqn.1
Eqn.2
Eqn.3
10. Average rate depends upon the change in conc. of
reactants or products and the time taken for that
change to occur.
Equations 1-3 represent the average rate of a
reaction, rav.
The rate of reaction at a particular moment of
time is called as the instantaneous rate, rins.
It is obtained when we consider the average rate at
the smallest time interval say dt ( i.e. when Δt
approaches zero).
11. • Mathematically for an infinitesimally small time
interval, dt, instantaneous rate is given by –
• rav = −Δ[R ] = Δ[P ]
Δt Δt
As Δt → 0 or
rins. = - d[R] = d[P]
dt dt
Unit of rate of reaction:– mol L-1 s-1
12. H2O2(aq) → H2O(l) + ½ O2(g)
-(-1.7 M / 2600 s) =
6 x 10-4 M s-1
-(-2.32 M / 1360 s) = 1.7 x 10-3 M s-1 Rate =
-Δ[H2O2]
Δt
Initial rate ,Average rate over a time period. Instantaneous rate – slope of tangent
lin.
13. Factors affecting the Rate of a Chemical
Reaction
1-Nature of reactant : Ionic substance react much faster than
covalent substances.
2-Concencentration of Reactants
: Rate of reaction is directly
proportional to conc. of reactants
(partial pressure in case of gaseous
- phase reactions).
3-Temperature : Rate of reaction increases with increase
in temperature.
4-Presence of Catalyst : A catalyst alters the Rate of a reaction.
5-Surface Area of the Reactants:
Rate of rean. ∝ surface area.
6- Radiations
14. Rate Law or Rate Expression and Rate
Constant
• The expression which relates of rate of
reaction to concentration of the reactants is
known as rate law. It is also called as rate
equation or rate expression.
• Consider a general reaction
aA + bB → cC + dD
• where a, b, c and d are the stoichiometric
coefficients of reactants and products.
15. Rate Law or Rate Expression and Rate
Constant
• The rate expression for this reaction is -
• where exponents x and y may or may not be equal
to the stoichiometric coefficients (a and b) of the
reactants.
Rate of reaction ∝ [A]x[B]y
or eqn.4
Rate of reaction = k [A]x[B]y eqn.5
16. Rate Law or Rate Expression and Rate
Constant
• Equation 5 can also be written as-
eqn.6
• This form(eq.6) of equation (5) is known as
differential rate equation, where k is a
proportionality constant called rate constant or
velocity constant or specific reaction rate.
d[R]
dt
= k[A]x[B]y
17. Rate Law or Rate Expression and Rate
Constant
• Thus, rate law is the expression in which reaction
rate is given in terms of molar concentration of
reactants with each term raised to some power,
which may or may not be same as the
stoichiometric coefficient of the reacting species in
a balanced chemical equation.
• Note:Rate law for any reaction cannot be predicted
by merely looking at the balanced chemical
equation, i.e., theoretically but must be determined
experimentally.
18. Rate Law or Rate Expression and Rate Constant
• Rate Constant (k) : For a general reaction
aA + bB → cC + dD
Where k is known as rate constant
When [A] = [B] = 1 mol/L, than
thus rate constant of a chemical reaction may be
defined as the reaction rate when the
Rate of reaction = k [A]x[B]y
Rate of reaction = k
19. The value of rate constant is definite and
constant for a particular reaction at given
temperature.
Rate constant is independent of
concentration of reactants it depends only
upon temperature and presence of catalyst.
Rate Law or Rate Expression and Rate Constant
20. • The sum of powers of the concentration of the
reactants in the rate law expression is called the
order of that chemical reaction.
• For a general reaction
aA + bB → cC + dD
Let Rate of reaction = k [A]x[B]y
Here ,
x = order of reaction w.r.t. A
y = order of reaction w.r.t. B
Overall order of reaction(n) = x + y
22. Order of a reaction can be 0, 1, 2, 3 and even a
fraction.
Depending upon order of reaction, reactions are
termed as zero, first or second order reactions.
A zero order reaction means that the rate of reaction
is independent of the concentration of reactants.
Order of reaction cannot be predicted by merely
looking at the balanced chemical equation, i.e.,
theoretically but must be determined experimentally.
23. For a nth order reaction- A → Product
Rate = k [A]n
a
Rate
k =
[A]n
=
concentration
time
x
(concentration)n
1
= (concentration)1-n time-1
k
24.
25. 1.
2.
3.
Practice Problems
For the reaction
A + B Products
The following initial rates were obtained at various given intial
concentrations
S. No [A] [B] Rate (mol lt–1 sec–1)
1. 0.1 0.1 0.05
2. 0.2 0.1 0.10
3. 0.1 0.2 0.05
Write rate law and find the rate constant of the above reaction.
