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1 | 3005-3008 | Thus, we can say that:
Rate law for any reaction cannot be predicted by merely looking at
the balanced chemical equation, i e , theoretically but must be determined
experimentally In the rate equation (3 |
1 | 3006-3009 | e , theoretically but must be determined
experimentally In the rate equation (3 4)
Rate = k [A]x [B]y
x and y indicate how sensitive the rate is to the change in concentration
of A and B |
1 | 3007-3010 | , theoretically but must be determined
experimentally In the rate equation (3 4)
Rate = k [A]x [B]y
x and y indicate how sensitive the rate is to the change in concentration
of A and B Sum of these exponents, i |
1 | 3008-3011 | In the rate equation (3 4)
Rate = k [A]x [B]y
x and y indicate how sensitive the rate is to the change in concentration
of A and B Sum of these exponents, i e |
1 | 3009-3012 | 4)
Rate = k [A]x [B]y
x and y indicate how sensitive the rate is to the change in concentration
of A and B Sum of these exponents, i e , x + y in (3 |
1 | 3010-3013 | Sum of these exponents, i e , x + y in (3 4) gives the overall
order of a reaction whereas x and y represent the order with respect
to the reactants A and B respectively |
1 | 3011-3014 | e , x + y in (3 4) gives the overall
order of a reaction whereas x and y represent the order with respect
to the reactants A and B respectively Hence, the sum of powers of the concentration of the
reactants in the rate law expression is called the order of that
chemical reaction |
1 | 3012-3015 | , x + y in (3 4) gives the overall
order of a reaction whereas x and y represent the order with respect
to the reactants A and B respectively Hence, the sum of powers of the concentration of the
reactants in the rate law expression is called the order of that
chemical reaction Order of a reaction can be 0, 1, 2, 3 and even a fraction |
1 | 3013-3016 | 4) gives the overall
order of a reaction whereas x and y represent the order with respect
to the reactants A and B respectively Hence, the sum of powers of the concentration of the
reactants in the rate law expression is called the order of that
chemical reaction Order of a reaction can be 0, 1, 2, 3 and even a fraction A zero
order reaction means that the rate of reaction is independent of the
concentration of reactants |
1 | 3014-3017 | Hence, the sum of powers of the concentration of the
reactants in the rate law expression is called the order of that
chemical reaction Order of a reaction can be 0, 1, 2, 3 and even a fraction A zero
order reaction means that the rate of reaction is independent of the
concentration of reactants 3 |
1 | 3015-3018 | Order of a reaction can be 0, 1, 2, 3 and even a fraction A zero
order reaction means that the rate of reaction is independent of the
concentration of reactants 3 2 |
1 | 3016-3019 | A zero
order reaction means that the rate of reaction is independent of the
concentration of reactants 3 2 3 Order of a
Reaction
Calculate the overall order of a reaction which
has the rate expression
(a) Rate = k [A]1/2 [B]3/2
(b) Rate = k [A]3/2 [B]–1
(a) Rate = k [A]x [B]y
order = x + y
So order = 1/2 + 3/2 = 2, i |
1 | 3017-3020 | 3 2 3 Order of a
Reaction
Calculate the overall order of a reaction which
has the rate expression
(a) Rate = k [A]1/2 [B]3/2
(b) Rate = k [A]3/2 [B]–1
(a) Rate = k [A]x [B]y
order = x + y
So order = 1/2 + 3/2 = 2, i e |
1 | 3018-3021 | 2 3 Order of a
Reaction
Calculate the overall order of a reaction which
has the rate expression
(a) Rate = k [A]1/2 [B]3/2
(b) Rate = k [A]3/2 [B]–1
(a) Rate = k [A]x [B]y
order = x + y
So order = 1/2 + 3/2 = 2, i e , second order
(b) order = 3/2 + (–1) = 1/2, i |
1 | 3019-3022 | 3 Order of a
Reaction
Calculate the overall order of a reaction which
has the rate expression
(a) Rate = k [A]1/2 [B]3/2
(b) Rate = k [A]3/2 [B]–1
(a) Rate = k [A]x [B]y
order = x + y
So order = 1/2 + 3/2 = 2, i e , second order
(b) order = 3/2 + (–1) = 1/2, i e |
1 | 3020-3023 | e , second order
(b) order = 3/2 + (–1) = 1/2, i e , half order |
1 | 3021-3024 | , second order
