Chapter
stringclasses 18
values | sentence_range
stringlengths 3
9
| Text
stringlengths 7
7.34k
|
|---|---|---|
1 | 2905-2908 | 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 2) |
1 | 2906-2909 | A tangent is drawn that touches the curve at t = 600 s (Fig 3 2) The slope of this tangent gives the instantaneous rate |
1 | 2907-2910 | 3 2) The slope of this tangent gives the instantaneous rate So, rinst at 600 s = –
mol L–1 = 5 |
1 | 2908-2911 | 2) The slope of this tangent gives the instantaneous rate So, rinst at 600 s = –
mol L–1 = 5 12 × 10–5 mol L–1s–1
At t = 250 s
rinst = 1 |
1 | 2909-2912 | The slope of this tangent gives the instantaneous rate So, rinst at 600 s = –
mol L–1 = 5 12 × 10–5 mol L–1s–1
At t = 250 s
rinst = 1 22 × 10–4
mol L–1s–1
t = 350 s
rinst = 1 |
1 | 2910-2913 | So, rinst at 600 s = –
mol L–1 = 5 12 × 10–5 mol L–1s–1
At t = 250 s
rinst = 1 22 × 10–4
mol L–1s–1
t = 350 s
rinst = 1 0 × 10–4 mol L–1s–1
t = 450 s
rinst = 6 |
1 | 2911-2914 | 12 × 10–5 mol L–1s–1
At t = 250 s
rinst = 1 22 × 10–4
mol L–1s–1
t = 350 s
rinst = 1 0 × 10–4 mol L–1s–1
t = 450 s
rinst = 6 4 ×× 10–5 mol L–1s–1
Now consider a reaction
Hg(l) + Cl2 (g) ® HgCl2(s)
Where stoichiometric coefficients of the reactants and products are
same, then rate of the reaction is given as
[
]
[
]
[
]
2
2
Hg
Cl
HgCl
Rate of reaction = –
–
t
t
t
∆
∆
∆
=
=
∆
∆
∆
i |
1 | 2912-2915 | 22 × 10–4
mol L–1s–1
t = 350 s
rinst = 1 0 × 10–4 mol L–1s–1
t = 450 s
rinst = 6 4 ×× 10–5 mol L–1s–1
Now consider a reaction
Hg(l) + Cl2 (g) ® HgCl2(s)
Where stoichiometric coefficients of the reactants and products are
same, then rate of the reaction is given as
[
]
[
]
[
]
2
2
Hg
Cl
HgCl
Rate of reaction = –
–
t
t
t
∆
∆
∆
=
=
∆
∆
∆
i e |
1 | 2913-2916 | 0 × 10–4 mol L–1s–1
t = 450 s
rinst = 6 4 ×× 10–5 mol L–1s–1
Now consider a reaction
Hg(l) + Cl2 (g) ® HgCl2(s)
Where stoichiometric coefficients of the reactants and products are
same, then rate of the reaction is given as
[
]
[
]
[
]
2
2
Hg
Cl
HgCl
Rate of reaction = –
–
t
t
t
∆
∆
∆
=
=
∆
∆
∆
i e , rate of disappearance of any of the reactants is same as the rate
of appearance of the products |
1 | 2914-2917 | 4 ×× 10–5 mol L–1s–1
Now consider a reaction
Hg(l) + Cl2 (g) ® HgCl2(s)
Where stoichiometric coefficients of the reactants and products are
same, then rate of the reaction is given as
[
]
[
]
[
]
2
2
Hg
Cl
HgCl
Rate of reaction = –
–
t
t
t
∆
∆
∆
=
=
∆
∆
∆
i e , rate of disappearance of any of the reactants is same as the rate
of appearance of the products But in the following reaction, two moles of
HI decompose to produce one mole each of H2 and I2,
2HI(g) ® H2(g) + I2(g)
For expressing the rate of such a reaction where stoichiometric
coefficients of reactants or products are not equal to one, rate of
disappearance of any of the reactants or the rate of appearance of
products is divided by their respective stoichiometric coefficients |
1 | 2915-2918 | e , rate of disappearance of any of the reactants is same as the rate
of appearance of the products But in the following reaction, two moles of
HI decompose to produce one mole each of H2 and I2,
2HI(g) ® H2(g) + I2(g)
For expressing the rate of such a reaction where stoichiometric
coefficients of reactants or products are not equal to one, rate of
disappearance of any of the reactants or the rate of appearance of
products is divided by their respective stoichiometric coefficients Since
rate of consumption of HI is twice the rate of formation of H2 or I2, to
