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1 | 2805-2808 | 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 Therefore, most people think
After studying this Unit, you will be
able to
·
define
the
average
and
instantaneous rate of a reaction;
·
express the rate of a reaction in
terms of change in concentration
of either of the reactants or
products with time;
·
distinguish between elementary
and complex reactions;
·
differentiate
between
the
molecularity and order of a
reaction;
·
define rate constant;
·
discuss the dependence of rate of
reactions
on
concentration,
temperature and catalyst;
·
derive integrated rate equations
for the zero and first order
reactions;
·
determine the rate constants for
zeroth and first order reactions;
·
describe collision theory Objectives
Chemical Kinetics helps us to understand how chemical reactions
occur |
1 | 2806-2809 | 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 Therefore, most people think
After studying this Unit, you will be
able to
·
define
the
average
and
instantaneous rate of a reaction;
·
express the rate of a reaction in
terms of change in concentration
of either of the reactants or
products with time;
·
distinguish between elementary
and complex reactions;
·
differentiate
between
the
molecularity and order of a
reaction;
·
define rate constant;
·
discuss the dependence of rate of
reactions
on
concentration,
temperature and catalyst;
·
derive integrated rate equations
for the zero and first order
reactions;
·
determine the rate constants for
zeroth and first order reactions;
·
describe collision theory Objectives
Chemical Kinetics helps us to understand how chemical reactions
occur 3
Chemical Kinetics
Unit
Unit
Unit
Unit3Unit
Chemical Kinetics
Rationalised 2023-24
62
Chemistry
that diamond is forever |
1 | 2807-2810 | Therefore, most people think
After studying this Unit, you will be
able to
·
define
the
average
and
instantaneous rate of a reaction;
·
express the rate of a reaction in
terms of change in concentration
of either of the reactants or
products with time;
·
distinguish between elementary
and complex reactions;
·
differentiate
between
the
molecularity and order of a
reaction;
·
define rate constant;
·
discuss the dependence of rate of
reactions
on
concentration,
temperature and catalyst;
·
derive integrated rate equations
for the zero and first order
reactions;
·
determine the rate constants for
zeroth and first order reactions;
·
describe collision theory Objectives
Chemical Kinetics helps us to understand how chemical reactions
occur 3
Chemical Kinetics
Unit
Unit
Unit
Unit3Unit
Chemical Kinetics
Rationalised 2023-24
62
Chemistry
that diamond is forever 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 |
1 | 2808-2811 | Objectives
Chemical Kinetics helps us to understand how chemical reactions
occur 3
Chemical Kinetics
Unit
Unit
Unit
Unit3Unit
Chemical Kinetics
Rationalised 2023-24
62
Chemistry
that diamond is forever 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 |
1 | 2809-2812 | 3
Chemical Kinetics
Unit
Unit
Unit
Unit3Unit
Chemical Kinetics
Rationalised 2023-24
62
Chemistry
that diamond is forever 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 At the macroscopic level, we are interested in
amounts reacted or formed and the rates of their consumption or
formation |
1 | 2810-2813 | 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 At the macroscopic level, we are interested in
amounts reacted or formed and the rates of their consumption or
formation At the molecular level, the reaction mechanisms involving
orientation and energy of molecules undergoing collisions,
are discussed |
1 | 2811-2814 | The factors
such as concentration, temperature, pressure and catalyst affect the
rate of a reaction At the macroscopic level, we are interested in
amounts reacted or formed and the rates of their consumption or
formation At the molecular level, the reaction mechanisms involving
orientation and energy of molecules undergoing collisions,