(b) order = 3/2 + (–1) = 1/2, i e , half order Example 3 |
1 | 3022-3025 | e , half order Example 3 3
Example 3 |
1 | 3023-3026 | , half order Example 3 3
Example 3 3
Example 3 |
1 | 3024-3027 | Example 3 3
Example 3 3
Example 3 3
Example 3 |
1 | 3025-3028 | 3
Example 3 3
Example 3 3
Example 3 3
Example 3 |
1 | 3026-3029 | 3
Example 3 3
Example 3 3
Example 3 3
Solution
Solution
Solution
Solution
Solution
A balanced chemical equation never gives us a true picture of how
a reaction takes place since rarely a reaction gets completed in one
step |
1 | 3027-3030 | 3
Example 3 3
Example 3 3
Solution
Solution
Solution
Solution
Solution
A balanced chemical equation never gives us a true picture of how
a reaction takes place since rarely a reaction gets completed in one
step The reactions taking place in one step are called elementary
reactions |
1 | 3028-3031 | 3
Example 3 3
Solution
Solution
Solution
Solution
Solution
A balanced chemical equation never gives us a true picture of how
a reaction takes place since rarely a reaction gets completed in one
step The reactions taking place in one step are called elementary
reactions When a sequence of elementary reactions (called mechanism)
gives us the products, the reactions are called complex reactions |
1 | 3029-3032 | 3
Solution
Solution
Solution
Solution
Solution
A balanced chemical equation never gives us a true picture of how
a reaction takes place since rarely a reaction gets completed in one
step The reactions taking place in one step are called elementary
reactions When a sequence of elementary reactions (called mechanism)
gives us the products, the reactions are called complex reactions Rationalised 2023-24
69
Chemical Kinetics
Example 3 |
1 | 3030-3033 | The reactions taking place in one step are called elementary
reactions When a sequence of elementary reactions (called mechanism)
gives us the products, the reactions are called complex reactions Rationalised 2023-24
69
Chemical Kinetics
Example 3 4
Example 3 |
1 | 3031-3034 | When a sequence of elementary reactions (called mechanism)
gives us the products, the reactions are called complex reactions Rationalised 2023-24
69
Chemical Kinetics
Example 3 4
Example 3 4
Example 3 |
1 | 3032-3035 | Rationalised 2023-24
69
Chemical Kinetics
Example 3 4
Example 3 4
Example 3 4
Example 3 |
1 | 3033-3036 | 4
Example 3 4
Example 3 4
Example 3 4
Example 3 |
1 | 3034-3037 | 4
Example 3 4
Example 3 4
Example 3 4
Solution
Solution
Solution
Solution
Solution
These may be consecutive reactions (e |
1 | 3035-3038 | 4
Example 3 4
Example 3 4
Solution
Solution
Solution
Solution
Solution
These may be consecutive reactions (e g |
1 | 3036-3039 | 4
Example 3 4
Solution
Solution
Solution
Solution
Solution
These may be consecutive reactions (e g , oxidation of ethane to CO2
and H2O passes through a series of intermediate steps in which alcohol,
aldehyde and acid are formed), reverse reactions and side reactions
(e |
1 | 3037-3040 | 4
Solution
Solution
Solution
Solution
Solution
These may be consecutive reactions (e g , oxidation of ethane to CO2
and H2O passes through a series of intermediate steps in which alcohol,
aldehyde and acid are formed), reverse reactions and side reactions
(e g |
1 | 3038-3041 | g , oxidation of ethane to CO2
and H2O passes through a series of intermediate steps in which alcohol,
aldehyde and acid are formed), reverse reactions and side reactions
(e g , nitration of phenol yields o-nitrophenol and p-nitrophenol) |
1 | 3039-3042 | , oxidation of ethane to CO2
and H2O passes through a series of intermediate steps in which alcohol,
aldehyde and acid are formed), reverse reactions and side reactions
(e g , nitration of phenol yields o-nitrophenol and p-nitrophenol) Units of rate constant
For a general reaction
aA + bB ® cC + dD
Rate = k [A]
x [B]
y
Where x + y = n = order of the reaction
k =
x
Rate
[A] [B]y
(
)
(
)
=
n
concentration
1
=
×
where [A] [B]
time
concentration
Taking SI units of concentration, mol L
–1 and time, s, the units of
k for different reaction order are listed in Table 3 |