make them equal, the term D[HI] is divided by 2 |
1 | 2916-2919 | , rate of disappearance of any of the reactants is same as the rate
of appearance of the products But in the following reaction, two moles of
HI decompose to produce one mole each of H2 and I2,
2HI(g) ® H2(g) + I2(g)
For expressing the rate of such a reaction where stoichiometric
coefficients of reactants or products are not equal to one, rate of
disappearance of any of the reactants or the rate of appearance of
products is divided by their respective stoichiometric coefficients Since
rate of consumption of HI is twice the rate of formation of H2 or I2, to
make them equal, the term D[HI] is divided by 2 The rate of this reaction
is given by
Rate of reaction
[
]
[
]
[ ]
2
2
H
I
1
HI
2
t
t
t
∆
∆
∆
= −
=
=
∆
∆
∆
Similarly, for the reaction
5 Br- (aq) + BrO3
– (aq) + 6 H+ (aq) ® 3 Br2 (aq) + 3 H2O (l)
Rate
Br
BrO
H
Br
H
= −
[
] = −
= −
[
] =
[
] =
−
−
+
51
61
31
1
3
3
2
2
∆
∆
∆
∆
∆
∆
∆
∆
∆
t
t
t
t
OO
[
]
∆t
For a gaseous reaction at constant temperature, concentration is
directly proportional to the partial pressure of a species and hence, rate
can also be expressed as rate of change in partial pressure of the reactant
or the product |
1 | 2917-2920 | But in the following reaction, two moles of
HI decompose to produce one mole each of H2 and I2,
2HI(g) ® H2(g) + I2(g)
For expressing the rate of such a reaction where stoichiometric
coefficients of reactants or products are not equal to one, rate of
disappearance of any of the reactants or the rate of appearance of
products is divided by their respective stoichiometric coefficients Since
rate of consumption of HI is twice the rate of formation of H2 or I2, to
make them equal, the term D[HI] is divided by 2 The rate of this reaction
is given by
Rate of reaction
[
]
[
]
[ ]
2
2
H
I
1
HI
2
t
t
t
∆
∆
∆
= −
=
=
∆
∆
∆
Similarly, for the reaction
5 Br- (aq) + BrO3
– (aq) + 6 H+ (aq) ® 3 Br2 (aq) + 3 H2O (l)
Rate
Br
BrO
H
Br
H
= −
[
] = −
= −
[
] =
[
] =
−
−
+
51
61
31
1
3
3
2
2
∆
∆
∆
∆
∆
∆
∆
∆
∆
t
t
t
t
OO
[
]
∆t
For a gaseous reaction at constant temperature, concentration is
directly proportional to the partial pressure of a species and hence, rate
can also be expressed as rate of change in partial pressure of the reactant
or the product Rationalised 2023-24
66
Chemistry
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 |
1 | 2918-2921 | Since
rate of consumption of HI is twice the rate of formation of H2 or I2, to
make them equal, the term D[HI] is divided by 2 The rate of this reaction
is given by
Rate of reaction
[
]
[
]
[ ]
2
2
H
I
1
HI
2
t
t
t
∆
∆
∆
= −
=
=
∆
∆
∆
Similarly, for the reaction
5 Br- (aq) + BrO3
– (aq) + 6 H+ (aq) ® 3 Br2 (aq) + 3 H2O (l)
Rate
Br
BrO
H
Br
H
= −
[
] = −
= −
[
] =
[
] =
−
−
+
51
61
31
1
3
3
2
2
∆
∆
∆
∆
∆
∆
∆
∆
∆
t
t
t
t
OO
[
]
∆t
For a gaseous reaction at constant temperature, concentration is
directly proportional to the partial pressure of a species and hence, rate
can also be expressed as rate of change in partial pressure of the reactant
or the product Rationalised 2023-24
66
Chemistry
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 1 For the reaction R ® P, the concentration of a reactant changes from 0 |
1 | 2919-2922 | The rate of this reaction
is given by
Rate of reaction
[
]
[
]
[ ]
2
2
H
I
1
HI
2
t
t
t
∆
∆
∆
= −
=
=
∆
∆
∆
Similarly, for the reaction
5 Br- (aq) + BrO3
– (aq) + 6 H+ (aq) ® 3 Br2 (aq) + 3 H2O (l)
Rate
Br
BrO
H
Br
H
= −
[
] = −
= −
[
] =
[
] =
−
−
+
51
61
31
1
3
