 # JEE Main Chemical Kinetics Previous Year Questions with Solutions

Chemical kinetics JEE Main Previous Year Questions with Solutions are given here. The word ‘kinetics’ deals with the rate of change of some quantity. Chemical kinetics helps us to understand the rates of reactions and how it is influenced by certain conditions. It further helps to gather and analyze the information about the mechanism of the reaction and define the characteristics of a chemical reaction. In any chemical reaction, as the reaction proceeds, the amount of reactants decreases, whereas the amount of products increases. So the rate of the overall reaction depends on the rate at which reactants are consumed or the rate at which the products are formed.

The important topics related to chemical kinetics are the rate of formation and disappearance, average and instantaneous rate, factors affecting reaction rate, etc. As far as the JEE exam is concerned, this is an important topic. This article gives an idea of what type of questions can be expected from this topic. BYJU’S provides solutions designed by our experts.

## JEE Main Previous Year Solved Questions on Chemical Kinetics

1. For the equilibrium, A(g) ⇌ B(g), ΔH is –40 kJ/mol. If the ratio of the activation energies of the forward (Ef) and reverse (Eb) reactions is 2/3 then:

(1) Ef = 60kJ / mol; Eb = 100 kJ/mol

(2) Ef = 30kJ / mol; Eb = 70 kJ/mol

(3) Ef = 80kJ / mol; Eb = 120 kJ/mol

(4) Ef = 70kJ / mol; Eb = 30 kJ/mol

Solution:

A(g) ⇌ B(g)

Given ΔH = -40KJ/mol

Ef / Eb = ⅔

∴ Ef = ⅔ Eb

ΔH = Eb – Ef

-40 = Eb – ⅔ Eb

-40 = ⅓ Eb

∴ Eb = -40 ×3 = -120 KJ/mol

Ef = Eb – ΔH

= -120- (-40)

= -120+40

= -80 KJ/mol

Hence option (3) is the answer.

2. At 5180 C, the rate of decomposition of a sample of gaseous acetaldehyde, initially at a pressure of 363 Torr, was 1.00 s-1 when 5% had reacted and 0.5 Torr s-1 when 33% had reacted. The order of the reaction is :

(1) 3

(2) 1

(3) 0

(4) 2

Solution:

r1 = 1 torr/sec

When 5% is reacted, 95% is unreacted.

r2 = 0.5 torr/sec

When 33% is reacted, (67% is unreacted)

m = order of reaction,

unreacted = a-x

r1/r2 = [(a-x1)/(a-x2)]m

1/0.5 = (0.95/0.67)m

2 = (1.414)m

⇒ 2 = √2m

⇒ m = 2

So order of the reaction is 2.

Hence option (4) is the answer.

3. For the reaction A + 2B → C, rate is given by R = [A] [B]2 then the order of the reaction is

(1) 3

(2) 6

(3) 5

(4) 7

Solution:

The order of the reaction is the sum of the power of the concentration terms in rate law expression. R = [A] [B]2

So, order of reaction = 1+2 = 3

Hence option (1) is the answer.

4. The rate of a chemical reaction doubles for every 100 C rise of temperature. If the temperature is raised by 500 C, the rate of the reaction increases by about:-

(1) 32 times

(2) 64 times

(3) 10 times

(4) 24 times

Solution:

Given the rate of chemical reaction doubles for every 100 C rise of temperature. If the temperature is raised by 500 C, the rate of reaction increases by 2n times. Here n = 5.

So 2n = 25 = 32.

Hence option (1) is the answer.

5. If 50% of a reaction occurs in 100 seconds and 75% of the reaction occurs in 200 seconds, the order of this reaction is

(1) 1

(2) 2

(3) zero

(4) 3

Solution:

t1/2 = 100 second (50% reaction)

After 200 seconds, 75% of reaction will be completed,

i.e., t75% = 200 seconds.

So, it follows first-order kinetics as the half-life is independent of concentration and follows the relation t3/4 = 2 × t1/2

Hence option (1) is the answer.

6. The half-life period of a first-order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be (log 2 = 0.301):

(1) 46.06 minutes

(2) 460.6 minutes

(3) 230.3 minutes

(4) 23.03 minutes

Solution:

Given half-life period t1/2 = 6.93 min.

Decay constant, λ = 0.693/ t1/2

= 0.693/ 6.93

= 0.1 /min

Let t be time required for completion of chemical reaction.

We have t = (2.303/ λ) log (a/a-x)

∴ t = (2.303/0.1) log ( 100/100-99)

∴ t = (2.303/0.1) log 100

∴ t = (2.303/0.1) × 2

t = 46.06 min

Hence option (1) is the answer.

