Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics)


37 Questions MCQ Test Chemistry for JEE Advanced | Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics)


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This mock test of Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics) for JEE helps you for every JEE entrance exam. This contains 37 Multiple Choice Questions for JEE Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics) (mcq) to study with solutions a complete question bank. The solved questions answers in this Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics) quiz give you a good mix of easy questions and tough questions. JEE students definitely take this Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics) exercise for a better result in the exam. You can find other Revisal Problems (Past 13 Years) JEE Advanced (Chemical Kinetics) extra questions, long questions & short questions for JEE on EduRev as well by searching above.
QUESTION: 1

Direction (Q. Nos. 1-12) This section contains 12 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct.

For the first order gaseous phase reaction, A → B + C

initial pressure is 200 mm and after 20 min, total pressure is 250 mm. Thus, half-life period is 

Solution:







QUESTION: 2

For the elementary reaction (M → N), the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M is

[JEE Advanced 2014]

Solution:


QUESTION: 3

For the reaction,

experimental data for the measured initial rates is given below.

Q.

The order of the reaction with respect of P,Q and R respectively is

Solution:







QUESTION: 4

Reaction coordinate diagram for the reaction

Solution:

 By Arrhenius equation




Given reaction is endothermic, ΔH = + 103.1kJ.
Thus, reaction-coordinate diagram is

QUESTION: 5

For a reaction, k = 1.2 x 103 mol-1 L s-1 and Ea = 2.0 x 102 kJ mol-1

When T→ ∞, Arrhenius pre-exponential factor is

Solution:

By Arrhenius equation,


QUESTION: 6

Half-life period of the first order reaction is 100 days. After 144.3 days, concentration of the reactant is reduced to ......of the original value.

Solution:






Thus, concentration is reduced to   of the initial value.

QUESTION: 7

For the following chemical equation, a first order reaction, A(g) → nB(g) total pressure of the system as a function of time is 

Solution:







QUESTION: 8

What function of [X], plotted against time will give a straight line for a second order reaction?

Solution:

For a second order reaction





Thus, (i) represents a straight line.
Hence,  when plotted against time
will give a straight line.

QUESTION: 9

The rate constant at 298 K for the reaction of and OH+ to form NH4OH is 4 .0 x 1010 M-1 s-1. Thus, rate constant for proton transfer to NH3 is

Solution:








QUESTION: 10

For a reaction A → Product

[A]0 = Initial concentration, [A] = Concentration of the reactant A after time t.

Then

Solution:

This represents a second order reaction







QUESTION: 11

For a second order reaction,

where and a and b are the initial concentrations of A and B. Reaction w ould be pseudo-unimolecular when

Solution:




This represents unimolecular reaction.

QUESTION: 12

A certain reaction, A + B → Product

is first order w.r.t. each reactant with k = 5.0 x 10-3 M-1 s-1

then concentration of A remaining after 100 s is 

Solution:


Thus, concentration of B almost remains constant and reaction is first order w.r.t. A only.



*Multiple options can be correct
QUESTION: 13

Direction (Q. Nos. 13-16) This section contains 4 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONE or MORE THAN ONE are correct.

Q.

Rate constant k varies with tem perature as given by the equation

Select the correct statement(s) about this equation.

Solution:



(a) Unit of k is min-1, hence it is first order reaction thus (a) is correct.



Thus, (c) is correct.


Thus, (d) is correct.

*Multiple options can be correct
QUESTION: 14

Which is/are the graphical representation for the zeroth order reaction?

Solution:


Thus, rate remains constant.
Thus, (a) is correct.

In (c), rate increases with time.

Hence log(x) varies as log(t) increases. Thus, (d) is also correct.

*Multiple options can be correct
QUESTION: 15

Select the correct staiement(s) about half-life period,

Solution:

For zero order reaction














*Multiple options can be correct
QUESTION: 16

For the reaction,

In alkaline aqueous solution, the value of the second order (in BrC-), rate constant at 80°C in the rate law for   was found to be 0.056 L mol-1 s-1

Select the correct alternate reaction.

Solution:








Thus, (b) is correct.
BrO- has been oxidised to  and has been reduced to Br-.
Thus, it is a redox as well as disproportionation reaction.
Thus, (c) and (d) are correct.

QUESTION: 17

Direction (Q. No. 17) Choices for the correct combination of elements from Column I and Column II are given as options (a), (b), (c) and (d), out of which one is correct.

Q. Rate law of the nth order reaction is given by

Match the different properties in Column I with their related values of half-life in Column II and select the correct answer from the codes given.

Solution:
















QUESTION: 18

Direction (Q. Nos. 18-27) This section contains 5 paragraphs, each describing theory, experiments, data, etc. Ten questions related to the paragraphs have been given. Each question has only one correct answer among the four given options (a), (b), (c) and (d).

Passage I

A 22.4 L flask contains 0.76 mm of O3 at 298 K. It reacts with oxygen atoms as 
O + O3 → 2O2, k = 1.5 x 107 L mol-1 s-1 at the rate of 0.15 mol L-1 s-1.

Q. 

What is the concentration of oxygen atoms needed to maintain this rate?

Solution:




QUESTION: 19

Passage I

A 22.4 L flask contains 0.76 mm of O3 at 298 K. It reacts with oxygen atoms as 
O + O3 → 2O2, k = 1.5 x 107 L mol-1 s-1 at the rate of 0.15 mol L-1 s-1.

Q. 

What is the rate of formation oxygen (O2) under these conditions?

Solution:




QUESTION: 20

Passage II

The complex ion of Fe2+ with the chelating agent diphyridyl (abbreviated as dipy) has been studied kinetically in both the forward and the reverse directions.


