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Previous year question hub

Chemical Kinetics - Physical Chemistry - Chemistry Previous Year Questions

Practice Chemical Kinetics - Physical Chemistry - Chemistry previous year questions organised from real papers, with year-wise coverage and clear topic navigation.

37Papers
26Years
75Questions
1Topics

Chemical Kinetics question pattern

Every graph below is calculated only from this selection.

Questions by year

Year-wise coverage for Chemical Kinetics. Each bar uses a separate theme-derived color.

Difficulty distribution

How the classified questions are distributed by difficulty.

Not classified 69 92%
Easy 4 5.3%
Medium 2 2.7%

Question type distribution

MCQ, numerical, multiple-select and other formats found in these papers.

Multiple Choices 75 100%

Subject weightage

Top subjects by unique question coverage.

Chemistry
75 Qs

Most asked topics

Top topics across the included previous year papers.

Physical Chemistry
75 Qs

Subtopic coverage

Top subtopics inside this exact selection.

Chemical Kinetics
75 Qs

Paper coverage

Question coverage for the most populated papers. Every active PYP paper remains listed below.

NEET 2026
3 Qs
NEET 2025
2 Qs
NEET 2024
3 Qs
NEET 2024 RE EXAMINATION
3 Qs
NEET 2023
2 Qs
NEET 2023 MANIPUR
2 Qs
NEET 2022 Phase 1
2 Qs
NEET 2022 PHASE 2
1 Qs
NEET 2021
2 Qs
NEET 2020 PHASE 1
2 Qs
AIIMS 2019
2 Qs
NEET 2019
2 Qs
AIIMS 2018
3 Qs
NEET 2018
2 Qs
NEET 2017
2 Qs
NEET 2016 PHASE 1
2 Qs
NEET 2016 PHASE 2
1 Qs
AIPMT 2015 Cancelled Paper
2 Qs
AIPMT 2015
1 Qs
NEET 2013 KARNATAKA
2 Qs
NEET 2013
1 Qs
AIPMT 2012 PRELIMS
2 Qs
AIPMT 2012 MAINS
1 Qs
AIPMT 2011 MAINS
3 Qs
AIPMT 2011 PRELIMS
1 Qs
AIPMT 2010 PRELIMS
2 Qs
AIPMT 2010 MAINS
1 Qs
AIPMT 2009
4 Qs
AIPMT 2008
2 Qs
AIPMT 2007
3 Qs
AIPMT 2006
2 Qs
AIPMT 2005
2 Qs
AIPMT 2004
1 Qs
AIPMT 2003
4 Qs
AIPMT 2002
1 Qs
AIPMT 2001
2 Qs
AIPMT 2000
2 Qs

Included previous year papers

Newest papers appear first. Sort by year, question coverage or name.

PaperYear / sessionQuestions in this viewOpen
NEET 202620263View paper
NEET 202520252View paper
NEET 202420243View paper
NEET 2024 RE EXAMINATION20243View paper
NEET 202320232View paper
NEET 2023 MANIPUR20232View paper
NEET 2022 Phase 120222View paper
NEET 2022 PHASE 220221View paper
NEET 202120212View paper
NEET 2020 PHASE 120202View paper
AIIMS 201920192View paper
NEET 201920192View paper
AIIMS 201820183View paper
NEET 201820182View paper
NEET 201720172View paper
NEET 2016 PHASE 120162View paper
NEET 2016 PHASE 220161View paper
AIPMT 201520151View paper
AIPMT 2015 Cancelled Paper20152View paper
NEET 201320131View paper
NEET 2013 KARNATAKA20132View paper
AIPMT 2012 MAINS20121View paper
AIPMT 2012 PRELIMS20122View paper
AIPMT 2011 MAINS20113View paper
AIPMT 2011 PRELIMS20111View paper
AIPMT 2010 MAINS20101View paper
AIPMT 2010 PRELIMS20102View paper
AIPMT 200920094View paper
AIPMT 200820082View paper
AIPMT 200720073View paper
AIPMT 200620062View paper
AIPMT 200520052View paper
AIPMT 200420041View paper
AIPMT 200320034View paper
AIPMT 200220021View paper
AIPMT 200120012View paper
AIPMT 200020002View paper

All Chemical Kinetics previous year questions

Practice every matching question in batches of 20, with every available option.

