The burning of coal represented by the equation; ${\rm{C}}\left( s \right) + {{\rm{O}}_2}\left( {\rm{g}} \right) \to {\rm{C}}{{\rm{O}}_2}\left( {\rm{g}} \right){\rm{.}}$ The rate of this reaction is increased by:

Decrease in the concentration of oxygen

Providing inert atmosphere for burning

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JEE • CHEMISTRY • CHEMICAL KINETICS

Chemical kinetics practice · Easy

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Practice format and chapter quiz

These sets use single-correct-answer MCQs. They do not cover every JEE Main or JEE Advanced question format and are not full-length mock papers.

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Showing 1-30 of 103 questions

1 Easy

1 of 103

Remembering +4 | -1

For the first order reaction with the rate constant

k

, which expression gives the rate half-life period?

(Initial\mathrm{ }conc.\mathrm{ } = a)

View answer and explanation

Correct option: D

\frac{{0.693}}{k}

Option D (

\frac{{0.693}}{k}

) is correct because the half-life of a first-order reaction is given by the formula

t_{1/2} = \frac{{0.693}}{k}

2 Easy

2 of 103

Analyzing +4 | -1

For a certain reaction involving a single reactant, it is found that

C_0 \sqrt{T}

is constant, where

C_0

is the initial concentration of the reactant and

T

is the half-life. What is the order of the reaction?

View answer and explanation

Correct option: D

Option D (3) is correct because the rate law can be determined from the given relationship between initial concentration and half-life, leading to a third-order reaction.

3 Easy

3 of 103

Remembering +4 | -1

Arrhenius equation is

View answer and explanation

Correct option: C

k = A{e^{ - {E_a}/RT}}

Option C (

k = A{e^{ - {E_a}/RT}}

) is the correct Arrhenius equation, which relates the rate constant of a reaction to temperature and activation energy.

4 Easy

4 of 103

Remembering +4 | -1

The rate at which a substance reacts depends on its

View answer and explanation

Correct option: D

Active mass

Option D (Active mass) is correct because the rate of a reaction is directly proportional to the active masses (effective concentrations) of the reactants.

5 Easy

5 of 103

Remembering +4 | -1

The temperature coefficient of a reaction is:

View answer and explanation

Correct option: C

The ratio of rate constant differing by

10^\circ C

, preferably

35^\circ C\;and\;25^\circ C

Option C is correct because the temperature coefficient is defined as the ratio of rate constants at two temperatures differing by 10°C, often measured at 35°C and 25°C.

6 Easy

6 of 103

Application +4 | -1

For the reaction,

2A + B \to products

, the active mass of B is kept constant, and that of A is doubled. The rate of reaction will be then

View answer and explanation

Correct option: C

Increase 4 times

Option C (Increase 4 times) is correct because the rate of the reaction is proportional to the square of the concentration of reactant A.

7 Easy

7 of 103

Understanding +4 | -1

Which one of the following reactions is a true first order reaction?

View answer and explanation

Correct option: C

Decomposition of

{N}_2 {O}

Option A (Alkaline hydrolysis of ethyl acetate) is incorrect. Option B (Acid catalyst hydrolysis of ethyl acetate) is incorrect. Option C (Decomposition of

{N}_2 {O}

) is correct because it follows first-order kinetics. Option D (Decomposition of gaseous ammonia on a hot platinum surface) is incorrect.

8 Easy

8 of 103

Understanding +4 | -1

According to collision theory of reaction rates:

View answer and explanation

Correct option: D

Rate of reaction is directly proportional to collision frequency

Option D is correct because, according to collision theory, the rate of a reaction is directly proportional to the frequency of collisions between reactant molecules.

9 Easy

9 of 103

Remembering +4 | -1

Effect of temperature on reaction rate is given by

View answer and explanation

Correct option: B

Arrhenius equation

Option B (Arrhenius equation) is correct because the Arrhenius equation describes the relationship between temperature and reaction rate.

10 Easy

10 of 103

Analyzing +4 | -1

The rate constant

(K)

for the reaction

2A + B \to product

  was found to be

2.5 \times {10^{ - 5}}\;\mathrm{litre}\;\mathrm{mo}{\mathrm{l}^{ - 1}}\;{\sec ^{ - 1}}\;\;after\;\;15\sec ,\;2.60 \times {10^{ - 5}}\;\mathrm{litre}\;\mathrm{mo}{\mathrm{l}^{ - 1}}\;{\sec ^{ - 1}}\;\mathrm{after}\;\;30\sec

and

2.55 \times {10^{ - 5}}\;\mathrm{litre}\;\mathrm{mo}{\mathrm{l}^{ - 1}}\;{\sec ^{ - 1}}\;\mathrm{after}\;\;50\;\mathrm{sec}\mathrm{.}

The order of reaction is:

View answer and explanation

Correct option: A

Option A (2) is correct because the rate constant K remains approximately constant over time, and the units of K (litre mol^-1 sec^-1) indicate a second-order reaction.

