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1 | 3505-3508 | 0 × 10–6 mol–2 L2 s–1 Calculate the initial
rate of the reaction when [A] = 0 1 mol L–1, [B] = 0 2 mol L–1 |
1 | 3506-3509 | Calculate the initial
rate of the reaction when [A] = 0 1 mol L–1, [B] = 0 2 mol L–1 Calculate
the rate of reaction after [A] is reduced to 0 |
1 | 3507-3510 | 1 mol L–1, [B] = 0 2 mol L–1 Calculate
the rate of reaction after [A] is reduced to 0 06 mol L–1 |
1 | 3508-3511 | 2 mol L–1 Calculate
the rate of reaction after [A] is reduced to 0 06 mol L–1 3 |
1 | 3509-3512 | Calculate
the rate of reaction after [A] is reduced to 0 06 mol L–1 3 3
The decomposition of NH3 on platinum surface is zero order reaction |
1 | 3510-3513 | 06 mol L–1 3 3
The decomposition of NH3 on platinum surface is zero order reaction What
are the rates of production of N2 and H2 if k = 2 |
1 | 3511-3514 | 3 3
The decomposition of NH3 on platinum surface is zero order reaction What
are the rates of production of N2 and H2 if k = 2 5 × 10–4 mol–1 L s–1 |
1 | 3512-3515 | 3
The decomposition of NH3 on platinum surface is zero order reaction What
are the rates of production of N2 and H2 if k = 2 5 × 10–4 mol–1 L s–1 3 |
1 | 3513-3516 | What
are the rates of production of N2 and H2 if k = 2 5 × 10–4 mol–1 L s–1 3 4
The decomposition of dimethyl ether leads to the formation of CH4, H2
and CO and the reaction rate is given by
Rate = k [CH3OCH3]3/2
The rate of reaction is followed by increase in pressure in a closed
vessel, so the rate can also be expressed in terms of the partial pressure
of dimethyl ether, i |
1 | 3514-3517 | 5 × 10–4 mol–1 L s–1 3 4
The decomposition of dimethyl ether leads to the formation of CH4, H2
and CO and the reaction rate is given by
Rate = k [CH3OCH3]3/2
The rate of reaction is followed by increase in pressure in a closed
vessel, so the rate can also be expressed in terms of the partial pressure
of dimethyl ether, i e |
1 | 3515-3518 | 3 4
The decomposition of dimethyl ether leads to the formation of CH4, H2
and CO and the reaction rate is given by
Rate = k [CH3OCH3]3/2
The rate of reaction is followed by increase in pressure in a closed
vessel, so the rate can also be expressed in terms of the partial pressure
of dimethyl ether, i e ,
(
)
3
3
3/2
CH OCH
Rate
kp
=
If the pressure is measured in bar and time in minutes, then what are
the units of rate and rate constants |
1 | 3516-3519 | 4
The decomposition of dimethyl ether leads to the formation of CH4, H2
and CO and the reaction rate is given by
Rate = k [CH3OCH3]3/2
The rate of reaction is followed by increase in pressure in a closed
vessel, so the rate can also be expressed in terms of the partial pressure
of dimethyl ether, i e ,
(
)
3
3
3/2
CH OCH
Rate
kp
=
If the pressure is measured in bar and time in minutes, then what are
the units of rate and rate constants 3 |
1 | 3517-3520 | e ,
(
)
3
3
3/2
CH OCH
Rate
kp
=
If the pressure is measured in bar and time in minutes, then what are
the units of rate and rate constants 3 5
Mention the factors that affect the rate of a chemical reaction |
1 | 3518-3521 | ,
(
)
3
3
3/2
CH OCH
Rate
kp
=
If the pressure is measured in bar and time in minutes, then what are
the units of rate and rate constants 3 5
Mention the factors that affect the rate of a chemical reaction 3 |
1 | 3519-3522 | 3 5
Mention the factors that affect the rate of a chemical reaction 3 6
A reaction is second order with respect to a reactant |
1 | 3520-3523 | 5
Mention the factors that affect the rate of a chemical reaction 3 6
A reaction is second order with respect to a reactant How is the rate