1
2000 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2000
How enzymes increases the rate of reactions
A
by lowering activation energy
B
by increaing activation energy
C
by changing equilibrium constant
D
by forming enzyme substrate complex.
Open complete paper
2
2000 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2000
For the reaction H+ + BrO\(_3^ -\) + 3Br\(-\) \(\to\) 5Br2 + H2O
which of the following relation correctly represents the consumption and formation of products.
A
\({{d\left[ {B{r^ - }} \right]} \over {dt}} = - {3 \over 5}{{d\left[ {B{r_2}} \right]} \over {dt}}\)
B
\({{d\left[ {B{r^ - }} \right]} \over {dt}} = {3 \over 5}{{d\left[ {B{r_2}} \right]} \over {dt}}\)
C
\({{d\left[ {B{r^ - }} \right]} \over {dt}} = - {5 \over 3}{{d\left[ {B{r_2}} \right]} \over {dt}}\)
D
\({{d\left[ {B{r^ - }} \right]} \over {dt}} = {5 \over 3}{{d\left[ {B{r_2}} \right]} \over {dt}}\)
Open complete paper
3
2001 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2001
When a bio-chemical reaction is carried out in laboratory, outside the human body in absence of enzyme, then rate of reaction obtained is 10\(-\)6 times, the activation energy of reaction in the presence of enzyme is
A
6/RT
B
P is required
C
different from E\(a\) obtained in laboratory
D
can't say anything.
Open complete paper
4
2001 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2001
For the reaction;

2N2O5 \(\to\) 4NO2 + O2 rate and rate constant are 1.02 \(\times\) 10\(-\)4 and 3.4 \(\times\) 10\(-\)5 sec\(-\)1 respectively, then concentration of N2O5 at that time will be
A
1.732
B
3
C
1.02 \(\times\) 10\(-\)4
D
3.4 \(\times\) 105
Open complete paper
5
2002 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2002
2A \(\to\) B + C

It would be a zero order reaction when
A
the rate of reaction is proportional to square of concentration of A
B
The rate of reaction remains same at any concentration of A
C
the rate remains unchanged at any concentration of B and C
D
the rate of reaction doubles if concentrations of B is increased to double.
Open complete paper
6
2003 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2003
The reaction A \(\to\) B follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B?
A
1 hour
B
0.5 hour
C
0.25 hour
D
2 hours
Open complete paper
7
2003 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2003
The activation energy for a simple chemical reaction A \(\rightleftharpoons\) B is E\(a\) in forward direction.
The activation energy for reverse reaction
A
is negative of E\(a\)
B
is always less than E\(a\)
C
can be less than or more than E\(a\)
D
is always double of E\(a\)
Open complete paper
8
2003 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2003
The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, \(k = A \cdot {e^{ - E{}^ * /RT}}\). Activation energy (E\(*\)) of the reaction can be calculated by plotting
A
\(k\,\,vs\,\,T\)
B
\(k\,\,vs\,\,{1 \over {\log T}}\)
C
\(\log \,k\,\,vs\,\,{1 \over T}\)
D
\(\log \,k\,\,vs\,{1 \over {\log T}}\)
Open complete paper
9
2003 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2003
If the rate of the reaction is equal to the rate constant, the order of the reaction is
A
0
B
1
C
2
D
3
Open complete paper
10
2004 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2004
The rate of a first order reaction is 1.5 \(\times\) 10\(-\)2 mol L\(-\)1 min\(-\)1 at 0.5 M concentration of the reactant. The half-life of the reaction is
A
0.383 min
B
23.1 min
C
8.73 min
D
7.53 min
Open complete paper
11
2005 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2005
The rate of reaction between two reactions A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is
A
2
B
\(-\)2
C
1
D
\(-\)1
Open complete paper
12
2005 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2005
For a first order reaction A \(\to\) B the reaction rate a reactant concentration of 0.01 M is found to be 2.0 \(\times\) 10\(-\)5 mol L\(-\)1 s\(-\)1. The half-life period of the reaction is
A
30 s
B
220 s
C
300 s
D
347 s
Open complete paper
13
2006 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2006
For the reaction, 2A + B \(\to\) 3C + D, which of the following does not express the reaction rate?
A
\(- {{d\left[ A \right]} \over {2dt}}\)
B
\(- {{d\left[ C \right]} \over {3dt}}\)
C
\(- {{d\left[ B \right]} \over {dt}}\)
D
\({{d\left[ D \right]} \over {dt}}\)
Open complete paper
14
2006 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2006
Consider the reaction :  N2(g) + 3H2(g) \(\to\) 2NH3(g)

