NEET PYQ Chemical Kinetics - Chapter-wise Questions with Solutions

About Chemical Kinetics PYQs

Chemical Kinetics has 819 previous year questions in the Quantrex Academy NEET UG Chemistry bank. The 220 questions in this list come from NEET (148), AIIMS (41), JIPMER (25) and 1 other source, spanning 2001 to 2026. Each question opens on its own page with the options, the correct answer and the worked solution where available.

NEET Chemical Kinetics PYQs with Solutions

About Chemical Kinetics PYQs

Questions by year (this list)

Chemical Kinetics questions with solutions

The combination of NO_2(g) and CO(g) occurs in two steps as follows: What is the rate law for the reaction? 2NO_2 arrow NO + NO_3(k_1) - slow NO_3 + CO arrow CO_2 + NO_2(k_2)

The slope of the graph [A]_t against time for zero order reaction is

For the reaction C_2H_5Br_ (l) arrow C_2H_ 4(g) + HBr , r = K(C_2H_5Br) What is order and molecularity of the reaction respectively ?

The decomposition of N_2O_ 5(g) occurs as: 2\ N_2O_ 5(g) arrow 4\ NO_ 2(g) + O_ 2(g) . If initial concentration of N_2O_ 5(g) is 1.63 × 10^ -2 \ mol L^ -1 and after 400 seconds it

Which of the following statements represents rate of reaction?

What is the order of reaction for the following? 2H_2O_2(l) arrow 2H_2O(l) + O_2(g)

2A k B is a zero-order reaction, where k=1.0 mol L ^ -1 min ^ -1 . If the initial concentration of A is 2 M, then the time taken to complete 75\% of the reaction will be

Match List I with List II : List I (Order of reaction) List II (Unit of rate constant) A. Zero order I. mol^ -1 \ L\ s^ -1 B. First order II. mol^ -2 \ L^ 2 \ s^ -1 C. Second

For an elementary chemical reaction, the Arrhenius plot is given below. If the energy of activation is 6.64 kJ mol ^ -1 and R =8.3 J K ^ -1 mol ^ -1 , the temperature at which the

Given below is an expression for the rate constant of a first order reaction occurring at a certain temperature, T (K). k = 14.34 - 1.25 × 10^ 4 T The energy of activation in kcal

For a certain reaction R arrow Product, the plot of concentration [R] vs time has a negative slope as shown. The order of reaction is :

If the half-life (t_ 1 / 2 ) for a first order reaction is 1 minutes, then the time required for 99.9 \% completion of the reaction is closest to:

If the rate constant of a reaction is 0.03 ~s^ -1 , how much time does it take for 7.2 ~mol ~L^ -1 concentration of the reactant to get reduced to 0.9 ~mol ~L^ -1 ? (Given

Following data is for a reaction between reactants A and B : The order of the reaction with respect to A and B , respectively, are

Which of the following plot represents the variation of k versus (1)/(T) in accordance with Arrhenius equation?

Activation energy of any chemical reaction can be calculated if one knows the value of

Rate constants of a reaction at 500 K and 700 K are 0.04 ~s^ -1 and 0.14 ~s^ -1 , respectively; then, activation energy of the reaction is : (Given: 3.5=0.5441, R=8.31 ~J ~K^ -1

The rate of a reaction quadruples when temperature changes from 27^ ∘ C to 57^ ∘ C . Calculate the energy o activation. Given R=8.314 ~J ~K^ -1 ~mol^ -1 , 4=0.6021

Which plot of k vs 1 ~T is consistent with Arrhenius equation?