26. Elementary reactions are those which complete is one
step while complex reactions are multistep reactions
where products are obtained after completion of a
sequence of elementary reactions.
e.g. (a) Elementary reaction
(b) Complex reaction
Elementary & complex reactions
27. Molecularity of a Reaction
Molecularity of a reaction is simply the
number of reacting species (atoms, ions or
molecules) involving is an elementary
reaction which must collide simultaneously.
Let us consider the following reactions,
28. Ans:- Since the chances of collision and
reaction of more than three molecules at a
time are very less, the molecularity greater
than three is rare.
Molecularity of a Reaction
Q.Why the reactions having molecularity
greater than three is rare ?
29. Molecularity of a Reaction
Molecularity in case of complex reactions?
Molecularity of a complex reaction has no meaning.
Actually a complex reaction is the series of two or
more elementary reactions and thus, it completes in
several steps. The slowest step or slowest reaction
determines the rate of the reaction. Hence we find
out the molecularity of the slowest elementary
reaction of a complex reaction which is, in general,
similar to the overall order of the complex reaction.
30. Molecularity vs. Order
Order of reaction is for overall
reaction.
The overall molecularity of complex
reaction has no significance.
Individual step has its own
molecularity.
It can even have fractional values.
It is always a whole number.
It is determined experimentally.
It is a theoretical concept.
Order of reaction can be zero.
Molecularity of reaction
Cannot be zero.
It is the sum of the power of
concentration terms on which the rate
of reaction actually depends or it is
the sum of powers of the
concentration terms in the rate law
equation.
It is the number of atoms, ions or
molecules that must collide with one
another simultaneously so as to
result into a chemical
reaction.
Order of Reaction
Molecularity of Reaction
31. Integrated Rate Equations
Zero Order Reactions
Zero order reaction means that the rate of the reaction is
proportional to zero power of the concentration of reactants.
Consider the reaction,
R → P
34. Integrated Rate Equations
First Order Reactions
First order reaction means that the rate of the reaction is
proportional to first power of the concentration of reactants.
Consider the reaction,
R → P
37. Integrated Rate Equations
1. The thermal decomposition of HCOOH is a first order reaction
with a rate constant of 2.4 x 10─3 s ─1 at a certain temperature.
Calculate how long will it take for three-fourth (3/4) of initial
quantity of HCOOH to decompose ? (log 0.25 = − 0.6021 ) [2011]
2.A first order reaction has a rate constant of 0.0051 min─1 . If we
begin with 0.10 M conc. of the reactant, how much conc. of the
reactant will remain is solution after 3 hrs? [2011,09]
3. The rate constant for a reaction of Zero order in A is 0.0030
mol L─1 s─1 . How long will it take for the initial conc. of A to
fall from 0.10 M to .075 M ? [2010]
38. The half-life of a reaction is the time in which the
concentration of a reactant is reduced to one half of its initial
concentration. It is represented as t1/2
Half-Life of a Reaction
t1/2 for a Zero Order Reactions
39. Half-Life of a Reaction
t1/2 for a First Order Reactions
Thus for a first order
reaction, half-life
period is constant, i.e.,
it is independent of
initial concentration
of the reacting species.
40. Half-Life of a Reaction
Practice Problems
1. A first order reaction takes 40 minutes for 30 %
completion . calculate its t1/2 value. (2008,13)
2. The decomposition of phosphine PH3 . Proceeds acc. to
following eqn:
4 PH3 (g) ---> P4(g) + 6H2 (g) ;
It is found that he reaction follows the following rate equation:
Rate = K [PH3] ;
The half lite of PH3 is 37.9 S at 1200C
(a) How much time is required of 3/4th of PH3 to decompose ?
(2) What fraction of original sample of PH3 remains behind
after 1 minute ? (2010,09)
41. Pseudo - first order reaction
Reactions which are not truly of the first order but under certain
conditions reactions become that of first order are called
pseudo unimolecular reaction.
For example: Hydrolysis of ester in presence of acid
CH3COOC2H5 + H2O CH3COOH + C2H5OH
From this reaction, the rate expression should be
r = k [ester] [H2O]
Since, hydrolysis takes place in the excess of H2O and
concentration change of H2O is negligible practically.
therefore, r = k’ [ester]
Where k’ = k[H2O].
42. Methods of determining the order of a reaction
Integrated method
The equation which gives a constant value of k decides the order
of reaction
Graphical method
The data are plotted acc to different integrated rate equations
so as to yield a straight line .Slope gives the value of rate
constant
Initial rate method
Concentration of one of the reactant is varied
Half life method
In this method we plot half life of the reactant versus conc. of
the reactant.