1 | 3040-3043 | g , nitration of phenol yields o-nitrophenol and p-nitrophenol) Units of rate constant
For a general reaction
aA + bB ® cC + dD
Rate = k [A]
x [B]
y
Where x + y = n = order of the reaction
k =
x
Rate
[A] [B]y
(
)
(
)
=
n
concentration
1
=
×
where [A] [B]
time
concentration
Taking SI units of concentration, mol L
–1 and time, s, the units of
k for different reaction order are listed in Table 3 3
Table 3 |
1 | 3041-3044 | , nitration of phenol yields o-nitrophenol and p-nitrophenol) Units of rate constant
For a general reaction
aA + bB ® cC + dD
Rate = k [A]
x [B]
y
Where x + y = n = order of the reaction
k =
x
Rate
[A] [B]y
(
)
(
)
=
n
concentration
1
=
×
where [A] [B]
time
concentration
Taking SI units of concentration, mol L
–1 and time, s, the units of
k for different reaction order are listed in Table 3 3
Table 3 3: Units of rate constant
Reaction
Order
Units of rate constant
Zero order reaction
0
(
)
1
1
1
10
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
First order reaction
1
(
)
1
1
11
mol L
1
s
s
mol L
−
−
−
×
=
Second order reaction
2
(
)
1
1
1
12
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
Identify the reaction order from each of the following rate constants |
1 | 3042-3045 | Units of rate constant
For a general reaction
aA + bB ® cC + dD
Rate = k [A]
x [B]
y
Where x + y = n = order of the reaction
k =
x
Rate
[A] [B]y
(
)
(
)
=
n
concentration
1
=
×
where [A] [B]
time
concentration
Taking SI units of concentration, mol L
–1 and time, s, the units of
k for different reaction order are listed in Table 3 3
Table 3 3: Units of rate constant
Reaction
Order
Units of rate constant
Zero order reaction
0
(
)
1
1
1
10
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
First order reaction
1
(
)
1
1
11
mol L
1
s
s
mol L
−
−
−
×
=
Second order reaction
2
(
)
1
1
1
12
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
Identify the reaction order from each of the following rate constants (i) k = 2 |
1 | 3043-3046 | 3
Table 3 3: Units of rate constant
Reaction
Order
Units of rate constant
Zero order reaction
0
(
)
1
1
1
10
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
First order reaction
1
(
)
1
1
11
mol L
1
s
s
mol L
−
−
−
×
=
Second order reaction
2
(
)
1
1
1
12
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
Identify the reaction order from each of the following rate constants (i) k = 2 3 × 10–5 L mol–1 s–1
(ii) k = 3 × 10–4 s–1
(i) The unit of second order rate constant is L mol–1 s–1, therefore
k = 2 |
1 | 3044-3047 | 3: Units of rate constant
Reaction
Order
Units of rate constant
Zero order reaction
0
(
)
1
1
1
10
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
First order reaction
1
(
)
1
1
11
mol L
1
s
s
mol L
−
−
−
×
=
Second order reaction
2
(
)
1
1
1
12
mol L
1
mol L s
s
mol L
−
−
−
−
×
=
Identify the reaction order from each of the following rate constants (i) k = 2 3 × 10–5 L mol–1 s–1
(ii) k = 3 × 10–4 s–1
(i) The unit of second order rate constant is L mol–1 s–1, therefore
k = 2 3 × 10–5 L mol–1 s–1 represents a second order reaction |
1 | 3045-3048 | (i) k = 2 3 × 10–5 L mol–1 s–1
(ii) k = 3 × 10–4 s–1
(i) The unit of second order rate constant is L mol–1 s–1, therefore
k = 2 3 × 10–5 L mol–1 s–1 represents a second order reaction (ii) The unit of a first order rate constant is s–1 therefore
k = 3 × 10–4 s–1 represents a first order reaction |
1 | 3046-3049 | 3 × 10–5 L mol–1 s–1
(ii) k = 3 × 10–4 s–1
(i) The unit of second order rate constant is L mol–1 s–1, therefore
k = 2 3 × 10–5 L mol–1 s–1 represents a second order reaction (ii) The unit of a first order rate constant is s–1 therefore
k = 3 × 10–4 s–1 represents a first order reaction 3 |
1 | 3047-3050 | 3 × 10–5 L mol–1 s–1 represents a second order reaction (ii) The unit of a first order rate constant is s–1 therefore
k = 3 × 10–4 s–1 represents a first order reaction 3 2 |
1 | 3048-3051 | (ii) The unit of a first order rate constant is s–1 therefore
k = 3 × 10–4 s–1 represents a first order reaction 3 2 4 Molecularity
of a
Reaction
Another property of a reaction called molecularity helps in