of reaction affected if the concentration of the reactant is
(i) doubled
(ii) reduced to half |
1 | 3521-3524 | 3 6
A reaction is second order with respect to a reactant How is the rate
of reaction affected if the concentration of the reactant is
(i) doubled
(ii) reduced to half 3 |
1 | 3522-3525 | 6
A reaction is second order with respect to a reactant How is the rate
of reaction affected if the concentration of the reactant is
(i) doubled
(ii) reduced to half 3 7
What is the effect of temperature on the rate constant of a reaction |
1 | 3523-3526 | How is the rate
of reaction affected if the concentration of the reactant is
(i) doubled
(ii) reduced to half 3 7
What is the effect of temperature on the rate constant of a reaction How can this effect of temperature on rate constant be represented
quantitatively |
1 | 3524-3527 | 3 7
What is the effect of temperature on the rate constant of a reaction How can this effect of temperature on rate constant be represented
quantitatively 3 |
1 | 3525-3528 | 7
What is the effect of temperature on the rate constant of a reaction How can this effect of temperature on rate constant be represented
quantitatively 3 8
In a pseudo first order reaction in water, the following results were
obtained:
t/s
0
30
60
90
[A]/ mol L–1
0 |
1 | 3526-3529 | How can this effect of temperature on rate constant be represented
quantitatively 3 8
In a pseudo first order reaction in water, the following results were
obtained:
t/s
0
30
60
90
[A]/ mol L–1
0 55
0 |
1 | 3527-3530 | 3 8
In a pseudo first order reaction in water, the following results were
obtained:
t/s
0
30
60
90
[A]/ mol L–1
0 55
0 31
0 |
1 | 3528-3531 | 8
In a pseudo first order reaction in water, the following results were
obtained:
t/s
0
30
60
90
[A]/ mol L–1
0 55
0 31
0 17
0 |
1 | 3529-3532 | 55
0 31
0 17
0 085
Calculate the average rate of reaction between the time interval 30
to 60 seconds |
1 | 3530-3533 | 31
0 17
0 085
Calculate the average rate of reaction between the time interval 30
to 60 seconds 3 |
1 | 3531-3534 | 17
0 085
Calculate the average rate of reaction between the time interval 30
to 60 seconds 3 9
A reaction is first order in A and second order in B |
1 | 3532-3535 | 085
Calculate the average rate of reaction between the time interval 30
to 60 seconds 3 9
A reaction is first order in A and second order in B (i) Write the differential rate equation |
1 | 3533-3536 | 3 9
A reaction is first order in A and second order in B (i) Write the differential rate equation (ii) How is the rate affected on increasing the concentration of B three
times |
1 | 3534-3537 | 9
A reaction is first order in A and second order in B (i) Write the differential rate equation (ii) How is the rate affected on increasing the concentration of B three
times (iii) How is the rate affected when the concentrations of both A and B
are doubled |
1 | 3535-3538 | (i) Write the differential rate equation (ii) How is the rate affected on increasing the concentration of B three
times (iii) How is the rate affected when the concentrations of both A and B
are doubled Exercises
Exercises
Exercises
Exercises
Exercises
Rationalised 2023-24
86
Chemistry
3 |
1 | 3536-3539 | (ii) How is the rate affected on increasing the concentration of B three
times (iii) How is the rate affected when the concentrations of both A and B
are doubled Exercises
Exercises
Exercises
Exercises
Exercises
Rationalised 2023-24
86
Chemistry
3 10
In a reaction between A and B, the initial rate of reaction (r0) was measured
for different initial concentrations of A and B as given below:
A/ mol L–1
0 |