43. Methods of determining the order of a reaction
L mole-1 sec-1
k
1/[A] vs t
Second
sec-1
-k
In[A] vs t
[A]=[Ao]e-kt
First
Mole l-1 sec-1
-k
[A] vs t
[A]=[Ao]-kt
Zero
Units of rate
constant
Slope
of
kinetic
s plot
Characteristic
kinetics Plot
Integrated rate
law
Differential
rate law
Reaction
Order
d[A]
k
dt
d[A]
k[A]
dt
2
d[A]
k[A]
dt
[Ao]
A
1 k [A]
45. Conc. [A]
t
log [A]
t t
1/ [A]
Graphical representation for concentration of integrated rate equation versus time
zero order first order second order
Graphical Representation
46. Initial rate method
• This method involves the determination of the order
of each reactant separately.
• To determine the order of a particular reactant, its
concentration is varied keeping the concentrations of
other reactants constant.
• In every experiment, we determine the initial rate of
the reaction and observe the dependence of rate on
that particular reactant.
m n
r [A] [B]
m
m n
1 1 1 1
m n
2 2 2 2
r [A ] [B] r [A ]
= ; =
r [A ] [B] r [A ]
Keeping [B] constant
47. Illustrative Example
Rate of the reaction; A + B = products; is given below as a
function of the initial concentration of ‘A’ and ‘B’.
[A](mol L-1) [B](mol L-1) rate(mol L-1min-1)
0.01 0.01 0.005
0.02 0.01 0.010
0.01 0.02 0.005
Determine the order of the reaction with respect to ‘A’ and ‘B’.
Solution:
For first two experiments, the concentration of the reactant ‘B’ is
constant.
Rate of the reaction depend linearly on reactant ‘A’.
Now, taking experiments first and third, the concentration of the
reactant ‘A’ is constant.
Therefore, rate of the reaction is independent of ‘B’.
Thus, order of the reaction with respect to ‘A’ = one.
Order of the reaction with respect to ‘B’ = zero.
48. Half life method
1/2 n 1
0
1
t
[A]
Graphical representation for half lives versus concentration
t1/2
a
zero order
1/a
second order
t1/2 t1/2
a
first order
49. Illustrative Example
The half-life of a particular chemical reaction at two different
initial concentrations 5 x 10-4 and 25 x10-5 M are 2 and 16 hours.
Calculate the order of reaction.
n 1
0
1 / 2 2 1
1 / 2 1
0 2
A
(t )
(t ) A
n 1
4
n 1
5
16 5 10
(2)
2 25 10
Solution:
n-1
8 = (2)
n - 1 =3
n = 4
50. Integrated method
In this method, we put the data into the integrated
form of the rate laws and calculate the values of the
rate constants for different kinetics of the reaction.
The order of the reaction is that one for which the value
of rate constant is constant.
51. Some first order reactions
Decomposition of H2O2
2 2 2 2
1
H O H O O
2
Let Vo & Vt be volume of KMnO4 used during zero & time
t respectively
t
o
t
V a
V a x
V
2.303
k log
t V
52. Some first order reactions
Hydrolysis of ester
H
3 2 5 2 3 2 5
CH COOC H H O CH COOH C H OH
a 0 0
a x x x
0 a a
O
t
V HCl
V HCl x
V HCl a
t
V V a x
V a
o
t
V V
2.303
k log
t V V
Let V0 , Vt be the volume of alkali required for titration
during 0 ,t & infinite time
V
54. Collision theory
Reaction occurs when reacting species have sufficient energy
to collide and proper orientation in space.
Energy barrier:
The minimum energy which the colliding particles possess in
order to bring about the chemical reaction is called threshold
energy
The energy difference between threshold energy & average
energy of reacting molecules is called activation energy
Orientation barrier:
Colliding molecules should be in their proper orientation at
the time of collision.
55. Transition State Theory
In the activated complex theory, we consider two reactants
approaching and their potential energy rising and reaching a
maximum.
a a
H E E `
Activation energy - the energy needed to form activated
complex is called energy of activation. It is very low for some
reactions and very high for others.
56. Some Points about Ea
1. Ea is always positive.
2. The larger the value of Ea, the slower the
rate of a reaction at a given temperature.
3. The larger the value of Ea, the steeper the
slope of (ln k) vs (1/T). A high activation
energy corresponds to a reaction rate that
is very sensitive to temperature.