are discussed In this Unit, we shall be dealing with average and instantaneous
rate of reaction and the factors affecting these |
1 | 2812-2815 | At the macroscopic level, we are interested in
amounts reacted or formed and the rates of their consumption or
formation At the molecular level, the reaction mechanisms involving
orientation and energy of molecules undergoing collisions,
are discussed In this Unit, we shall be dealing with average and instantaneous
rate of reaction and the factors affecting these Some elementary
ideas about the collision theory of reaction rates are also given |
1 | 2813-2816 | At the molecular level, the reaction mechanisms involving
orientation and energy of molecules undergoing collisions,
are discussed In this Unit, we shall be dealing with average and instantaneous
rate of reaction and the factors affecting these Some elementary
ideas about the collision theory of reaction rates are also given However, in order to understand all these, let us first learn about the
reaction rate |
1 | 2814-2817 | In this Unit, we shall be dealing with average and instantaneous
rate of reaction and the factors affecting these Some elementary
ideas about the collision theory of reaction rates are also given However, in order to understand all these, let us first learn about the
reaction rate Some reactions such as ionic reactions occur very fast, for example,
precipitation of silver chloride occurs instantaneously by mixing of
aqueous solutions of silver nitrate and sodium chloride |
1 | 2815-2818 | Some elementary
ideas about the collision theory of reaction rates are also given However, in order to understand all these, let us first learn about the
reaction rate Some reactions such as ionic reactions occur very fast, for example,
precipitation of silver chloride occurs instantaneously by mixing of
aqueous solutions of silver nitrate and sodium chloride On the other
hand, some reactions are very slow, for example, rusting of iron in
the presence of air and moisture |
1 | 2816-2819 | However, in order to understand all these, let us first learn about the
reaction rate Some reactions such as ionic reactions occur very fast, for example,
precipitation of silver chloride occurs instantaneously by mixing of
aqueous solutions of silver nitrate and sodium chloride On the other
hand, some reactions are very slow, for example, rusting of iron in
the presence of air and moisture Also there are reactions like inversion
of cane sugar and hydrolysis of starch, which proceed with a moderate
speed |
1 | 2817-2820 | Some reactions such as ionic reactions occur very fast, for example,
precipitation of silver chloride occurs instantaneously by mixing of
aqueous solutions of silver nitrate and sodium chloride On the other
hand, some reactions are very slow, for example, rusting of iron in
the presence of air and moisture Also there are reactions like inversion
of cane sugar and hydrolysis of starch, which proceed with a moderate
speed Can you think of more examples from each category |
1 | 2818-2821 | On the other
hand, some reactions are very slow, for example, rusting of iron in
the presence of air and moisture Also there are reactions like inversion
of cane sugar and hydrolysis of starch, which proceed with a moderate
speed Can you think of more examples from each category You must be knowing that speed of an automobile is expressed in
terms of change in the position or distance covered by it in a certain
period of time |
1 | 2819-2822 | Also there are reactions like inversion
of cane sugar and hydrolysis of starch, which proceed with a moderate
speed Can you think of more examples from each category You must be knowing that speed of an automobile is expressed in
terms of change in the position or distance covered by it in a certain
period of time Similarly, 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 |
1 | 2820-2823 | Can you think of more examples from each category You must be knowing that speed of an automobile is expressed in
terms of change in the position or distance covered by it in a certain