understanding its mechanism |
1 | 3049-3052 | 3 2 4 Molecularity
of a
Reaction
Another property of a reaction called molecularity helps in
understanding its mechanism The number of reacting species
(atoms, ions or molecules) taking part in an elementary
reaction, which must collide simultaneously in order to bring
about a chemical reaction is called molecularity of a reaction |
1 | 3050-3053 | 2 4 Molecularity
of a
Reaction
Another property of a reaction called molecularity helps in
understanding its mechanism The number of reacting species
(atoms, ions or molecules) taking part in an elementary
reaction, which must collide simultaneously in order to bring
about a chemical reaction is called molecularity of a reaction The reaction can be unimolecular when one reacting species is involved,
for example, decomposition of ammonium nitrite |
1 | 3051-3054 | 4 Molecularity
of a
Reaction
Another property of a reaction called molecularity helps in
understanding its mechanism The number of reacting species
(atoms, ions or molecules) taking part in an elementary
reaction, which must collide simultaneously in order to bring
about a chemical reaction is called molecularity of a reaction The reaction can be unimolecular when one reacting species is involved,
for example, decomposition of ammonium nitrite Rationalised 2023-24
70
Chemistry
NH4NO2 ® N2 + 2H2O
Bimolecular reactions involve simultaneous collision between two
species, for example, dissociation of hydrogen iodide |
1 | 3052-3055 | The number of reacting species
(atoms, ions or molecules) taking part in an elementary
reaction, which must collide simultaneously in order to bring
about a chemical reaction is called molecularity of a reaction The reaction can be unimolecular when one reacting species is involved,
for example, decomposition of ammonium nitrite Rationalised 2023-24
70
Chemistry
NH4NO2 ® N2 + 2H2O
Bimolecular reactions involve simultaneous collision between two
species, for example, dissociation of hydrogen iodide 2HI ® H2 + I2
Trimolecular or termolecular reactions involve simultaneous collision
between three reacting species, for example,
2NO + O2 ® 2NO2
The probability that more than three molecules can collide and
react simultaneously is very small |
1 | 3053-3056 | The reaction can be unimolecular when one reacting species is involved,
for example, decomposition of ammonium nitrite Rationalised 2023-24
70
Chemistry
NH4NO2 ® N2 + 2H2O
Bimolecular reactions involve simultaneous collision between two
species, for example, dissociation of hydrogen iodide 2HI ® H2 + I2
Trimolecular or termolecular reactions involve simultaneous collision
between three reacting species, for example,
2NO + O2 ® 2NO2
The probability that more than three molecules can collide and
react simultaneously is very small Hence, reactions with the
molecularity three are very rare and slow to proceed |
1 | 3054-3057 | Rationalised 2023-24
70
Chemistry
NH4NO2 ® N2 + 2H2O
Bimolecular reactions involve simultaneous collision between two
species, for example, dissociation of hydrogen iodide 2HI ® H2 + I2
Trimolecular or termolecular reactions involve simultaneous collision
between three reacting species, for example,
2NO + O2 ® 2NO2
The probability that more than three molecules can collide and
react simultaneously is very small Hence, reactions with the
molecularity three are very rare and slow to proceed It is, therefore, evident that complex reactions involving more than
three molecules in the stoichiometric equation must take place in more
than one step |
1 | 3055-3058 | 2HI ® H2 + I2
Trimolecular or termolecular reactions involve simultaneous collision
between three reacting species, for example,
2NO + O2 ® 2NO2
The probability that more than three molecules can collide and
react simultaneously is very small Hence, reactions with the
molecularity three are very rare and slow to proceed It is, therefore, evident that complex reactions involving more than
three molecules in the stoichiometric equation must take place in more