1 | 3537-3540 | (iii) How is the rate affected when the concentrations of both A and B
are doubled Exercises
Exercises
Exercises
Exercises
Exercises
Rationalised 2023-24
86
Chemistry
3 10
In a reaction between A and B, the initial rate of reaction (r0) was measured
for different initial concentrations of A and B as given below:
A/ mol L–1
0 20
0 |
1 | 3538-3541 | Exercises
Exercises
Exercises
Exercises
Exercises
Rationalised 2023-24
86
Chemistry
3 10
In a reaction between A and B, the initial rate of reaction (r0) was measured
for different initial concentrations of A and B as given below:
A/ mol L–1
0 20
0 20
0 |
1 | 3539-3542 | 10
In a reaction between A and B, the initial rate of reaction (r0) was measured
for different initial concentrations of A and B as given below:
A/ mol L–1
0 20
0 20
0 40
B/ mol L–1
0 |
1 | 3540-3543 | 20
0 20
0 40
B/ mol L–1
0 30
0 |
1 | 3541-3544 | 20
0 40
B/ mol L–1
0 30
0 10
0 |
1 | 3542-3545 | 40
B/ mol L–1
0 30
0 10
0 05
r0/mol L–1s–1
5 |
1 | 3543-3546 | 30
0 10
0 05
r0/mol L–1s–1
5 07 × 10–5
5 |
1 | 3544-3547 | 10
0 05
r0/mol L–1s–1
5 07 × 10–5
5 07 × 10–5
1 |
1 | 3545-3548 | 05
r0/mol L–1s–1
5 07 × 10–5
5 07 × 10–5
1 43 × 10–4
What is the order of the reaction with respect to A and B |
1 | 3546-3549 | 07 × 10–5
5 07 × 10–5
1 43 × 10–4
What is the order of the reaction with respect to A and B 3 |
1 | 3547-3550 | 07 × 10–5
1 43 × 10–4
What is the order of the reaction with respect to A and B 3 11
The following results have been obtained during the kinetic studies of the reaction:
2A + B ® C + D
Experiment
[A]/mol L–1
[B]/mol L–1
Initial rate of formation
of D/mol L–1 min–1
I
0 |
1 | 3548-3551 | 43 × 10–4
What is the order of the reaction with respect to A and B 3 11
The following results have been obtained during the kinetic studies of the reaction:
2A + B ® C + D
Experiment
[A]/mol L–1
[B]/mol L–1
Initial rate of formation
of D/mol L–1 min–1
I
0 1
0 |
1 | 3549-3552 | 3 11
The following results have been obtained during the kinetic studies of the reaction:
2A + B ® C + D
Experiment
[A]/mol L–1
[B]/mol L–1
Initial rate of formation
of D/mol L–1 min–1
I
0 1
0 1
6 |
1 | 3550-3553 | 11
The following results have been obtained during the kinetic studies of the reaction:
2A + B ® C + D
Experiment
[A]/mol L–1
[B]/mol L–1
Initial rate of formation
of D/mol L–1 min–1
I
0 1
0 1
6 0 × 10–3
II
0 |
1 | 3551-3554 | 1
0 1
6 0 × 10–3
II
0 3
0 |
1 | 3552-3555 | 1
6 0 × 10–3
II
0 3
0 2
7 |
1 | 3553-3556 | 0 × 10–3
II
0 3
0 2
7 2 × 10–2
III
0 |
1 | 3554-3557 | 3
0 2
7 2 × 10–2
III
0 3
0 |
1 | 3555-3558 | 2
7 2 × 10–2
III
0 3
0 4
2 |
1 | 3556-3559 | 2 × 10–2
III
0 3
0 4
2 88 × 10–1
IV
0 |
1 | 3557-3560 | 3
0 4
2 88 × 10–1
IV
0 4
0 |
1 | 3558-3561 | 4
2 88 × 10–1
IV
0 4
0 1
2 |
1 | 3559-3562 | 88 × 10–1
IV
0 4
0 1
2 40 × 10–2
Determine the rate law and the rate constant for the reaction |
1 | 3560-3563 | 4
0 1
2 40 × 10–2
Determine the rate law and the rate constant for the reaction 3 |
1 | 3561-3564 | 1
2 40 × 10–2
Determine the rate law and the rate constant for the reaction 3 12
The reaction between A and B is first order with respect to A and zero order
with respect to B |
1 | 3562-3565 | 40 × 10–2
Determine the rate law and the rate constant for the reaction 3 12
The reaction between A and B is first order with respect to A and zero order
with respect to B Fill in the blanks in the following table:
Experiment
[A]/ mol L–1
[B]/ mol L–1
Initial rate/
mol L–1 min–1
I
0 |
1 | 3563-3566 | 3 12
The reaction between A and B is first order with respect to A and zero order
with respect to B Fill in the blanks in the following table:
Experiment