3
2
2
∆
∆
∆
∆
∆
∆
∆
∆
∆
t
t
t
t
OO
[
]
∆t
For a gaseous reaction at constant temperature, concentration is
directly proportional to the partial pressure of a species and hence, rate
can also be expressed as rate of change in partial pressure of the reactant
or the product Rationalised 2023-24
66
Chemistry
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 1 For the reaction R ® P, the concentration of a reactant changes from 0 03M
to 0 |
1 | 2920-2923 | Rationalised 2023-24
66
Chemistry
Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
3 1 For the reaction R ® P, the concentration of a reactant changes from 0 03M
to 0 02M in 25 minutes |
1 | 2921-2924 | 1 For the reaction R ® P, the concentration of a reactant changes from 0 03M
to 0 02M in 25 minutes Calculate the average rate of reaction using units
of time both in minutes and seconds |
1 | 2922-2925 | 03M
to 0 02M in 25 minutes Calculate the average rate of reaction using units
of time both in minutes and seconds 3 |
1 | 2923-2926 | 02M in 25 minutes Calculate the average rate of reaction using units
of time both in minutes and seconds 3 2 In a reaction, 2A ® Products, the concentration of A decreases from 0 |
1 | 2924-2927 | Calculate the average rate of reaction using units
of time both in minutes and seconds 3 2 In a reaction, 2A ® Products, the concentration of A decreases from 0 5
mol L–1 to 0 |
1 | 2925-2928 | 3 2 In a reaction, 2A ® Products, the concentration of A decreases from 0 5
mol L–1 to 0 4 mol L–1 in 10 minutes |
1 | 2926-2929 | 2 In a reaction, 2A ® Products, the concentration of A decreases from 0 5
mol L–1 to 0 4 mol L–1 in 10 minutes Calculate the rate during this interval |
1 | 2927-2930 | 5
mol L–1 to 0 4 mol L–1 in 10 minutes Calculate the rate during this interval Rate of reaction depends upon the experimental conditions such
as concentration of reactants (pressure in case of gases),
temperature and catalyst |
1 | 2928-2931 | 4 mol L–1 in 10 minutes Calculate the rate during this interval Rate of reaction depends upon the experimental conditions such
as concentration of reactants (pressure in case of gases),
temperature and catalyst The rate of a chemical reaction at a given temperature may depend on
the concentration of one or more reactants and products |
1 | 2929-2932 | Calculate the rate during this interval Rate of reaction depends upon the experimental conditions such
as concentration of reactants (pressure in case of gases),
temperature and catalyst The rate of a chemical reaction at a given temperature may depend on
the concentration of one or more reactants and products The
representation of rate of reaction in terms of concentration of the
reactants is known as rate law |
1 | 2930-2933 | Rate of reaction depends upon the experimental conditions such
as concentration of reactants (pressure in case of gases),
temperature and catalyst The rate of a chemical reaction at a given temperature may depend on
the concentration of one or more reactants and products The
representation of rate of reaction in terms of concentration of the
reactants is known as rate law It is also called as rate equation or
rate expression |
1 | 2931-2934 | The rate of a chemical reaction at a given temperature may depend on
the concentration of one or more reactants and products The
representation of rate of reaction in terms of concentration of the
reactants is known as rate law It is also called as rate equation or
rate expression The results in Table 3 |