11 Easy

11 of 103

Understanding +4 | -1

For a first order reaction, the half-life period is independent of

View answer and explanation

Correct option: C

Initial concentration

Option C (Initial concentration) is correct because the half-life of a first-order reaction is independent of the initial concentration of the reactant.

12 Easy

12 of 103

Application +4 | -1

For a reaction

aA \to bB

when

\left[ A \right] = 2.2\;\mathrm{m}\;\mathrm{M},

the rate was found to be

2.4\;\mathrm{m}\;\mathrm{M}{\mathrm{s}^{ - 1}}.

On reducing concentration of

\left[ A \right]

to half, the rate changes to

0.6\;\mathrm{m}\;\mathrm{M}{\mathrm{s}^{ - 1}}.

The order of reaction with respect to

A

is:

View answer and explanation

Correct option: B

Option B (2) is correct because the rate equation is of the form

r = k[A]^n

, and solving for n using the given data yields n = 2.

13 Easy

13 of 103

Application +4 | -1

If the rate constant for a first order reaction is k, the time (t) required for the completion of 99% of the reaction is given by:

View answer and explanation

Correct option: A

\mathrm{t = 4}\mathrm{.606/k}

Option A (

\mathrm{t = 4}\mathrm{.606/k}

) is correct because it is derived from the integrated rate law for a first-order reaction when 99% of the reaction is completed.

14 Easy

14 of 103

Understanding +4 | -1

The burning of coal represented by the equation;

\mathrm{C}\left( s \right) + {\mathrm{O}_2}\left( \mathrm{g} \right) \to \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right)\mathrm{.}

The rate of this reaction is increased by:

View answer and explanation

Correct option: B

Powdering the lumps of coal

Option B (Powdering the lumps of coal) is correct because increasing the surface area of the coal by powdering it allows for more contact with oxygen, thus increasing the reaction rate.

15 Easy

15 of 103

Application +4 | -1

A reaction was found to 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

View answer and explanation

Correct option: C

Increases by factor of four

The correct answer is C (6 (app.)) because the maximum concentration of zwitterion occurs at the isoelectric point, which is the average of the pKa values of the amino and carboxyl groups.

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16 Easy

16 of 103

Understanding +4 | -1

The decomposition of

{N_2}{O_5}

occur as

2{N_2}{O_5}\, \to \,\,4N{O_2} + {O_2},

and follows Ist order kinetics, hance

View answer and explanation

Correct option: C

{t_{1/2}} \propto {a^0}

Option C (

{t_{1/2}} \propto {a^0}

) is correct because for a first-order reaction, the half-life is independent of the initial concentration, meaning it's proportional to

a^0

17 Easy

17 of 103

Understanding +4 | -1

For fourth order reaction, what is the unit of

K

View answer and explanation

Correct option: A

{\left( {\frac{{mol}}{L}} \right)^{ - 3}}\;{s^{ - 1}}

The correct answer is C (

{MgF}_2

) because it is an ionic compound where both Mg and F achieve octet configuration through electron transfer, thus not an exception to the octet rule.

18 Easy

18 of 103

Understanding +4 | -1

Consider the reaction

{N_2}(g) + 3{H_2}(g) \to 2N{H_3}(g)

. The equality relationship between

\frac{{d\left[ {N{H_3}} \right]}}{{dt}}\alpha - \frac{{d\left[ {{H_2}} \right]}}{{dt}}

View answer and explanation

Correct option: A

+ \frac{{d\left[ {N{H_3}} \right]}}{{dt}} = \frac{{ - 2}}{3}\frac{{d\left[ {{H_2}} \right]}}{{dt}}

Option A is correct because the rate of formation of

NH_3

is related to the rate of consumption of

H_2

by the stoichiometric coefficients in the balanced chemical equation.

19 Easy

19 of 103

Understanding +4 | -1

\frac{1}{{{{\left[ A \right]}^2}}}

vs times are a straight line. Order of reaction is

View answer and explanation

Correct option: D

Third

Option D (Third) is correct because if the graph of

\frac{1}{{{\left[ A \right]}^2}}

versus time yields a straight line, it indicates a third-order reaction.

20 Easy

20 of 103

Application +4 | -1

For a chemical reaction

X \to P

, the rate of reaction doubles when the concentration of X is increased 4 times. The order of reaction with respect to X is

View answer and explanation

Correct option: A

\frac{1}{2}

Option A (1/2) is correct because the rate of reaction is proportional to the square root of the concentration of X, indicating a half-order reaction.