57. Effect of temperature on rate of chemical
reaction
For a chemical reaction with rise in temperature by 10°,
the rate constant is nearly doubled
The ratio is called the temperature
coefficient and its value is 2 or 3
k(T+10)
kT
58. A is frequency factor or Arhenius constant, Ea is activation
energy
-Ea/RT
k = A.e
Plot of log k vs 1/T is a straight line & slope = ̶ Ea/2.303R
The temperature dependence of the rate of a chemical reaction
can be accurately explained by Arrhenius equation
Effect of temperature on rate of chemical
reaction
or
Arrhenius equation
59. Plot of ln k vs 1/T is a straight line & slope =-Ea/R
Effect of temperature on rate of chemical
reaction
60. Effect of temperature on rate of chemical
reaction
At temperature T1 Eqn.1
At temperature T2 Eqn.2
k1 and k2 are the values of rate constants at temperatures T1 and T2
respectively. Subtracting equation (2) from (1), we obtain
61. -Ea/RT
k = A.e
a
2
1 1 2
E
k 1 1
or log = -
k 2.303 R T T
Effect of temperature on rate of chemical
reaction
62.
a
2 2 1
10
1 1 2
E
K T - T
log =
K 2.303 R T T
a
E 320-300
log4=
2.303×1.987 300×320
a
0.60205×2.303×1.987×300×320
E =
20
= 13222.98 cals
Ea = 13.311 K cals
The specific reaction rate for a reaction increases by a factor 4 if
the temperature is changed from 27o C to 47o C. Find the
activation energy for the reaction.
Illustrative Example
Solution:
63. Illustrative Example
The activation energy of one of the reactions in the Krebs citric
acid cycle is 87 kJ/mol. What is the change in the rate constant
when the temperature falls from 37oC to 15oC?
Solution:
64. Catalysis
Catalyst: A substance that changes the rate of a reaction
without being consumed in the reaction.
• Provides an easier way to react.
• Lower activation energy.
• Still make the same products.
• Enzymes are biological catalysts.
Inhibitor: A substance that decreases the rate of reaction (a
negative catalyst).
65. How catalyst change reaction rate
• Catalysts are
the one way to
lower the
energy of
activation
for a particular
reaction by
altering the
path of the
reaction.
• The lower
activation
energy allows
the reaction to
proceed
faster.
66. Rate Law and Mechanism
A mechanism is a collection of elementary steps devised to
explain the reaction in view of the observed rate law.
For the reaction, 2 NO2 (g) + F2 (g) 2 NO2F (g), the rate
law is,
rate = k [NO2] [F2] .
Can the elementary reaction be the same as the overall
reaction?
If they were the same the rate law would have been
rate = k [NO2]2 [F2],
Therefore, the overall reaction is not an elementary
reaction.
67. Rate-determining Step in a Mechanism
Slowest step:
The rate determining step is the slowest elementary step
in a mechanism, and the rate law for this step is the rate
law for the overall reaction.
Steady-state approximation:
The steady-state approximation is a general method for
deriving rate laws when the relative speed cannot be
identified. It is based on the assumption that the
concentration of the intermediate is constant.
68. Illustrative Problem
The hypothetical reaction A2+ B2 2AB
follows the following mechanism
2
A A + A (fast)
2
A + B AB + B (slow)
A B AB (fast)
The order of the overall reaction is
(a) 0 (b) 1
(c) 2 (d) 3/2
69. Solution
The order depends on slowest step
2
1/2
2 2
1/2
2 2
Rate(slow step) = k[A][B ]
= k[B ].k`[A ]
= k"[A ] [B ]
1 3
Overall order 1
2 2
Hence, the answer is (d).
70. Illustrative Problem
At 380° C, the half-life period for the first order
decomposition of H2O2 is 360 min. The energy of
activation of the reaction is 200 kJ mole-1. Calculate the
time required for 75% decomposition at 450° C.
71. Solution
-3 -1
380
0.693
k = =1.925×10 min
360
450
380
k 200×103 1 1
log = -
k 2.303×8.314 653 723
-2
450
450
-3
k
log =1.55 k = 6.83×10
1.925×10
1 -2
2
0.693
t at 450°C = =10.15 min
6.83×10
75% 1
2
t =2t =20.29 min.
Since, Δ[R] is a negative quantity (as concentration of reactants is
decreasing), it is multiplied with –1 to make the rate of the reaction a
positive quantity.
Eqn.1
Unit of rate of reaction :- mol L-1 s-1
Initial rate
Average rate over a time period.
Instantaneous rate – slope of tangent lin.
-
Rate k==[A concentration time x (concentration)1-n= k (concentration)1-n time-1
1