1 | 2932-2935 | The
representation of rate of reaction in terms of concentration of the
reactants is known as rate law It is also called as rate equation or
rate expression The results in Table 3 1 clearly show that rate of a reaction decreases with
the passage of time as the concentration of reactants decrease |
1 | 2933-2936 | It is also called as rate equation or
rate expression The results in Table 3 1 clearly show that rate of a reaction decreases with
the passage of time as the concentration of reactants decrease Conversely,
rates generally increase when reactant concentrations increase |
1 | 2934-2937 | The results in Table 3 1 clearly show that rate of a reaction decreases with
the passage of time as the concentration of reactants decrease Conversely,
rates generally increase when reactant concentrations increase So, rate of
a reaction depends upon the concentration of reactants |
1 | 2935-2938 | 1 clearly show that rate of a reaction decreases with
the passage of time as the concentration of reactants decrease Conversely,
rates generally increase when reactant concentrations increase So, rate of
a reaction depends upon the concentration of reactants Example 3 |
1 | 2936-2939 | Conversely,
rates generally increase when reactant concentrations increase So, rate of
a reaction depends upon the concentration of reactants Example 3 2
Example 3 |
1 | 2937-2940 | So, rate of
a reaction depends upon the concentration of reactants Example 3 2
Example 3 2
Example 3 |
1 | 2938-2941 | Example 3 2
Example 3 2
Example 3 2
Example 3 |
1 | 2939-2942 | 2
Example 3 2
Example 3 2
Example 3 2
Example 3 |
1 | 2940-2943 | 2
Example 3 2
Example 3 2
Example 3 2
3 |
1 | 2941-2944 | 2
Example 3 2
Example 3 2
3 2 |
1 | 2942-2945 | 2
Example 3 2
3 2 2 Rate
Expression
and Rate
Constant
The decomposition of N2O5 in CCl4 at 318K has been studied by
monitoring the concentration of N2O5 in the solution |
1 | 2943-2946 | 2
3 2 2 Rate
Expression
and Rate
Constant
The decomposition of N2O5 in CCl4 at 318K has been studied by
monitoring the concentration of N2O5 in the solution Initially the
concentration of N2O5 is 2 |
1 | 2944-2947 | 2 2 Rate
Expression
and Rate
Constant
The decomposition of N2O5 in CCl4 at 318K has been studied by
monitoring the concentration of N2O5 in the solution Initially the
concentration of N2O5 is 2 33 mol L–1 and after 184 minutes, it is reduced
to 2 |
1 | 2945-2948 | 2 Rate
Expression
and Rate
Constant
The decomposition of N2O5 in CCl4 at 318K has been studied by
monitoring the concentration of N2O5 in the solution Initially the
concentration of N2O5 is 2 33 mol L–1 and after 184 minutes, it is reduced
to 2 08 mol L–1 |
1 | 2946-2949 | Initially the
concentration of N2O5 is 2 33 mol L–1 and after 184 minutes, it is reduced
to 2 08 mol L–1 The reaction takes place according to the equation
2 N2O5 (g) ® 4 NO2 (g) + O2 (g)
Calculate the average rate of this reaction in terms of hours, minutes
and seconds |
1 | 2947-2950 | 33 mol L–1 and after 184 minutes, it is reduced
to 2 08 mol L–1 The reaction takes place according to the equation
2 N2O5 (g) ® 4 NO2 (g) + O2 (g)
Calculate the average rate of this reaction in terms of hours, minutes
and seconds What is the rate of production of NO2 during this period |
1 | 2948-2951 | 08 mol L–1 The reaction takes place according to the equation
2 N2O5 (g) ® 4 NO2 (g) + O2 (g)
Calculate the average rate of this reaction in terms of hours, minutes
and seconds What is the rate of production of NO2 during this period Average Rate =