21 Easy

21 of 103

Understanding +4 | -1

Which of the following statements is in accordance with the Arrhenius equation?

View answer and explanation

Correct option: B

Rate of a reaction increases with decrease in activation energy

Option B (Rate of a reaction increases with decrease in activation energy) is correct because the Arrhenius equation shows an inverse exponential relationship between the rate constant and activation energy.

22 Easy

22 of 103

Application +4 | -1

The rate of a chemical reaction doubles for every

10\,^\circ C

rise of temperature. If the temperature is raised by

50\,^\circ C

, the rate of the reaction increases by about

View answer and explanation

Correct option: C

32 times

Option C (32 times) is correct because the rate increases by a factor of 2 for every 10°C increase, resulting in a 32-fold increase for a 50°C increase.

23 Easy

23 of 103

Application +4 | -1

Half life period of a reaction is found to be inversely proportional to the cube of the initial concentration. The order of reaction is

View answer and explanation

Correct option: A

Option A (4) is correct because the half-life is inversely proportional to the initial concentration raised to the power of (n-1), where n is the order of the reaction.

24 Easy

24 of 103

Application +4 | -1

A first order reaction is 10% complete in 20 min. The time taken for 19% completion is

View answer and explanation

Correct option: B

40 Min

Option B (40 Min) is correct because the time for a first-order reaction to complete a certain percentage depends on the rate constant, and 19% completion takes approximately twice the time of 10% completion given the logarithmic nature of first-order kinetics.

25 Easy

25 of 103

Application +4 | -1

In the reversible reaction,

2N{O_2}\,\underset{{{k_2}}}{\overset{{{k_1}}}{\leftrightharpoons}}\,{N_2}{O_4};

the rate of disappearance of

N{O_2}

is equal to

View answer and explanation

Correct option: C

2{k_1}\left[ {N{O_2}} \right]{\,^2} - 2{k_2}\left[ {{N_2}\,{O_4}} \right]

Option C (

2{k_1}\left[ {N{O_2}} \right]{\,^2} - 2{k_2}\left[ {{N_2}\,{O_4}} \right]

) is correct because it represents the rate of disappearance of

NO_2

considering both forward and reverse reactions.

26 Easy

26 of 103

Application +4 | -1

The order of a gaseous phase reaction for which rate becomes half if volume of container having same amount of reactant is doubled is:

View answer and explanation

Correct option: A

Option A (1) is correct because for a first-order reaction, the rate is directly proportional to the concentration, and doubling the volume halves the concentration, thus halving the rate.

27 Easy

27 of 103

Understanding +4 | -1

Assertion (A):Emission of light as a result of exposure of

P

to air in night is called phosphorescence.

Reason (R): Phosphorus burns in

\mathrm{O}_2

to give

\mathrm{P}_2 \mathrm{O}_5

and conversion of chemical energy into light energy producing cold light and the phenomenon is called chemi-luminescence.

View answer and explanation

Correct option: B

A is wrong but R is correct

Option B (A is wrong but R is correct) is correct because the emission of light by phosphorus in air is chemiluminescence, not phosphorescence, and the reason correctly describes chemiluminescence.

28 Easy

28 of 103

Analyzing +4 | -1

Which one of the following is wrongly matched?

View answer and explanation

Correct option: D

Combination of

{H_2}

and

{B_{r2}}\;

to give

HBr

-first order reaction

Option D (Combination of H₂ and Br₂ to give HBr - first order reaction) is wrongly matched because the reaction is actually a complex reaction with a non-integer order, not a first-order reaction.

29 Easy

29 of 103

Application +4 | -1

The

{t_{\frac{1}{2}}}

of a reaction is halved as the initial concentration of the reactant is doubled. What is order of reaction?

View answer and explanation

Correct option: C

Option C (2) is correct because the half-life of a second-order reaction is inversely proportional to the initial concentration of the reactant.

30 Easy

30 of 103

Understanding +4 | -1

For the elementary step,

{\left( {\mathrm{C}{\mathrm{H}_3}} \right)_3} \cdot \mathrm{CBr}\left( {aq} \right) \to {\left( {\mathrm{C}{\mathrm{H}_3}} \right)_3}{\mathrm{C}^ + }\left( {aq} \right) + \mathrm{B}{\mathrm{r}^ - }\left( {aq} \right)

the molecularity is:

View answer and explanation

Correct option: B

Option B (1) is correct because molecularity is the number of reactant molecules involved in an elementary step, which is one in this case.

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Key Takeaways

✓ This set contains 103 single-correct-answer MCQs on CHEMICAL KINETICS.
✓ Try each question before opening its answer. Read the explanation where one is available.
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