The correct option for the rate law that corresponds to overall first order reaction is

For a reaction 3 ~A arrow 2 ~B The average rate of appearance of B is given by (Δ[B])/(Δ t) . The correct relation between the average rate of appearance of B with the average

Given below are two statements: one labelled as Assertion A and other is labelled as Reason R : Assertion A: A reaction can have zero activation energy Reason R: The minimum extra

For a certain reaction, the rate = k [ A ] ^ 2 [ B ] , when the initial concentration of A is tripled keeping concentration of B constant, the initial rate would

The half life of a first order reaction is 2000 years. If the concentration after 8000 years is 0.02 M , then the initial concentration was :

For a chemical reaction 4 ~A+3 ~B arrow 6 C+9 D rate of formation of C is 6 × 10^ -2 ~mol ~L^ -1 ~s^ -1 and rate of disappearance of A is 4 × 10^ -2 ~mol ~L^ -1 ~s^ -1 . The rate

The given graph is a representation of kinetics of a reaction. The y and x axes for zero and first order reactions, respectively are

For a first order reaction A → Products, initial concentration of A is 0 . 1M , which becomes 0 . 001M after 5 minutes. Rate constant for the reaction in min ^ - 1 is

For a reaction A → B, enthalpy of reaction is - 4 . 2kJ mol ^ - 1 and enthalpy of activation is 9 . 6kJ mol ^ - 1 . The correct potential energy profile for the reaction is shown

The slope of Arrhenius Plot (lnkv/s(1)/(T)) of first order reaction is - 5 × 10 ^ 3 K . The value of E _ a of the reaction is. Choose the correct option for your answer. [Given R

The half-life for a zero order reaction having 0 . 02M initial concentration of reactant is 100s . The rate constant (in mol L ^ - 1 s ^ - 1 ) for the reaction is

In collision theory of chemical reaction, Z _ AB represents

The rate constant for a first order reaction is 4.606 × 10 ^ – 3 s ^ – 1 . The time required to reduce 2.0g of the reactant to 0.2g is :

An increase in the concentration of the reactants of a reaction leads to change in

Assertion : Half-life period of a reaction of first order is independent of initial concentration. Reason : Half-life period for a first order reaction, t_ 1 / 2 =(2.303)/(k) 2 .

The decomposition of NH_3 on platinum surface is zero order reaction. The rates of production of N_2 and H_2 are respectively (k=2.5 × 10^ -4 ~mol ~L^ -1 ~s^ -1 )

For a first order gas phase reaction, A_ (g) 2 B_ (g) +C_ (g) P_0 be initial pressure of A and P_t the total pressure at time ' t '. Integrated rate equation is

What is the activation energy (kJ / mol) for a reaction if its rate constant doubles when the temperature is raised from 300 ~K to 400 ~K ? (R=8.314 ~J ~mol^ -1 ~K^ -1 )

Find out the time required for 2 / 3^ rd completion of a first order reaction, if the value of rate constant is 4.3 × 10^ -4 s^ -1 .

If half-life of a substance is 36 minutes. Find amount left after 2 hrs . Initial amount is 10 gm ?

Formula for half- life of a zero order reaction is

A first order reaction has a rate constant of 2.303 × 10^ -3 ~s^ -1 . The time required for 40 ~g of this reactant to reduce to 10 ~g will be [Given that _ 10 2=0.3010 ]

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

For the chemical reaction N _ 2 (g) + 3 H _ 2 (g) ⇋ 2N H _ 3 (g) , the correct option is:

For a reaction, activation energy E_ a =0 and the rate constant at 200 ~K is 1.6 × 10^6 ~s^ -1 . The rate constant at 400 ~K will be [Given that gas constant R=8.314 JK^ -1 ~mol^

If energy of activation of the reaction is 53.6 ~kJ ~mol^ -1 and the temperature changes from 27^ ∘ C to 37^ ∘ C then the value of ( k_ 37^ ∘ C k_ 27^ ∘ C ) is

Which option is valid for a zero order reaction?

In the reversible reaction, 2 NO_2 k_2 k_1 leftharpoons N_2 O_4 the rate of disappearance of NO_2 is equal to

When initial concentration of the reactant is doubled, what happens to the half-life period of a zero order reaction?

What is the correct difference between first and second order reactions?