−
[
]
= −
−
(
)
−
21
21
2 08
2 33
184
2
5
1
∆
∆
N O
mol L
t |
1 | 2949-2952 | The reaction takes place according to the equation
2 N2O5 (g) ® 4 NO2 (g) + O2 (g)
Calculate the average rate of this reaction in terms of hours, minutes
and seconds What is the rate of production of NO2 during this period Average Rate =
−
[
]
= −
−
(
)
−
21
21
2 08
2 33
184
2
5
1
∆
∆
N O
mol L
t min
=
6 |
1 | 2950-2953 | What is the rate of production of NO2 during this period Average Rate =
−
[
]
= −
−
(
)
−
21
21
2 08
2 33
184
2
5
1
∆
∆
N O
mol L
t min
=
6 79 × 10–4 mol L–1/min = (6 |
1 | 2951-2954 | Average Rate =
−
[
]
= −
−
(
)
−
21
21
2 08
2 33
184
2
5
1
∆
∆
N O
mol L
t min
=
6 79 × 10–4 mol L–1/min = (6 79 × 10–4 mol L–1 min–1) × (60 min/1h)
=
4 |
1 | 2952-2955 | min
=
6 79 × 10–4 mol L–1/min = (6 79 × 10–4 mol L–1 min–1) × (60 min/1h)
=
4 07 × 10–2 mol L–1/h
=
6 |
1 | 2953-2956 | 79 × 10–4 mol L–1/min = (6 79 × 10–4 mol L–1 min–1) × (60 min/1h)
=
4 07 × 10–2 mol L–1/h
=
6 79 × 10–4 mol L–1 × 1min/60s
=
1 |
1 | 2954-2957 | 79 × 10–4 mol L–1 min–1) × (60 min/1h)
=
4 07 × 10–2 mol L–1/h
=
6 79 × 10–4 mol L–1 × 1min/60s
=
1 13 × 10–5 mol L–1s–1
It may be remembered that
Rate
NO
=
[
]
1
4
2
∆
∆t
[
2]
NO
t
∆
=
∆
6 |
1 | 2955-2958 | 07 × 10–2 mol L–1/h
=
6 79 × 10–4 mol L–1 × 1min/60s
=
1 13 × 10–5 mol L–1s–1
It may be remembered that
Rate
NO
=
[
]
1
4
2
∆
∆t
[
2]
NO
t
∆
=
∆
6 79 × 10–4 × 4 mol L–1 min–1 = 2 |
1 | 2956-2959 | 79 × 10–4 mol L–1 × 1min/60s
=
1 13 × 10–5 mol L–1s–1
It may be remembered that
Rate
NO
=
[
]
1
4
2
∆
∆t
[
2]
NO
t
∆
=
∆
6 79 × 10–4 × 4 mol L–1 min–1 = 2 72 × 10–3 mol L–1min–1
Solution
Solution
Solution
Solution
Solution
3 |
1 | 2957-2960 | 13 × 10–5 mol L–1s–1
It may be remembered that
Rate
NO
=
[
]
1
4
2
∆
∆t
[
2]
NO
t
∆
=
∆
6 79 × 10–4 × 4 mol L–1 min–1 = 2 72 × 10–3 mol L–1min–1
Solution
Solution
Solution
Solution
Solution
3 2
3 |
1 | 2958-2961 | 79 × 10–4 × 4 mol L–1 min–1 = 2 72 × 10–3 mol L–1min–1
Solution
Solution
Solution
Solution
Solution
3 2
3 2
3 |
1 | 2959-2962 | 72 × 10–3 mol L–1min–1
Solution
Solution
Solution
Solution
Solution
3 2
3 2
3 2
3 |
1 | 2960-2963 | 2
3 2
3 2
3 2
3 |
1 | 2961-2964 | 2
3 2
3 2
3 2 Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
3 |
1 | 2962-2965 | 2
3 2
3 2 Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
3 2 |
1 | 2963-2966 | 2
3 2 Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
3 2 1 Dependence
of Rate on
Concentration
Rationalised 2023-24
67
Chemical Kinetics
Consider a general reaction
aA + bB ® cC + dD
where a, b, c and d are the stoichiometric coefficients of reactants
and products |
1 | 2964-2967 | 2 Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Factors Influencing
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
Rate of a Reaction
3 2 1 Dependence
of Rate on
Concentration
Rationalised 2023-24
67
Chemical Kinetics
Consider a general reaction
aA + bB ® cC + dD
where a, b, c and d are the stoichiometric coefficients of reactants
and products The rate expression for this reaction is
Rate µ [A]
x [B]
y
(3 |
1 | 2965-2968 | 2 1 Dependence
of Rate on
Concentration
Rationalised 2023-24
67
Chemical Kinetics
Consider a general reaction
aA + bB ® cC + dD
where a, b, c and d are the stoichiometric coefficients of reactants
and products The rate expression for this reaction is
Rate µ [A]
x [B]
y
(3 4)
where exponents x and y may or may not be equal to the
stoichiometric coefficients (a and b) of the reactants |
1 | 2966-2969 | 1 Dependence
