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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) Revision for JEE

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  1. 1.Core idea: 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)
  2. 2.Relates to other subtopics in Chemical Kinetics
  3. 3.Rate law, order, molecularity
  4. 4.Zero and first-order integrated forms
  5. 5.Master 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) definitions and standard results
  6. 6.Solve 20 timed MCQs for 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)

Syllabus context

Part of Chemical Kinetics in JEE Main Chemistry.

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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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