than one step KClO3 + 6FeSO4 + 3H2SO4 ® KCl + 3Fe2(SO4)3 + 3H2O
This reaction which apparently seems to be of tenth order is actually
a second order reaction |
1 | 3056-3059 | Hence, reactions with the
molecularity three are very rare and slow to proceed It is, therefore, evident that complex reactions involving more than
three molecules in the stoichiometric equation must take place in more
than one step KClO3 + 6FeSO4 + 3H2SO4 ® KCl + 3Fe2(SO4)3 + 3H2O
This reaction which apparently seems to be of tenth order is actually
a second order reaction This shows that this reaction takes place in
several steps |
1 | 3057-3060 | It is, therefore, evident that complex reactions involving more than
three molecules in the stoichiometric equation must take place in more
than one step KClO3 + 6FeSO4 + 3H2SO4 ® KCl + 3Fe2(SO4)3 + 3H2O
This reaction which apparently seems to be of tenth order is actually
a second order reaction This shows that this reaction takes place in
several steps Which step controls the rate of the overall reaction |
1 | 3058-3061 | KClO3 + 6FeSO4 + 3H2SO4 ® KCl + 3Fe2(SO4)3 + 3H2O
This reaction which apparently seems to be of tenth order is actually
a second order reaction This shows that this reaction takes place in
several steps Which step controls the rate of the overall reaction The
question can be answered if we go through the mechanism of reaction,
for example, chances to win the relay race competition by a team
depend upon the slowest person in the team |
1 | 3059-3062 | This shows that this reaction takes place in
several steps Which step controls the rate of the overall reaction The
question can be answered if we go through the mechanism of reaction,
for example, chances to win the relay race competition by a team
depend upon the slowest person in the team Similarly, the overall rate
of the reaction is controlled by the slowest step in a reaction called the
rate determining step |
1 | 3060-3063 | Which step controls the rate of the overall reaction The
question can be answered if we go through the mechanism of reaction,
for example, chances to win the relay race competition by a team
depend upon the slowest person in the team Similarly, the overall rate
of the reaction is controlled by the slowest step in a reaction called the
rate determining step Consider the decomposition of hydrogen
peroxide which is catalysed by iodide ion in an alkaline medium |
1 | 3061-3064 | The
question can be answered if we go through the mechanism of reaction,
for example, chances to win the relay race competition by a team
depend upon the slowest person in the team Similarly, the overall rate
of the reaction is controlled by the slowest step in a reaction called the
rate determining step Consider the decomposition of hydrogen
peroxide which is catalysed by iodide ion in an alkaline medium 2H2O2
-I
Alkaline medium
2H2O + O2
The rate equation for this reaction is found to be
2
2
2
2
d H O
Rate
H O
I
d
k
t
This reaction is first order with respect to both H2O2 and I– |
1 | 3062-3065 | Similarly, the overall rate
of the reaction is controlled by the slowest step in a reaction called the
rate determining step Consider the decomposition of hydrogen
peroxide which is catalysed by iodide ion in an alkaline medium 2H2O2
-I
Alkaline medium
2H2O + O2
The rate equation for this reaction is found to be
2
2
2
2
d H O
Rate
H O
I
d
k
t
This reaction is first order with respect to both H2O2 and I– Evidences
suggest that this reaction takes place in two steps
(1) H2O2 + I– ® H2O + IO–
(2) H2O2 + IO– ® H2O + I– + O2
Both the steps are bimolecular elementary reactions |
1 | 3063-3066 | Consider the decomposition of hydrogen
peroxide which is catalysed by iodide ion in an alkaline medium 2H2O2
-I
Alkaline medium
2H2O + O2
The rate equation for this reaction is found to be
2
2
2
2
d H O
Rate
H O
I
d
k
t
This reaction is first order with respect to both H2O2 and I– Evidences
suggest that this reaction takes place in two steps
(1) H2O2 + I– ® H2O + IO–
(2) H2O2 + IO– ® H2O + I– + O2
Both the steps are bimolecular elementary reactions Species IO- is