of Rate on
Concentration
Rationalised 2023-24
67
Chemical Kinetics
Consider a general reaction
aA + bB ® cC + dD
where a, b, c and d are the stoichiometric coefficients of reactants
and products The rate expression for this reaction is
Rate µ [A]
x [B]
y
(3 4)
where exponents x and y may or may not be equal to the
stoichiometric coefficients (a and b) of the reactants Above equation
can also be written as
Rate = k [A]
x [B]
y
(3 |
1 | 2967-2970 | The rate expression for this reaction is
Rate µ [A]
x [B]
y
(3 4)
where exponents x and y may or may not be equal to the
stoichiometric coefficients (a and b) of the reactants Above equation
can also be written as
Rate = k [A]
x [B]
y
(3 4a)
[
]
[
] [ ]
x
y
d R
A
B
d
k
t
−
=
(3 |
1 | 2968-2971 | 4)
where exponents x and y may or may not be equal to the
stoichiometric coefficients (a and b) of the reactants Above equation
can also be written as
Rate = k [A]
x [B]
y
(3 4a)
[
]
[
] [ ]
x
y
d R
A
B
d
k
t
−
=
(3 4b)
This form of equation (3 |
1 | 2969-2972 | Above equation
can also be written as
Rate = k [A]
x [B]
y
(3 4a)
[
]
[
] [ ]
x
y
d R
A
B
d
k
t
−
=
(3 4b)
This form of equation (3 4 b) is known as differential rate equation,
where k is a proportionality constant called rate constant |
1 | 2970-2973 | 4a)
[
]
[
] [ ]
x
y
d R
A
B
d
k
t
−
=
(3 4b)
This form of equation (3 4 b) is known as differential rate equation,
where k is a proportionality constant called rate constant The
equation like (3 |
1 | 2971-2974 | 4b)
This form of equation (3 4 b) is known as differential rate equation,
where k is a proportionality constant called rate constant The
equation like (3 4), which relates the rate of a reaction to concentration
of reactants is called rate law or rate expression |
1 | 2972-2975 | 4 b) is known as differential rate equation,
where k is a proportionality constant called rate constant The
equation like (3 4), which relates the rate of a reaction to concentration
of reactants is called rate law or rate expression 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 |
1 | 2973-2976 | The
equation like (3 4), which relates the rate of a reaction to concentration
of reactants is called rate law or rate expression 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 For example:
2NO(g) + O2(g) ® 2NO2 (g)
We can measure the rate of this reaction as a function of initial
concentrations either by keeping the concentration of one of the reactants
constant and changing the concentration of the other reactant or by
changing the concentration of both the reactants |
1 | 2974-2977 | 4), which relates the rate of a reaction to concentration
of reactants is called rate law or rate expression 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 For example:
2NO(g) + O2(g) ® 2NO2 (g)
We can measure the rate of this reaction as a function of initial
concentrations either by keeping the concentration of one of the reactants
constant and changing the concentration of the other reactant or by
changing the concentration of both the reactants The following results
are obtained (Table 3 |
1 | 2975-2978 | 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 For example:
2NO(g) + O2(g) ® 2NO2 (g)
We can measure the rate of this reaction as a function of initial
concentrations either by keeping the concentration of one of the reactants
constant and changing the concentration of the other reactant or by
changing the concentration of both the reactants The following results
are obtained (Table 3 2) |