[A]/ mol L–1
[B]/ mol L–1
Initial rate/
mol L–1 min–1
I
0 1
0 |
1 | 3564-3567 | 12
The reaction between A and B is first order with respect to A and zero order
with respect to B Fill in the blanks in the following table:
Experiment
[A]/ mol L–1
[B]/ mol L–1
Initial rate/
mol L–1 min–1
I
0 1
0 1
2 |
1 | 3565-3568 | Fill in the blanks in the following table:
Experiment
[A]/ mol L–1
[B]/ mol L–1
Initial rate/
mol L–1 min–1
I
0 1
0 1
2 0 × 10–2
II
–
0 |
1 | 3566-3569 | 1
0 1
2 0 × 10–2
II
–
0 2
4 |
1 | 3567-3570 | 1
2 0 × 10–2
II
–
0 2
4 0 × 10–2
III
0 |
1 | 3568-3571 | 0 × 10–2
II
–
0 2
4 0 × 10–2
III
0 4
0 |
1 | 3569-3572 | 2
4 0 × 10–2
III
0 4
0 4
–
IV
–
0 |
1 | 3570-3573 | 0 × 10–2
III
0 4
0 4
–
IV
–
0 2
2 |
1 | 3571-3574 | 4
0 4
–
IV
–
0 2
2 0 × 10–2
3 |
1 | 3572-3575 | 4
–
IV
–
0 2
2 0 × 10–2
3 13
Calculate the half-life of a first order reaction from their rate constants given
below:
(i) 200 s–1
(ii) 2 min–1
(iii) 4 years–1
3 |
1 | 3573-3576 | 2
2 0 × 10–2
3 13
Calculate the half-life of a first order reaction from their rate constants given
below:
(i) 200 s–1
(ii) 2 min–1
(iii) 4 years–1
3 14
The half-life for radioactive decay of 14C is 5730 years |
1 | 3574-3577 | 0 × 10–2
3 13
Calculate the half-life of a first order reaction from their rate constants given
below:
(i) 200 s–1
(ii) 2 min–1
(iii) 4 years–1
3 14
The half-life for radioactive decay of 14C is 5730 years An archaeological
artifact containing wood had only 80% of the 14C found in a living tree |
1 | 3575-3578 | 13
Calculate the half-life of a first order reaction from their rate constants given
below:
(i) 200 s–1
(ii) 2 min–1
(iii) 4 years–1
3 14
The half-life for radioactive decay of 14C is 5730 years An archaeological
artifact containing wood had only 80% of the 14C found in a living tree Estimate
the age of the sample |
1 | 3576-3579 | 14
The half-life for radioactive decay of 14C is 5730 years An archaeological
artifact containing wood had only 80% of the 14C found in a living tree Estimate
the age of the sample 3 |
1 | 3577-3580 | An archaeological
artifact containing wood had only 80% of the 14C found in a living tree Estimate
the age of the sample 3 15
The experimental data for decomposition of N2O5
[2N2O5 ® 4NO2 + O2]
in gas phase at 318K are given below:
t/s
0
400
800
1200 1600 2000 2400 2800 3200
102 × [N2O5]/ 1 |
1 | 3578-3581 | Estimate
the age of the sample 3 15
The experimental data for decomposition of N2O5
[2N2O5 ® 4NO2 + O2]
in gas phase at 318K are given below:
t/s
0
400
800
1200 1600 2000 2400 2800 3200
102 × [N2O5]/ 1 63
1 |
1 | 3579-3582 | 3 15
The experimental data for decomposition of N2O5
[2N2O5 ® 4NO2 + O2]
in gas phase at 318K are given below:
t/s
0
400
800
1200 1600 2000 2400 2800 3200
102 × [N2O5]/ 1 63
1 36
1 |
1 | 3580-3583 | 15
The experimental data for decomposition of N2O5
[2N2O5 ® 4NO2 + O2]
in gas phase at 318K are given below:
t/s
0
400
800
1200 1600 2000 2400 2800 3200
102 × [N2O5]/ 1 63
1 36
1 14
0 |
1 | 3581-3584 | 63
1 36
1 14
0 93
0 |
1 | 3582-3585 | 36
1 14
0 93
0 78
0 |
1 | 3583-3586 | 14
0 93
0 78
0 64
0 |
1 | 3584-3587 | 93
0 78
0 64
0 53
0 |
1 | 3585-3588 | 78
0 64
0 53
0 43
0 |
1 | 3586-3589 | 64
0 53
0 43
0 35
mol L–1
(i) Plot [N2O5] against t |
1 | 3587-3590 | 53
0 43
0 35
mol L–1
(i) Plot [N2O5] against t (ii) Find the half-life period for the reaction |
1 | 3588-3591 | 43
0 35
mol L–1
(i) Plot [N2O5] against t (ii) Find the half-life period for the reaction (iii) Draw a graph between log[N2O5] and t |
1 | 3589-3592 | 35
mol L–1
(i) Plot [N2O5] against t (ii) Find the half-life period for the reaction (iii) Draw a graph between log[N2O5] and t (iv) What is the rate law |