period of time Similarly, 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 To be more specific, 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 |
1 | 2821-2824 | You must be knowing that speed of an automobile is expressed in
terms of change in the position or distance covered by it in a certain
period of time Similarly, 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 To be more specific, 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 Consider a hypothetical reaction, assuming that the volume of the
system remains constant |
1 | 2822-2825 | Similarly, 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 To be more specific, 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 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 |
1 | 2823-2826 | To be more specific, 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 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 P respectively at time t1
and [R]2 and [P]2 are their concentrations at time t2 then,
Dt
=
t2 – t1
D[R]
=
[R]2 – [R]1
D [P] =
[P]2 – [P]1
The square brackets in the above expressions are used to express
molar concentration |
1 | 2824-2827 | 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 P respectively at time t1
and [R]2 and [P]2 are their concentrations at time t2 then,
Dt
=
t2 – t1
D[R]
=
[R]2 – [R]1
D [P] =
[P]2 – [P]1
The square brackets in the above expressions are used to express
molar concentration Rate of disappearance of R
[
]
Decrease in concentration of R
R
=
Time taken
t
= −∆
∆
(3 |
1 | 2825-2828 | 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 P respectively at time t1
and [R]2 and [P]2 are their concentrations at time t2 then,
Dt
=
t2 – t1
D[R]
=
[R]2 – [R]1
D [P] =
[P]2 – [P]1
The square brackets in the above expressions are used to express
molar concentration Rate of disappearance of R
[
]
Decrease in concentration of R
R
=
Time taken
t
= −∆
∆
(3 1)
3 |
1 | 2826-2829 | If
[R]1 and [P]1 are the concentrations of R and P respectively at time t1
and [R]2 and [P]2 are their concentrations at time t2 then,
Dt
=
t2 – t1
D[R]
=
[R]2 – [R]1
D [P] =
[P]2 – [P]1
The square brackets in the above expressions are used to express
molar concentration Rate of disappearance of R
[
]
Decrease in concentration of R
R
=
Time taken
t
= −∆
∆
(3 1)
3 1
3 |
1 | 2827-2830 | Rate of disappearance of R
[
]
Decrease in concentration of R
R
=
Time taken
t
= −∆
∆
(3 1)
3 1
3 1
3 |
1 | 2828-2831 | 1)
3 1
3 1
3 1
3 |
1 | 2829-2832 | 1
3 1
3 1
3 1
3 |
1 | 2830-2833 | 1
3 1
3 1
3 1 Rate of a
Rate of a
Rate of a
Rate of a
Rate of a
Chemical
Chemical
Chemical
Chemical
Chemical
Reaction
Reaction
Reaction
Reaction
Reaction
Rationalised 2023-24
63
Chemical Kinetics
Rate of appearance of P
[ ]
Increase in concentration of P
P
=
Time taken
t
∆
= + ∆
(3 |
1 | 2831-2834 | 1
3 1
3 1 Rate of a
Rate of a
Rate of a
Rate of a
Rate of a
Chemical
Chemical
Chemical
Chemical
Chemical
Reaction
Reaction
Reaction
Reaction
Reaction
Rationalised 2023-24
63
Chemical Kinetics
Rate of appearance of P
[ ]
Increase in concentration of P
P
=
Time taken
t
∆
= + ∆
(3 2)
Since, D[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 |
1 | 2832-2835 | 1
3 1 Rate of a
Rate of a
Rate of a
Rate of a
Rate of a
Chemical
Chemical
Chemical
Chemical
Chemical
Reaction
Reaction
Reaction
Reaction
Reaction
Rationalised 2023-24
63
Chemical Kinetics
Rate of appearance of P
[ ]
Increase in concentration of P
P
=
Time taken
t
∆
= + ∆
(3 2)
Since, D[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 Equations (3 |
1 | 2833-2836 | 1 Rate of a
Rate of a
Rate of a
Rate of a
Rate of a
Chemical
Chemical
Chemical
Chemical
Chemical
Reaction
Reaction
Reaction
Reaction
Reaction
Rationalised 2023-24
63
Chemical Kinetics
Rate of appearance of P
[ ]
Increase in concentration of P
P
=
Time taken
t
∆
= + ∆
(3 2)
Since, D[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 Equations (3 1) and (3 |
1 | 2834-2837 | 2)
Since, D[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 Equations (3 1) and (3 2) given above represent the average rate of