1 | 2976-2979 | For example:
2NO(g) + O2(g) ® 2NO2 (g)
We can measure the rate of this reaction as a function of initial
concentrations either by keeping the concentration of one of the reactants
constant and changing the concentration of the other reactant or by
changing the concentration of both the reactants The following results
are obtained (Table 3 2) Table 3 |
1 | 2977-2980 | The following results
are obtained (Table 3 2) Table 3 2: Initial rate of formation of NO2
Experiment
Initial [NO]/ mol L-1
Initial [O2]/ mol L-1
Initial rate of
formation of NO2/ mol L-1s-1
1 |
1 | 2978-2981 | 2) Table 3 2: Initial rate of formation of NO2
Experiment
Initial [NO]/ mol L-1
Initial [O2]/ mol L-1
Initial rate of
formation of NO2/ mol L-1s-1
1 0 |
1 | 2979-2982 | Table 3 2: Initial rate of formation of NO2
Experiment
Initial [NO]/ mol L-1
Initial [O2]/ mol L-1
Initial rate of
formation of NO2/ mol L-1s-1
1 0 30
0 |
1 | 2980-2983 | 2: Initial rate of formation of NO2
Experiment
Initial [NO]/ mol L-1
Initial [O2]/ mol L-1
Initial rate of
formation of NO2/ mol L-1s-1
1 0 30
0 30
0 |
1 | 2981-2984 | 0 30
0 30
0 096
2 |
1 | 2982-2985 | 30
0 30
0 096
2 0 |
1 | 2983-2986 | 30
0 096
2 0 60
0 |
1 | 2984-2987 | 096
2 0 60
0 30
0 |
1 | 2985-2988 | 0 60
0 30
0 384
3 |
1 | 2986-2989 | 60
0 30
0 384
3 0 |
1 | 2987-2990 | 30
0 384
3 0 30
0 |
1 | 2988-2991 | 384
3 0 30
0 60
0 |
1 | 2989-2992 | 0 30
0 60
0 192
4 |
1 | 2990-2993 | 30
0 60
0 192
4 0 |
1 | 2991-2994 | 60
0 192
4 0 60
0 |
1 | 2992-2995 | 192
4 0 60
0 60
0 |
1 | 2993-2996 | 0 60
0 60
0 768
It is obvious, after looking at the results, that when the concentration
of NO is doubled and that of O2 is kept constant then the initial rate
increases by a factor of four from 0 |
1 | 2994-2997 | 60
0 60
0 768
It is obvious, after looking at the results, that when the concentration
of NO is doubled and that of O2 is kept constant then the initial rate
increases by a factor of four from 0 096 to 0 |
1 | 2995-2998 | 60
0 768
It is obvious, after looking at the results, that when the concentration
of NO is doubled and that of O2 is kept constant then the initial rate
increases by a factor of four from 0 096 to 0 384 mol L–1s–1 |
1 | 2996-2999 | 768
It is obvious, after looking at the results, that when the concentration
of NO is doubled and that of O2 is kept constant then the initial rate
increases by a factor of four from 0 096 to 0 384 mol L–1s–1 This
indicates that the rate depends upon the square of the concentration of
NO |
1 | 2997-3000 | 096 to 0 384 mol L–1s–1 This
indicates that the rate depends upon the square of the concentration of
NO When concentration of NO is kept constant and concentration of
O2 is doubled the rate also gets doubled indicating that rate depends
on concentration of O2 to the first power |
1 | 2998-3001 | 384 mol L–1s–1 This
indicates that the rate depends upon the square of the concentration of
NO When concentration of NO is kept constant and concentration of
O2 is doubled the rate also gets doubled indicating that rate depends
on concentration of O2 to the first power Hence, the rate equation for
this reaction will be
Rate = k [NO]
2[O2]
Rationalised 2023-24
68
Chemistry
The differential form of this rate expression is given as
[
]
[
] [
]
2
2
d R
O
NO
d
k
t
−
=
Now, we observe that for this reaction in the rate equation derived
from the experimental data, the exponents of the concentration terms
are the same as their stoichiometric coefficients in the balanced