called as an intermediate since it is formed during the course of the
reaction but not in the overall balanced equation |
1 | 3064-3067 | 2H2O2
-I
Alkaline medium
2H2O + O2
The rate equation for this reaction is found to be
2
2
2
2
d H O
Rate
H O
I
d
k
t
This reaction is first order with respect to both H2O2 and I– Evidences
suggest that this reaction takes place in two steps
(1) H2O2 + I– ® H2O + IO–
(2) H2O2 + IO– ® H2O + I– + O2
Both the steps are bimolecular elementary reactions Species IO- is
called as an intermediate since it is formed during the course of the
reaction but not in the overall balanced equation The first step, being
slow, is the rate determining step |
1 | 3065-3068 | Evidences
suggest that this reaction takes place in two steps
(1) H2O2 + I– ® H2O + IO–
(2) H2O2 + IO– ® H2O + I– + O2
Both the steps are bimolecular elementary reactions Species IO- is
called as an intermediate since it is formed during the course of the
reaction but not in the overall balanced equation The first step, being
slow, is the rate determining step Thus, the rate of formation of
intermediate will determine the rate of this reaction |
1 | 3066-3069 | Species IO- is
called as an intermediate since it is formed during the course of the
reaction but not in the overall balanced equation The first step, being
slow, is the rate determining step Thus, the rate of formation of
intermediate will determine the rate of this reaction Thus, from the discussion, till now, we conclude the following:
(i) Order of a reaction is an experimental quantity |
1 | 3067-3070 | The first step, being
slow, is the rate determining step Thus, the rate of formation of
intermediate will determine the rate of this reaction Thus, from the discussion, till now, we conclude the following:
(i) Order of a reaction is an experimental quantity It can be zero and
even a fraction but molecularity cannot be zero or a non integer |
1 | 3068-3071 | Thus, the rate of formation of
intermediate will determine the rate of this reaction Thus, from the discussion, till now, we conclude the following:
(i) Order of a reaction is an experimental quantity It can be zero and
even a fraction but molecularity cannot be zero or a non integer (ii) Order is applicable to elementary as well as complex reactions
whereas molecularity is applicable only for elementary reactions |
1 | 3069-3072 | Thus, from the discussion, till now, we conclude the following:
(i) Order of a reaction is an experimental quantity It can be zero and
even a fraction but molecularity cannot be zero or a non integer (ii) Order is applicable to elementary as well as complex reactions
whereas molecularity is applicable only for elementary reactions For complex reaction molecularity has no meaning |
1 | 3070-3073 | It can be zero and
even a fraction but molecularity cannot be zero or a non integer (ii) Order is applicable to elementary as well as complex reactions
whereas molecularity is applicable only for elementary reactions For complex reaction molecularity has no meaning Rationalised 2023-24
71
Chemical Kinetics
(iii) For complex reaction, order is given by the slowest step and
molecularity of the slowest step is same as the order of the overall
reaction |
1 | 3071-3074 | (ii) Order is applicable to elementary as well as complex reactions
whereas molecularity is applicable only for elementary reactions For complex reaction molecularity has no meaning Rationalised 2023-24
71
Chemical Kinetics
(iii) For complex reaction, order is given by the slowest step and
molecularity of the slowest step is same as the order of the overall
reaction Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 |
1 | 3072-3075 | For complex reaction molecularity has no meaning Rationalised 2023-24
71
Chemical Kinetics
(iii) For complex reaction, order is given by the slowest step and
molecularity of the slowest step is same as the order of the overall
reaction Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 3 For a reaction, A + B ® Product; the rate law is given by, r = k [ A]1/2 [B]2 |