1 | 3590-3593 | (ii) Find the half-life period for the reaction (iii) Draw a graph between log[N2O5] and t (iv) What is the rate law Rationalised 2023-24
87
Chemical Kinetics
(v) Calculate the rate constant |
1 | 3591-3594 | (iii) Draw a graph between log[N2O5] and t (iv) What is the rate law Rationalised 2023-24
87
Chemical Kinetics
(v) Calculate the rate constant (vi) Calculate the half-life period from k and compare it with (ii) |
1 | 3592-3595 | (iv) What is the rate law Rationalised 2023-24
87
Chemical Kinetics
(v) Calculate the rate constant (vi) Calculate the half-life period from k and compare it with (ii) 3 |
1 | 3593-3596 | Rationalised 2023-24
87
Chemical Kinetics
(v) Calculate the rate constant (vi) Calculate the half-life period from k and compare it with (ii) 3 16
The rate constant for a first order reaction is 60 s–1 |
1 | 3594-3597 | (vi) Calculate the half-life period from k and compare it with (ii) 3 16
The rate constant for a first order reaction is 60 s–1 How much time will
it take to reduce the initial concentration of the reactant to its 1/16th
value |
1 | 3595-3598 | 3 16
The rate constant for a first order reaction is 60 s–1 How much time will
it take to reduce the initial concentration of the reactant to its 1/16th
value 3 |
1 | 3596-3599 | 16
The rate constant for a first order reaction is 60 s–1 How much time will
it take to reduce the initial concentration of the reactant to its 1/16th
value 3 17
During nuclear explosion, one of the products is 90Sr with half-life of
28 |
1 | 3597-3600 | How much time will
it take to reduce the initial concentration of the reactant to its 1/16th
value 3 17
During nuclear explosion, one of the products is 90Sr with half-life of
28 1 years |
1 | 3598-3601 | 3 17
During nuclear explosion, one of the products is 90Sr with half-life of
28 1 years If 1mg of 90Sr was absorbed in the bones of a newly born
baby instead of calcium, how much of it will remain after 10 years and
60 years if it is not lost metabolically |
1 | 3599-3602 | 17
During nuclear explosion, one of the products is 90Sr with half-life of
28 1 years If 1mg of 90Sr was absorbed in the bones of a newly born
baby instead of calcium, how much of it will remain after 10 years and
60 years if it is not lost metabolically 3 |
1 | 3600-3603 | 1 years If 1mg of 90Sr was absorbed in the bones of a newly born
baby instead of calcium, how much of it will remain after 10 years and
60 years if it is not lost metabolically 3 18
For a first order reaction, show that time required for 99% completion
is twice the time required for the completion of 90% of reaction |
1 | 3601-3604 | If 1mg of 90Sr was absorbed in the bones of a newly born
baby instead of calcium, how much of it will remain after 10 years and
60 years if it is not lost metabolically 3 18
For a first order reaction, show that time required for 99% completion
is twice the time required for the completion of 90% of reaction 3 |
1 | 3602-3605 | 3 18
For a first order reaction, show that time required for 99% completion
is twice the time required for the completion of 90% of reaction 3 19
A first order reaction takes 40 min for 30% decomposition |
1 | 3603-3606 | 18
For a first order reaction, show that time required for 99% completion
is twice the time required for the completion of 90% of reaction 3 19
A first order reaction takes 40 min for 30% decomposition Calculate t1/2 |
1 | 3604-3607 | 3 19
A first order reaction takes 40 min for 30% decomposition Calculate t1/2 3 |
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