7. The rate of a reaction doubles when its temperature changes from 300 K to 310 K. Activation energy of such a reaction will be (R = 8.314KJmol-1 and log 2=0.301)

(1) 53.6 KJmol-1

(2) 48.6 KJmol-1

(3) 58.5 KJmol-1

(4) 60.5 KJmol-1

Solution:

According to Arrhenius equation,

ln k2/k1 = -(Ea/2.303R)(1/T2 – 1/T1)

r2/r1 = k2/k1 = 2

Given T1 = 300K

T2 = 310 K

log(2) = -(Ea/2.303 × 8.314) [(1/310) – (1/300)]

0.301 = -Ea/19.147 [(300-310)/93000 ]

0.301 = -Ea/19.147 [-10/93000 ]

Ea = 0.301×19.147×9300

= 53598.19 J

= 53.6 kJ/mol

Hence option (1) is the answer.

8. The time for half-life period of a certain reaction A → Products is 1 hour when the initial concentration of the reactant ‘A’ is 2.0 mol L–1, How much time does it take for its concentration to come from 0.50 to 0.25 mol L–1 if it is a zero-order reaction?

(1) 1 h

(2) 4 h

(3) 0.5 h

(4) 0.25 h

Solution:

The half life period for a zero order reaction is given by t1/2 = [A0]/2k

A0 is the initial concentration of the reactant.

K0 = [A0]/2t1/2

= 2/2×1

= 1 mol L-1h-1

Rate constant for a zero order reaction is given by k = (1/t) [A0 – A]

t = (1/k) [A0 – A]

= 0.50-0.25/1

= 0.25 h

Hence option (4) is the answer.

9. Decomposition of X exhibits a rate constant of 0.05 mg/year. How many years are required for the decomposition of 5 mg of X into 2.5 mg?

(1) 25

(2) 50

(3) 20

(4) 40

Solution:

According to unit of rate constant it is a zero-order reaction.

t1/2 = a0 / 2k

= 5/2×0.05

= 50 years

Hence option (2) is the answer.

10. In a first-order reaction, the concentration of the reactant, decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is

(a) 30 minutes

(b) 15 minutes

(c) 7.5 minutes

(d) 60 minutes.

Solution:

Gine that the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes.

t1/2 = 15 minute.

So, the concentration of reactant will fall from 0.1 M to 0.025 M in two half lives.

i.e., 2t1/2 = 2 ×15 = 30 minutes.

Hence option (1) is the answer.

11. The rate law for the reaction below is given by the expression k[A] [B]

A + B → Product

If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be

(1) 3 k

(2) 9 k

(3) k/3

(4) k

Solution:

The rate constant varies with the temperature only. It is independent of the concentration of reactants. So the rate constant will be k.

Hence option (4) is the answer.

12. For the reaction, 2A + B → products, when the concentrations of A and B both were doubled the rate of the reaction increased from 0.3 mol L–1 s–1 to 2.4 mol L–1 s–1. When the concentration of A alone is doubled, the rate increased from 0.3 mol L–1 s–1 to 0.6 mol L–1 s–1. Which one of the following statements is correct?

(1) Order of the reaction with respect to B is 2.

(2) Order of the reaction with respect to B is 1.

(3) Order of the reaction with respect to A is 2.

(4) Total order of the reaction is 4.

Solution:

If concentration of [A] is doubled, then the rate will be doubled, so the order of A is 1.

Then again if the concentration of A and B both were doubled, the rate will increase 8 times. Rate = [2A] [2B]2 = 8[A] [B]2

So the order of B is two.

So, the overall order is 3.

Hence option (1) is the answer.

13. A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of carbon monoxide is doubled, with everything else kept the same, the rate of reaction will be

(1) remain unchanged

(2) tripled

(3) increased by a factor of 4

(4) doubled.

Solution:

Given r1 = dx/dt = k[CO]2

r2 = k[2CO]2 = 4k[CO]2

According to the rate law expression doubling the concentration of CO increases the rate by a factor of 4.

Hence option (3) is the answer.

14. The formation of gas at the surface of tungsten due to adsorption is the reaction of order

(1) 0

(2) 1

(3) 2

(4) insufficient data.

Solution:

Adsorption on the metal surface do not depend on the concentration of gas.

So it is a zero-order reaction.

Hence option (1) is the answer.

15. Higher-order (>3) reactions are rare due to:

(1) shifting of equilibrium towards reactants due to elastic collision

(2) loss of active species on collision

(3) low probability of simultaneous collision of all the reacting species

(4) increase in entropy and activation energy as more molecules are involved.

Solution:

Higher-order (>3) reactions are rare due to the low probability of simultaneous collision of all the reacting species.

Hence option (3) is the answer.