AIPMT Mains Chemistry Chemical Kinetics Class 12 Questions

Activation energy (Eₐ) and rate constants (k₁ and k₂) of a chemical reaction at two different temperatures (T₁ and T₂) are related by:

The unit of rate constant for a zero order reaction is

The rate of the reaction 2N₂O₅ → 4NO₂ + O₂ can be written in three ways: -d[N₂O₅]/dt = k[N₂O₅], d[NO₂]/dt = k'[N₂O₅], d[O₂]/dt = k''[N₂O₅]. The relationship between k and k' and between k and k'' are

The half life of a substance in a certain enzyme-catalysed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg L⁻¹ to 0.04 mg L⁻¹ is

The figure given below shows the conversion of a substrate into product by an enzyme. In which one of the four options (1–4) the components of reaction labelled as A, B, C and D are identified correctly?

The rate of the reaction 2NO + Cl₂ → 2NOCl is given by the rate equation rate = k[NO]²[Cl₂]. The value of the rate constant can be increased by

For the reaction N₂ + 3H₂ → 2NH₃, if (d[NH₃]/dt = 2 × 10⁻⁴ mol L⁻¹ s⁻¹, the value of (-d[H₂]/dt would be :

In the reaction BrO₃⁻ (aq) + 5 Br⁻(aq) + 6H⁺ → 3 Br₂(l) + 3 H₂O(l). The rate of appearance of bromine (Br₂) is related to rate of disappearance of bromide ions as following:

Half life period of a first-order reaction is 1386 seconds. The specific rate constant of the reaction is:

For the reaction A + B → products, it is observed that: (a) on doubling the initial concentration of A only, the rate of reaction is also doubled and (b) on doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction. The rate of this reaction is given by:

The bromination of acetone that occurs in acid solution is represented by this equation CH₃COCH₃(aq) + Br₂(aq) → 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 0.05 0.05 0.20 Initial rate, disappearance of Br₂, M s⁻¹ 5.7 × 10⁻⁵ 5.7 × 10⁻⁵ 1.2 × 10⁻⁴ 3.1 × 10⁻⁴ Based on these data, the rate equation is

The rate constants k₁ and k₂ for two different reactions are 10¹⁶ · e⁻²⁰⁰⁰/ᵀ and 10¹⁵ · e⁻¹⁰⁰⁰/ᵀ respectively. The temperature at which k₁ = k₂ is