Practice & Test Chemical Kinetics

Class 12 Chemistry · Chapter 3. Practice 53 free NEET 2027 questions on Chemical Kinetics (Class 12 Chemistry), across 22 concepts. Asked ~3.5× per paper since 2013.

53
Practice questions
22
Concepts tagged
45
Asked 2013–2025
3.5×
Per paper

How much does Chemical Kinetics matter?

Across the 13 NEET papers from 2013 to 2025, Chemical Kinetics has been examined 45 times — an average of 3.5 questions per paper. At 4 marks each, that is roughly 14 marks a year riding on this one chapter.

What gets asked: 22 concepts

Every question in the bank is tagged to one of these, so practice can target the exact idea you keep missing.

Activation EnergyArrhenius Collision TheoryArrhenius EquationCollision Theory of Chemical ReactionsDetermination of Order of ReactionDifference between Order and Molecularity of a ReactionEffect of Concentration of Reactants on Rate of a ReactionEffect of Temperature on Rate of a ReactionHalf-life Vs Initial Concentration graph for First Order ReactionIntegrated Rate Equation for First Order ReactionsIntegrated Rate Equations of Chemical ReactionMechanism of a Chemical ReactionMolecularity of a ReactionOrder of a ReactionRate Constant of a Chemical ReactionRate Law Expression of a Chemical ReactionRate law: Law of mass actionRate of a Chemical ReactionRate-Time Graph for First Order ReactionRate-Time Graph for Zero Order ReactionTime-Concentration Graphs for Second Order Reaction with One ReactantUnits of Rate Constant

Sample questions

Question 1

The energy profile shown has two transition states and one intermediate. This mechanism corresponds to:

Question 2

Assertion (A): The rate of reaction usually decreases with a decrease in temperature. Reason (R): Lowering the temperature decreases the number of collisions between reactant molecules, and also decreases the fraction of molecules with activation energy.

Question 3

The rate constant for the first order decomposition of a certain reaction is described by the equation In $k\left(s^{-1}\right) = 14.34 - \dfrac{1.25 \times 10^{4}K}{T}$. The energy of activation for this reaction is

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