1 | 3073-3076 | Rationalised 2023-24
71
Chemical Kinetics
(iii) For complex reaction, order is given by the slowest step and
molecularity of the slowest step is same as the order of the overall
reaction Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 3 For a reaction, A + B ® Product; the rate law is given by, r = k [ A]1/2 [B]2 What is the order of the reaction |
1 | 3074-3077 | Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 3 For a reaction, A + B ® Product; the rate law is given by, r = k [ A]1/2 [B]2 What is the order of the reaction 3 |
1 | 3075-3078 | 3 For a reaction, A + B ® Product; the rate law is given by, r = k [ A]1/2 [B]2 What is the order of the reaction 3 4 The conversion of molecules X to Y follows second order kinetics |
1 | 3076-3079 | What is the order of the reaction 3 4 The conversion of molecules X to Y follows second order kinetics If
concentration of X is increased to three times how will it affect the rate of
formation of Y |
1 | 3077-3080 | 3 4 The conversion of molecules X to Y follows second order kinetics If
concentration of X is increased to three times how will it affect the rate of
formation of Y We have already noted that the concentration dependence of rate is
called differential rate equation |
1 | 3078-3081 | 4 The conversion of molecules X to Y follows second order kinetics If
concentration of X is increased to three times how will it affect the rate of
formation of Y We have already noted that the concentration dependence of rate is
called differential rate equation It is not always convenient to
determine the instantaneous rate, as it is measured by determination
of slope of the tangent at point ‘t’ in concentration vs time plot
(Fig |
1 | 3079-3082 | If
concentration of X is increased to three times how will it affect the rate of
formation of Y We have already noted that the concentration dependence of rate is
called differential rate equation It is not always convenient to
determine the instantaneous rate, as it is measured by determination
of slope of the tangent at point ‘t’ in concentration vs time plot
(Fig 3 |
1 | 3080-3083 | We have already noted that the concentration dependence of rate is
called differential rate equation It is not always convenient to
determine the instantaneous rate, as it is measured by determination
of slope of the tangent at point ‘t’ in concentration vs time plot
(Fig 3 1) |
1 | 3081-3084 | It is not always convenient to
determine the instantaneous rate, as it is measured by determination
of slope of the tangent at point ‘t’ in concentration vs time plot
(Fig 3 1) This makes it difficult to determine the rate law and hence
the order of the reaction |
1 | 3082-3085 | 3 1) This makes it difficult to determine the rate law and hence
the order of the reaction In order to avoid this difficulty, we can
integrate the differential rate equation to give a relation between directly
measured experimental data, i |
1 | 3083-3086 | 1) This makes it difficult to determine the rate law and hence
the order of the reaction In order to avoid this difficulty, we can
integrate the differential rate equation to give a relation between directly
measured experimental data, i e |
1 | 3084-3087 | This makes it difficult to determine the rate law and hence
the order of the reaction In order to avoid this difficulty, we can
integrate the differential rate equation to give a relation between directly
measured experimental data, i e , concentrations at different times
and rate constant |
1 | 3085-3088 | In order to avoid this difficulty, we can
integrate the differential rate equation to give a relation between directly
measured experimental data, i e , concentrations at different times
and rate constant The integrated rate equations are different for the reactions of different
reaction orders |
1 | 3086-3089 | e , concentrations at different times
and rate constant The integrated rate equations are different for the reactions of different
reaction orders We shall determine these equations only for zero and
first order chemical reactions |
