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The effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of bi-molecular gaseous reactions (no derivation) Concepts for JEE

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The effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of bi-molecular gaseous reactions (no derivation) is a core JEE Main Chemistry subtopic under Chemical Kinetics. Master the definitions, standard results, and typical MCQ patterns tested in JEE Main and Advanced.

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  • Revise The effect of temperature on the rate of reactions, Arrhenius theory, activation energy and its calculation, collision theory of bi-molecular gaseous reactions (no derivation) with a one-page formula sheet before attempting mixed tests
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Syllabus context

Part of Chemical Kinetics in JEE Main Chemistry.

Free sample questions

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Q1ChemistryUnit 8: Chemical Kinetics
H2H_{2} reacts much faster with Cl2C l_{2} then D2D_{2} because:
Q2ChemistryUnit 8: Chemical Kinetics
Which of the following rules states that with the increase of every 10∘C10^{\circ} \mathrm{C} temperature the rate of metabolic activity gets doubled?
Q3ChemistryUnit 8: Chemical Kinetics
Which of the following statements is not correct about physisorption?
Q4ChemistryUnit 8: Chemical Kinetics
Which one of the following statements is false? This question has multiple correct options
Q5ChemistryUnit 8: Chemical Kinetics
Rate of disappearance of the reactant A\boldsymbol{A} at two different temperature is given by A⇌B\boldsymbol{A} \rightleftharpoons \boldsymbol{B} −d[A]dt=(2×10−2S−1)[A]−4×\frac{-\boldsymbol{d}[\boldsymbol{A}]}{\boldsymbol{d t}}=\left(\boldsymbol{2} \times \mathbf{1 0}^{-2} \boldsymbol{S}^{-1}\right)[\boldsymbol{A}]-\boldsymbol{4} \times 10−3S−1[B],T=300K\mathbf{1 0}^{-3} \boldsymbol{S}^{-\mathbf{1}}[\boldsymbol{B}], \boldsymbol{T}=\mathbf{3 0 0} \boldsymbol{K} −d[A]dt=(4×10−2S−1)[A]−16×\frac{-\boldsymbol{d}[\boldsymbol{A}]}{\boldsymbol{d t}}=\left(\boldsymbol{4} \times \mathbf{1 0}^{-2} \boldsymbol{S}^{-1}\right)[\boldsymbol{A}]-\mathbf{1 6} \times 10−4[B],T=400K\mathbf{1 0}^{-\mathbf{4}}[\boldsymbol{B}], \boldsymbol{T}=\mathbf{4 0 0} \boldsymbol{K} Calculate heat of reaction in the given temperature range, when equilibrium is set⁡\operatorname{set} up.
Q6ChemistryUnit 8: Chemical Kinetics
N2(g)+3H2(g)⇌2NH3(g)+22N_{2}(g)+3 H_{2}(g) \rightleftharpoons 2 N H_{3}(g)+22 kcal. The activation energy for the forward reaction 50 kcal. What is the activation energy for the backward reaction?
Q7ChemistryUnit 8: Chemical Kinetics
The rate constant for a reaction can be increased by a‾\underline{a} the stability of the reactant or by b‾\underline{b} the stability of the transition state. Select the correct choice for a and bb
Q8ChemistryUnit 8: Chemical Kinetics
Catalysts lower the activation energy of a reaction:

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