The chemical reaction, 2 O_3 3 O_2 proceeds as follows : Step 1: O_3 leftharpoons O_2+O .(fast) Step 2: O+O_3 2 O_2 .(slow) The rate law expression should be

The temperature dependence of a reaction is represented by the Arrhenius equation : k=-(E_a)/(R T)+ A Which among the following is wrong conclusion about the given plot?

In the following graph. The slope of line A B gives the information of the

For the chemical reaction, 2 O_3 leftharpoons 3 O_2 The reaction proceed as follows gathered O_3 leftharpoons O_2+O (fast) O+ O_3 2 O_2 (slow) gathered The rate law expression

A first order reaction is 50 \% completed in 1.26 × 10^ 14 ~s . How much time would it takes for 100\% completion?

A first-order reaction has a specific reaction rate 10 ^ - 2 sec ^ - 1 ⁡ . How much time will it take for 20g the reactant to reduce to 5g ?

Mechanism of a hypothetical reaction X _ 2 + Y _ 2 → 2XY is given below: (i) X _ 2 → X + X(fast) (ii) X + Y _ 2 ⇌ XY + Y(slow) (iii) X + Y → XY(fast) The overall order of the

During the decomposition of H_2 O_2 to give oxygen, 48 ~g O_2 is formed per minute at a certain point of time. The rate of formation of water at this point is

A first order reaction, which is 30 \% complete in 30 minutes has a half-life period of

Look at the graph Choose the correct equation from the following which best suited to the above graph

Two similar reactions have the same rate constant at 25^ ∘ C , but at 35^ ∘ C , one of the reaction has a higher rate constant than the other. The appropriate reason for this is

At radioactive equilibrium, the ratio between two atoms of radioactive elements A and B is 3.1 × 10^9: 1 . If the half-life period of A is 2 × 10^ 10 yrs, then the half-life of B

The decomposition of phosphine (P H _ 3 ) on tungsten at low pressure is a first-order reaction. It is because the

The rate of a first-order reaction is 0.04mol l ^ - 1 s ^ - 1 at 10 second and 0.03mol l ^ - 1 s ^ - 1 at 20 seconds after initiation of the reaction. The half-life period of the

The addition of a catalyst during a chemical reaction alters which of the following quantities?

In a decay process _Z^A X changes into _ Z-1 ^A Y . Which process is this?

For reaction a A arrow x P , when [A]=2.2 mM , the rate was found to be 2.4 mM s^ -1 . On reducing concentration of A to half, the rate changes to 0.6 mM s^ -1 . The order of

A hypothetical reaction, X_2+Y_2 2 X Y follows the following mechanism X_2 leftharpoons X+X … . . . . . . . fast X+Y_2 X Y+Y … … slow X+Y X Y .......... fast The order of the

The variation of concentration of the product P with time in the reaction, A arrow P is shown in following graph. The graph between (-d[A])/(d t) and time will be of the type

The rate constant of the reaction A ⟶ B is 0.6 × 10 ^ - 3 mole per liter per second. If the initial concentration of A is 5 M, then the concentration of B after 20 minutes is:

The activation energy of a reaction can be determined from the slope of which of the following graphs?

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is:

75 \% of a zero order reaction complete in 4 ~h 87.5 \% of the same reaction completes in

For the reaction A_ (g) B_ (g) +C_ (g) , the rate constant is given as (P_i. is initial pressure and P_t is pressure at time t )

Observe the following reaction 2 A+B C The rate of formation of C is 2.2 × 10^ -3 ~mol ~L^ -13 ~min^ -1 . What is the value of -(d[A])/(d t)(. in .mol L^ -1 ^ -1 ) ?

The plot of a concentration of the reactant versus time for a reaction is a straight line with a negative slope. The reaction follows a

For a reaction between A and B the order with respect to A is 2 and the other with respect to B is 3 . The concentrations of both A and B are doubled, the rate will increase by a