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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 10^{3} mol^{-1} L s^{-1} and E_{a} = 2.0 x 10^{2} 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 NH_{4}OH is 4 .0 x 10^{10} M^{-1} s^{-1}. Thus, rate constant for proton transfer to NH_{3} 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 O_{3} at 298 K. It reacts with oxygen atoms as

O + O_{3} → 2O_{2}, k = 1.5 x 10^{7} 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 O_{3} at 298 K. It reacts with oxygen atoms as

O + O_{3} → 2O_{2}, k = 1.5 x 10^{7} L mol^{-1} s^{-1} at the rate of 0.15 mol L^{-1} s^{-1}.

**Q. **

**What is the rate of formation oxygen (O _{2}) under these conditions?**

Solution:

QUESTION: 20

Passage II

The complex ion of Fe^{2+} 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 Fe^{2+} 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, t_{1} = t_{2} 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, t_{1} = t_{2} 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 CH_{4} 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 CH_{4} 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 CCI_{4}(l)at 45°.

An 80.0 g sample of N_{2}O_{5}(g)is dissolved inCCI_{4}(l) and allowed to decompose at 450°C.

**Q. **

**Time taken for the quantity of N _{2}O_{5} to be reduced to 2.5 g is**

Solution:

In CCI_{4}(l), N_{2}O_{5} and N_{2}O_{4} are soluble. Hence, volume of O_{2} is only formed.

QUESTION: 27

Passage V

The following first order reaction is conducted in CCI_{4}(l)at 45°.

An 80.0 g sample of N_{2}O_{5}(g)is dissolved inCCI_{4}(l) and allowed to decompose at 450°C.

**Q. **

**Volume of O _{2} produced at STP at this point is**

Solution:

InCCI_{4}(l), N_{2}O_{5} and N_{2}O_{4} are soluble. Hence, volume of O_{2} 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. O_{2} 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 10^{3} Lmol^{-1} s^{-1}. Unit of k indicates that rates of formation of HCO_{3} 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 10^{10} 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 t_{1} seconds to decrease concentration from 4 x 10^{-4} mol dm^{-3} to 2 x 10^{-4} mol dm^{-3} and t_{2} 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 t_{1} to t_{2}?

Solution:

t_{1} = time to decrease concentration from 4 x 10^{-4} mol dm^{-3} to 2 x 10^{-4} mol dm^{-3}.

t_{2} = 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

T_{50} (Radium-226) =1620 years, One year = 3.154x 10^{7} s

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

Solution:

One curie = 3.7 x 10^{10} 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 t_{1/8} and t_{1/10} respectively. What is the value of

**[IITJEE 2012]**

Solution:

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