a reaction, rav |
1 | 2835-2838 | Equations (3 1) and (3 2) given above represent the average rate of
a reaction, rav Average rate depends upon the change in concentration of reactants
or products and the time taken for that change to occur (Fig |
1 | 2836-2839 | 1) and (3 2) given above represent the average rate of
a reaction, rav Average rate depends upon the change in concentration of reactants
or products and the time taken for that change to occur (Fig 3 |
1 | 2837-2840 | 2) given above represent the average rate of
a reaction, rav Average rate depends upon the change in concentration of reactants
or products and the time taken for that change to occur (Fig 3 1) |
1 | 2838-2841 | Average rate depends upon the change in concentration of reactants
or products and the time taken for that change to occur (Fig 3 1) Fig |
1 | 2839-2842 | 3 1) Fig 3 |
1 | 2840-2843 | 1) Fig 3 1: Instantaneous and average rate of a reaction
Units of rate of a reaction
From equations (3 |
1 | 2841-2844 | Fig 3 1: Instantaneous and average rate of a reaction
Units of rate of a reaction
From equations (3 1) and (3 |
1 | 2842-2845 | 3 1: Instantaneous and average rate of a reaction
Units of rate of a reaction
From equations (3 1) and (3 2), it is clear that units of rate are
concentration time–1 |
1 | 2843-2846 | 1: Instantaneous and average rate of a reaction
Units of rate of a reaction
From equations (3 1) and (3 2), it is clear that units of rate are
concentration time–1 For example, if concentration is in mol L–1 and
time is in seconds then the units will be mol L-1s–1 |
1 | 2844-2847 | 1) and (3 2), it is clear that units of rate are
concentration time–1 For example, if concentration is in mol L–1 and
time is in seconds then the units will be mol L-1s–1 However, in gaseous
reactions, when the concentration of gases is expressed in terms of their
partial pressures, then the units of the rate equation will be atm s–1 |
1 | 2845-2848 | 2), it is clear that units of rate are
concentration time–1 For example, if concentration is in mol L–1 and
time is in seconds then the units will be mol L-1s–1 However, in gaseous
reactions, when the concentration of gases is expressed in terms of their
partial pressures, then the units of the rate equation will be atm s–1 From the concentrations of C4H9Cl (butyl chloride) at different times given
below, calculate the average rate of the reaction:
C4H9Cl + H2O ® C4H9OH + HCl
during different intervals of time |
1 | 2846-2849 | For example, if concentration is in mol L–1 and
time is in seconds then the units will be mol L-1s–1 However, in gaseous
reactions, when the concentration of gases is expressed in terms of their
partial pressures, then the units of the rate equation will be atm s–1 From the concentrations of C4H9Cl (butyl chloride) at different times given
below, calculate the average rate of the reaction:
C4H9Cl + H2O ® C4H9OH + HCl
during different intervals of time t/s
0
50
100
150
200
300
400
700
800
[C4H9Cl]/mol L–1 0 |
1 | 2847-2850 | However, in gaseous
reactions, when the concentration of gases is expressed in terms of their
partial pressures, then the units of the rate equation will be atm s–1 From the concentrations of C4H9Cl (butyl chloride) at different times given
below, calculate the average rate of the reaction:
C4H9Cl + H2O ® C4H9OH + HCl
during different intervals of time t/s
0
50
100
150
200
300
400
700
800
[C4H9Cl]/mol L–1 0 100 0 |
1 | 2848-2851 | From the concentrations of C4H9Cl (butyl chloride) at different times given
below, calculate the average rate of the reaction:
C4H9Cl + H2O ® C4H9OH + HCl
during different intervals of time t/s
0
50
100
150
200
300
400
700
800
[C4H9Cl]/mol L–1 0 100 0 0905 0 |
1 | 2849-2852 | t/s
0
50
100
150
200
300
400
700
800
[C4H9Cl]/mol L–1 0 100 0 0905 0 0820 0 |
1 | 2850-2853 | 100 0 0905 0 0820 0 0741 0 |
1 | 2851-2854 | 0905 0 0820 0 0741 0 0671 0 |
1 | 2852-2855 | 0820 0 0741 0 0671 0 0549 0 |
1 | 2853-2856 | 0741 0 0671 0 0549 0 0439 0 |
1 | 2854-2857 | 0671 0 0549 0 0439 0 0210 0 |
1 | 2855-2858 | 0549 0 0439 0 0210 0 017
We can determine the difference in concentration over different intervals
of time and thus determine the average rate by dividing D[R] by Dt
(Table 3 |
1 | 2856-2859 | 0439 0 0210 0 017
We can determine the difference in concentration over different intervals
of time and thus determine the average rate by dividing D[R] by Dt
(Table 3 1) |
1 | 2857-2860 | 0210 0 017
We can determine the difference in concentration over different intervals
of time and thus determine the average rate by dividing D[R] by Dt
(Table 3 1) { }
Example 3 |
1 | 2858-2861 | 017
We can determine the difference in concentration over different intervals
of time and thus determine the average rate by dividing D[R] by Dt
(Table 3 1) { }
Example 3 1
Example 3 |
1 | 2859-2862 | 1) { }
Example 3 1
Example 3 1
Example 3 |
1 | 2860-2863 | { }
Example 3 1
Example 3 1
Example 3 1
Example 3 |
1 | 2861-2864 | 1
Example 3 1
Example 3 1
Example 3 1
Example 3 |
1 | 2862-2865 | 1
Example 3 1
Example 3 1
Example 3 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
64
Chemistry
It can be seen (Table 3 |
1 | 2863-2866 | 1
Example 3 1
Example 3 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
64
Chemistry
It can be seen (Table 3 1) that the average rate falls from 1 |
1 | 2864-2867 | 1
Example 3 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
64
Chemistry
It can be seen (Table 3 1) that the average rate falls from 1 90 × 0-4 mol L-1s-1 to
0 |
1 | 2865-2868 | 1
Solution
Solution
Solution
Solution
Solution
Rationalised 2023-24
64
Chemistry
It can be seen (Table 3 1) that the average rate falls from 1 90 × 0-4 mol L-1s-1 to
0 4 × 10-4 mol L-1s-1 |
1 | 2866-2869 | 1) that the average rate falls from 1 90 × 0-4 mol L-1s-1 to
0 4 × 10-4 mol L-1s-1 However, average rate cannot be used to predict the
rate of a reaction at a particular instant as it would be constant for the
time interval for which it is calculated |
1 | 2867-2870 | 90 × 0-4 mol L-1s-1 to
0 4 × 10-4 mol L-1s-1 However, average rate cannot be used to predict the
rate of a reaction at a particular instant as it would be constant for the
time interval for which it is calculated So, to express the rate at a particular
moment of time we determine the instantaneous rate |
1 | 2868-2871 | 4 × 10-4 mol L-1s-1 However, average rate cannot be used to predict the
rate of a reaction at a particular instant as it would be constant for the
time interval for which it is calculated So, to express the rate at a particular
moment of time we determine the instantaneous rate It is obtained
when we consider the average rate at the smallest time interval say dt ( i |
1 | 2869-2872 | However, average rate cannot be used to predict the
rate of a reaction at a particular instant as it would be constant for the
time interval for which it is calculated So, to express the rate at a particular
moment of time we determine the instantaneous rate It is obtained
when we consider the average rate at the smallest time interval say dt ( i e |
1 | 2870-2873 | So, to express the rate at a particular
moment of time we determine the instantaneous rate It is obtained
when we consider the average rate at the smallest time interval say dt ( i e when Dt approaches zero) |
1 | 2871-2874 | It is obtained
when we consider the average rate at the smallest time interval say dt ( i e when Dt approaches zero) Hence, mathematically for an infinitesimally
small dt instantaneous rate is given by
[
]
[ ]
−∆
∆
=
=
∆
∆
av
R
P
r
t
t
(3 |
1 | 2872-2875 | e when Dt approaches zero) Hence, mathematically for an infinitesimally
small dt instantaneous rate is given by
[
]
[ ]
−∆
∆
=
=
∆
∆
av
R
P
r
t
t
(3 3)
As Dt ® 0
or
inst
d
d
R
P
d
d
r
t
t
Table 3 |
1 | 2873-2876 | when Dt approaches zero) Hence, mathematically for an infinitesimally
small dt instantaneous rate is given by
[
]
[ ]
−∆
∆
=
=
∆
∆
av
R
P
r
t
t
(3 3)
As Dt ® 0
or
inst
d
d
R
P
d
d
r
t
t
Table 3 1: Average rates of hydrolysis of butyl chloride