chemical equation |
1 | 2999-3002 | This
indicates that the rate depends upon the square of the concentration of
NO When concentration of NO is kept constant and concentration of
O2 is doubled the rate also gets doubled indicating that rate depends
on concentration of O2 to the first power Hence, the rate equation for
this reaction will be
Rate = k [NO]
2[O2]
Rationalised 2023-24
68
Chemistry
The differential form of this rate expression is given as
[
]
[
] [
]
2
2
d R
O
NO
d
k
t
−
=
Now, we observe that for this reaction in the rate equation derived
from the experimental data, the exponents of the concentration terms
are the same as their stoichiometric coefficients in the balanced
chemical equation Some other examples are given below:
Reaction
Experimental rate expression
1 |
1 | 3000-3003 | When concentration of NO is kept constant and concentration of
O2 is doubled the rate also gets doubled indicating that rate depends
on concentration of O2 to the first power Hence, the rate equation for
this reaction will be
Rate = k [NO]
2[O2]
Rationalised 2023-24
68
Chemistry
The differential form of this rate expression is given as
[
]
[
] [
]
2
2
d R
O
NO
d
k
t
−
=
Now, we observe that for this reaction in the rate equation derived
from the experimental data, the exponents of the concentration terms
are the same as their stoichiometric coefficients in the balanced
chemical equation Some other examples are given below:
Reaction
Experimental rate expression
1 CHCl3 + Cl2 ® CCl4 + HCl
Rate = k [CHCl3 ] [Cl2]1/2
2 |
1 | 3001-3004 | Hence, the rate equation for
this reaction will be
Rate = k [NO]
2[O2]
Rationalised 2023-24
68
Chemistry
The differential form of this rate expression is given as
[
]
[
] [
]
2
2
d R
O
NO
d
k
t
−
=
Now, we observe that for this reaction in the rate equation derived
from the experimental data, the exponents of the concentration terms
are the same as their stoichiometric coefficients in the balanced
chemical equation Some other examples are given below:
Reaction
Experimental rate expression
1 CHCl3 + Cl2 ® CCl4 + HCl
Rate = k [CHCl3 ] [Cl2]1/2
2 CH3COOC2H5 + H2O ® CH3COOH + C2H5OH Rate = k [CH3COOC2H5]1 [H2O]0
In these reactions, the exponents of the concentration terms are not
the same as their stoichiometric coefficients |
1 | 3002-3005 | Some other examples are given below:
Reaction
Experimental rate expression
1 CHCl3 + Cl2 ® CCl4 + HCl
Rate = k [CHCl3 ] [Cl2]1/2
2 CH3COOC2H5 + H2O ® CH3COOH + C2H5OH Rate = k [CH3COOC2H5]1 [H2O]0
In these reactions, the exponents of the concentration terms are not
the same as their stoichiometric coefficients Thus, we can say that:
Rate law for any reaction cannot be predicted by merely looking at
the balanced chemical equation, i |
1 | 3003-3006 | CHCl3 + Cl2 ® CCl4 + HCl
Rate = k [CHCl3 ] [Cl2]1/2
2 CH3COOC2H5 + H2O ® CH3COOH + C2H5OH Rate = k [CH3COOC2H5]1 [H2O]0
In these reactions, the exponents of the concentration terms are not
the same as their stoichiometric coefficients Thus, we can say that:
Rate law for any reaction cannot be predicted by merely looking at
the balanced chemical equation, i e |
1 | 3004-3007 | CH3COOC2H5 + H2O ® CH3COOH + C2H5OH Rate = k [CH3COOC2H5]1 [H2O]0
In these reactions, the exponents of the concentration terms are not
the same as their stoichiometric coefficients 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 |
Subsets and Splits
No community queries yet
The top public SQL queries from the community will appear here once available.