1 | 3087-3090 | , concentrations at different times
and rate constant The integrated rate equations are different for the reactions of different
reaction orders We shall determine these equations only for zero and
first order chemical reactions Zero order reaction means that the rate of the reaction is proportional
to zero power of the concentration of reactants |
1 | 3088-3091 | The integrated rate equations are different for the reactions of different
reaction orders We shall determine these equations only for zero and
first order chemical 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
Rate =
0
d R
R
d
k
t
As any quantity raised to power zero is unity
Rate =
d R
1
d
k ×
t
d[R] = – k dt
Integrating both sides
[R]
= – k t + I
(3 |
1 | 3089-3092 | We shall determine these equations only for zero and
first order chemical 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
Rate =
0
d R
R
d
k
t
As any quantity raised to power zero is unity
Rate =
d R
1
d
k ×
t
d[R] = – k dt
Integrating both sides
[R]
= – k t + I
(3 5)
where, I is the constant of integration |
1 | 3090-3093 | 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
Rate =
0
d R
R
d
k
t
As any quantity raised to power zero is unity
Rate =
d R
1
d
k ×
t
d[R] = – k dt
Integrating both sides
[R]
= – k t + I
(3 5)
where, I is the constant of integration At t = 0, the concentration of the reactant R = [R]0, where [R]0 is
initial concentration of the reactant |
1 | 3091-3094 | Consider the reaction,
R ® P
Rate =
0
d R
R
d
k
t
As any quantity raised to power zero is unity
Rate =
d R
1
d
k ×
t
d[R] = – k dt
Integrating both sides
[R]
= – k t + I
(3 5)
where, I is the constant of integration At t = 0, the concentration of the reactant R = [R]0, where [R]0 is
initial concentration of the reactant Substituting in equation (3 |
1 | 3092-3095 | 5)
where, I is the constant of integration At t = 0, the concentration of the reactant R = [R]0, where [R]0 is
initial concentration of the reactant Substituting in equation (3 5)
[R]0
= –k × 0 + I
[R]0
= I
Substituting the value of I in the equation (3 |
1 | 3093-3096 | At t = 0, the concentration of the reactant R = [R]0, where [R]0 is
initial concentration of the reactant Substituting in equation (3 5)
[R]0
= –k × 0 + I
[R]0
= I
Substituting the value of I in the equation (3 5)
[R]
= -kt + [R]0
(3 |
1 | 3094-3097 | Substituting in equation (3 5)
[R]0
= –k × 0 + I
[R]0
= I
Substituting the value of I in the equation (3 5)
[R]
= -kt + [R]0
(3 6)
3 |
1 | 3095-3098 | 5)
[R]0
= –k × 0 + I
[R]0
= I
Substituting the value of I in the equation (3 5)
[R]
= -kt + [R]0
(3 6)
3 3
3 |
1 | 3096-3099 | 5)
[R]
= -kt + [R]0
(3 6)
3 3
3 3
3 |
1 | 3097-3100 | 6)
3 3
3 3
3 3
3 |
1 | 3098-3101 | 3
3 3
3 3
3 3
3 |
1 | 3099-3102 | 3
3 3
3 3
3 3 Integrated
Integrated
Integrated
Integrated
Integrated
Rate
Rate
Rate
Rate
Rate
Equations
Equations
Equations
Equations
Equations
3 |
1 | 3100-3103 | 3
3 3
3 3 Integrated
Integrated
Integrated
Integrated
Integrated
Rate
Rate
Rate
Rate
Rate
Equations
Equations
Equations
Equations
Equations
3 3 |
1 | 3101-3104 | 3
3 3 Integrated
Integrated
Integrated
Integrated
Integrated
Rate
Rate
Rate
Rate
Rate
Equations
Equations
Equations
Equations
Equations
3 3 1 Zero Order
Reactions
Rationalised 2023-24
72
Chemistry
Fig |
1 | 3102-3105 | 3 Integrated
Integrated
Integrated
Integrated
Integrated
Rate
Rate
Rate
Rate
Rate
Equations
Equations
Equations
Equations
Equations
3 3 1 Zero Order
Reactions
Rationalised 2023-24
72
Chemistry
Fig 3 |
1 | 3103-3106 | 3 1 Zero Order
Reactions
Rationalised 2023-24
72
Chemistry
Fig 3 3: Variation in the concentration
vs time plot for a zero order
reaction
Time
k = -slope
Concentration of R
[R ]
0
0
Comparing (3 |
1 | 3104-3107 | 1 Zero Order
Reactions
Rationalised 2023-24
72
Chemistry
Fig 3 3: Variation in the concentration
vs time plot for a zero order
reaction
Time
k = -slope
Concentration of R
[R ]
0
0
Comparing (3 6) with equation of a straight line,
y = mx + c, if we plot [R] against t, we get a straight
line (Fig |
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