[C4H9CI]t1 /
[C4H9CI]t2 /
t1/s
t2/s
rav × 104/mol L–1s–1
mol L–1
mol L–1
[
]
[
]
(
)
{
}
= –
−
×
2
1
4
4
9
4
9
2
1
t
t
C H Cl
– C H Cl
/ t
t
10
0 |
1 | 2874-2877 | Hence, mathematically for an infinitesimally
small dt instantaneous rate is given by
[
]
[ ]
−∆
∆
=
=
∆
∆
av
R
P
r
t
t
(3 3)
As Dt ® 0
or
inst
d
d
R
P
d
d
r
t
t
Table 3 1: Average rates of hydrolysis of butyl chloride
[C4H9CI]t1 /
[C4H9CI]t2 /
t1/s
t2/s
rav × 104/mol L–1s–1
mol L–1
mol L–1
[
]
[
]
(
)
{
}
= –
−
×
2
1
4
4
9
4
9
2
1
t
t
C H Cl
– C H Cl
/ t
t
10
0 100
0 |
1 | 2875-2878 | 3)
As Dt ® 0
or
inst
d
d
R
P
d
d
r
t
t
Table 3 1: Average rates of hydrolysis of butyl chloride
[C4H9CI]t1 /
[C4H9CI]t2 /
t1/s
t2/s
rav × 104/mol L–1s–1
mol L–1
mol L–1
[
]
[
]
(
)
{
}
= –
−
×
2
1
4
4
9
4
9
2
1
t
t
C H Cl
– C H Cl
/ t
t
10
0 100
0 0905
0
50
1 |
1 | 2876-2879 | 1: Average rates of hydrolysis of butyl chloride
[C4H9CI]t1 /
[C4H9CI]t2 /
t1/s
t2/s
rav × 104/mol L–1s–1
mol L–1
mol L–1
[
]
[
]
(
)
{
}
= –
−
×
2
1
4
4
9
4
9
2
1
t
t
C H Cl
– C H Cl
/ t
t
10
0 100
0 0905
0
50
1 90
0 |
1 | 2877-2880 | 100
0 0905
0
50
1 90
0 0905
0 |
1 | 2878-2881 | 0905
0
50
1 90
0 0905
0 0820
50
100
1 |
1 | 2879-2882 | 90
0 0905
0 0820
50
100
1 70
0 |
1 | 2880-2883 | 0905
0 0820
50
100
1 70
0 0820
0 |
1 | 2881-2884 | 0820
50
100
1 70
0 0820
0 0741
100
150
1 |
1 | 2882-2885 | 70
0 0820
0 0741
100
150
1 58
0 |
1 | 2883-2886 | 0820
0 0741
100
150
1 58
0 0741
0 |
1 | 2884-2887 | 0741
100
150
1 58
0 0741
0 0671
150
200
1 |
1 | 2885-2888 | 58
0 0741
0 0671
150
200
1 40
0 |
1 | 2886-2889 | 0741
0 0671
150
200
1 40
0 0671
0 |
1 | 2887-2890 | 0671
150
200
1 40
0 0671
0 0549
200
300
1 |
1 | 2888-2891 | 40
0 0671
0 0549
200
300
1 22
0 |
1 | 2889-2892 | 0671
0 0549
200
300
1 22
0 0549
0 |
1 | 2890-2893 | 0549
200
300
1 22
0 0549
0 0439
300
400
1 |
1 | 2891-2894 | 22
0 0549
0 0439
300
400
1 10
0 |
1 | 2892-2895 | 0549
0 0439
300
400
1 10
0 0439
0 |
1 | 2893-2896 | 0439
300
400
1 10
0 0439
0 0335
400
500
1 |
1 | 2894-2897 | 10
0 0439
0 0335
400
500
1 04
0 |
1 | 2895-2898 | 0439
0 0335
400
500
1 04
0 0210
0 |
1 | 2896-2899 | 0335
400
500
1 04
0 0210
0 017
700
800
0 |
1 | 2897-2900 | 04
0 0210
0 017
700
800
0 4
Fig 3 |
1 | 2898-2901 | 0210
0 017
700
800
0 4
Fig 3 2
Instantaneous rate
of hydrolysis of butyl
chloride(C4H9Cl)
Rationalised 2023-24
65
Chemical Kinetics
It can be determined graphically by drawing a tangent at time t on
either of the curves for concentration of R and P vs time t and calculating
its slope (Fig |
1 | 2899-2902 | 017
700
800
0 4
Fig 3 2
Instantaneous rate
of hydrolysis of butyl
chloride(C4H9Cl)
Rationalised 2023-24
65
Chemical Kinetics
It can be determined graphically by drawing a tangent at time t on
either of the curves for concentration of R and P vs time t and calculating
its slope (Fig 3 |
1 | 2900-2903 | 4
Fig 3 2
Instantaneous rate
of hydrolysis of butyl
chloride(C4H9Cl)
Rationalised 2023-24
65
Chemical Kinetics
It can be determined graphically by drawing a tangent at time t on
either of the curves for concentration of R and P vs time t and calculating
its slope (Fig 3 1) |
1 | 2901-2904 | 2
Instantaneous rate
of hydrolysis of butyl
chloride(C4H9Cl)
Rationalised 2023-24
65
Chemical Kinetics
It can be determined graphically by drawing a tangent at time t on
either of the curves for concentration of R and P vs time t and calculating
its slope (Fig 3 1) So in problem 3 |
1 | 2902-2905 | 3 1) So in problem 3 1, rinst at 600s for example, can be
calculated by plotting concentration of butyl chloride as a function of
time |
1 | 2903-2906 | 1) So in problem 3 1, rinst at 600s for example, can be
calculated by plotting concentration of butyl chloride as a function of
time A tangent is drawn that touches the curve at t = 600 s (Fig |
1 | 2904-2907 | So in problem 3 1, rinst at 600s for example, can be
calculated by plotting concentration of butyl chloride as a function of
time A tangent is drawn that touches the curve at t = 600 s (Fig 3 |
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