The equality relationship between \({{d\left[ {N{H_3}} \right]} \over {dt}}\) and \(- {{d\left[ {{H_2}} \right]} \over {dt}}\) is
A
\({{d\left[ {N{H_3}} \right]} \over {dt}} = - {{d\left[ {{H_2}} \right]} \over {dt}}\)
B
\({{d\left[ {N{H_3}} \right]} \over {dt}} = - {1 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}\)
C
\(+ {{d\left[ {N{H_3}} \right]} \over {dt}} = - {2 \over 3}{{d\left[ {{H_2}} \right]} \over {dt}}\)
D
\(+ {{d\left[ {N{H_3}} \right]} \over {dt}} = - {3 \over 2}{{d\left[ {{H_2}} \right]} \over {dt}}\)
Open complete paper
15
2007 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2007
The reaction of hydrogen and iodine monochloride is given as :
H2(g) + 2ICl(g) \(\to\) 2HCl(g) + I2(g)
This reaction is of first order with respect to H2(g) and ICl(g),
following mechanisms were proposed.

Mechanism A :
     H2(g) + 2ICl(g) \(\to\) 2HCl(g) + I2(g)
Mechanism B :
     H2(g) + ICl(g) \(\to\) HCl(g) + HI(g) ; slow
     HI(g) + ICl(g) \(\to\) HCl(g) + I2(g) ; fast

Which of the above mechanism(s) can be consistent with the given information about the reaction?
A
A and B both
B
Neither A nor B
C
A only
D
B only
Open complete paper
16
2007 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2007
If 60% of a first order reaction was completed in 60 minutes, 50% of the same reaction would be completed in approximately
(log 4 = 0.60, log 5 = 0.69)
A
45 minutes
B
60 minutes
C
40 minutes
D
50 minutes
Open complete paper
17
2007 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2007
In a first-order reaction A \(\to\) B, if k is rate constant and initial concentration of the reactant A is 0.5 M, then the half-life is
A
\({{\log 2} \over k}\)
B
\({{\log 2} \over {k\sqrt {0.5} }}\)
C
\({{\ln 2} \over k}\)
D
\({{0.693} \over {0.5k}}\)
Open complete paper
18
2008 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2008
The rate constants k1 and k2 for two different reactions are 1016 \(\cdot\) e\(-\)2000/T and 1015 \(\cdot\) e\(-\)1000/T, respectively.
The temperature at which k1 = k2 is
A
2000 K
B
\({{1000} \over {2.303}}K\)
C
1000 K
D
\({{2000} \over {2.303}}K\)
Open complete paper
19
2008 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2008
The bromination of acetone that occurs in acid solution is represented by this equation.
CH3COCH3(aq) + Br2(aq)  \(\to\)
     CH3COCH2Br(aq) + H+(aq) + Br\(-\)(aq)
These kinetic data were obtained for given reaction concentrations.
Initial concentrations, M
[CH3COCH3 [Br2] [H+]
0.30 0.05 0.05
0.30 0.10 0.05
0.30 0.10 0.10
0.40 0.05 0.20

Initial rate, disappearance of Br2, Ms\(-\)1
5.7\(\times\)10\(-\)5
5.7\(\times\)10\(-\)5
1.2\(\times\)10\(-\)4
3.1\(\times\)10\(-\)4

Based on these data, the rate equation is
A
Rate = k[CH3COCH3][Br2][H+]2
B
Rate = k[CH3COCH3][Br2][H+]
C
Rate = k[CH3COCH3][H+]
D
Rate = k[CH3COCH3][Br2]
Open complete paper
20
2009 · Chemistry · Physical Chemistry · Chemical Kinetics
AIPMT 2009
In the reaction,
BrO\(_{3(aq)}^ -\) + 5Br\(_{(aq)}^ -\) + 6H+ \(\to\) 3Br2(l) + 3H2O(l).
The rate of appearance of bromine (Br2) is related to rate of disappearance of bromide ions as
A
\({{d\left[ {B{r_2}} \right]} \over {dt}} = - {5 \over 3}{{d\left[ {B{r^ - }} \right]} \over {dt}}\)
B
\({{d\left[ {B{r_2}} \right]} \over {dt}} = {5 \over 3}{{d\left[ {B{r^ - }} \right]} \over {dt}}\)
C
\({{d\left[ {B{r_2}} \right]} \over {dt}} = {3 \over 5}{{d\left[ {B{r^ - }} \right]} \over {dt}}\)
D
\({{d\left[ {B{r_2}} \right]} \over {dt}} = - {3 \over 5}{{d\left[ {B{r^ - }} \right]} \over {dt}}\)
Open complete paper

Showing 20 of 75 questions