Q. 

Half-life of the reverse reaction is

Solution:

For reverse reaction

It follows first order kinetics with rate constant.
 

Stability constant is obtained when rate of forward reaction
= rate of reverse reaction 

QUESTION: 21

Passage II

The complex ion of Fe2+ with the chelating agent diphyridyl (abbreviated as dipy) has been studied kinetically in both the forward and the reverse directions.


Q. 

Stability constant in terms of pk is

Solution:

For reverse reaction

It follows first order kinetics with rate constant 


Stability constant is obtained when rate of forward reaction
= rate of reverse reaction


QUESTION: 22

Passage III

Also, t1 = t2 and [A]0 = [B]0 = a

Q. 

The ratio of the rates of these two reactions at the start of the reaction is

Solution:










QUESTION: 23

Passage III

Also, t1 = t2 and [A]0 = [B]0 = a

Q. 

The ratio of the rates of these two reaction after a lapse of one half-life is

Solution:










QUESTION: 24

Passage IV

The rate constant for the decomposition of ethylene oxide into CH4 and CO may be described by

Q. 

Energy of activation for this reaction is 

Solution:






Unit of k indicates that reaction of first order. Rate constant at 670 K is

QUESTION: 25

Passage IV

The rate constant for the decomposition of ethylene oxide into CH4 and CO may be described by

Q. 

What is the rate constant at 670 K?

Solution:






Unit of k indicates that reaction of first order. Rate constant at 670 K is

QUESTION: 26

Passage V

The following first order reaction is conducted in CCI4(l)at 45°.

An 80.0 g sample of N2O5(g)is dissolved inCCI4(l) and allowed to decompose at 450°C.

Q. 

Time taken for the quantity of N2O5 to be reduced to 2.5 g is

Solution:

In CCI4(l), N2O5 and N2O4 are soluble. Hence, volume of O2 is only formed.









QUESTION: 27

Passage V

The following first order reaction is conducted in CCI4(l)at 45°.

An 80.0 g sample of N2O5(g)is dissolved inCCI4(l) and allowed to decompose at 450°C.

Q. 

Volume of O2 produced at STP at this point is

Solution:

InCCI4(l), N2O5 and N2O4 are soluble. Hence, volume of O2 is only formed.








*Answer can only contain numeric values
QUESTION: 28

Direction (Q. Nos. 28-37) This section contains 10 questions. When worked out will result in one integer from 0 to 9 (both inclusive).

The concentration of R in the reaction,

R→ P

was measured as a function of time and the following data is obtained :

Q. 

What is the order of reaction?

[IIT JEE 2010]


Solution:


Rate remains constant throughout thus, order = zero

*Answer can only contain numeric values
QUESTION: 29

For the reaction system,

volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order w.r.t. O2 and the second order w.r.t. NO, the rate of reaction will increase ......times of its initial value.


Solution:


Thus, rate increases 8 times of its initial value.

*Answer can only contain numeric values
QUESTION: 30

For the reaction, 

Initial pressure of A and B are respectively 0.60 atm and 0.80 atm. At a time when pressure of C is 0.20 atm, ratio of initial rate and final rate is y. What is the value of y?


Solution:





*Answer can only contain numeric values
QUESTION: 31

The rate constant for the reaction 

Number of moles of   ormed per second is x x 10-4 mol L-1.  What is the value of x? 


Solution:

Rate constant = k = 4 x 103 Lmol-1 s-1. Unit of k indicates that rates of formation of HCO3 is a second order reaction.


 

*Answer can only contain numeric values
QUESTION: 32

A flask contains a mixture of compounds A and B initially [A]0 = [S]0


After 54 minutes, [A] = x [B] What is the value of x? 


Solution:






*Answer can only contain numeric values
QUESTION: 33

For the bimolecular reaction 

The rate constant is k = 1 .3 x 1010 L mol -1 s-1
Compare the initial value of d/dt [O] for [O] = [OH] = 1.0 x 10-4 mol L-1 to that [O] = 1.0 x 10-4 mol L-1 and [OH]= 2.0 x 10-4 mol L-1


Solution:



*Answer can only contain numeric values
QUESTION: 34

A chemical reaction is known to be zeroth order with k = 5 x 10-8 mol s-1. The reaction takes t1 seconds to decrease concentration from 4 x 10-4 mol dm-3 to 2 x 10-4 mol dm-3 and t2 seconds to decrease concentration from 2 x 10-4 mol dm-3 to 1 x 10-4 mol dm J What is the ratio of t1  to t2?


Solution:

t1 = time to decrease concentration from 4 x 10-4 mol dm-3 to 2 x 10-4 mol dm-3.

t2 = time to decrease concentration from 2 x 10-4 mol dm-3 to 1 x 10-4 mol dm-3 

In both case, reaction takes place 50%


*Answer can only contain numeric values
QUESTION: 35

T50 (Radium-226) =1620 years, One year = 3.154x 107 s

Calculate the weight of Ra-226 which has activity equal to 5 curie.


Solution:

One curie = 3.7 x 1010 dps (disintegration of atoms per second)





*Answer can only contain numeric values
QUESTION: 36

For the zero order reaction, sets I and II are given.

What is the value of x?


Solution:

By set I
4 units of reactant change to 2 units in 2 min Thus, half-life is 2 min.



*Answer can only contain numeric values
QUESTION: 37

An organic compound undergoes first order decomposition. The time taken for its decomposition to  and  of its initial concentration are t1/8 and t1/10 respectively. What is the value of

[IITJEE 2012]


Solution: