For the reaction O₃(g) + O(g) → 2O₂(g), if the rate law expression is, rate = k [O_,][O], the molecularity and order of the reaction respectively are

• 2 and 2

• 2 and 1.33

• 2 and 1

• 1 and 2

The relationship between rate constant and half-life period of zero order reaction is given by

• ${\mathrm{t}}_{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.}$ = [A₀] 2k

• ${\mathrm{t}}_{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.}$ = $\frac{0.693}{\mathrm{k}}$

• ${\mathrm{t}}_{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.} = \frac{\left[{\mathrm{A}}_0\right]}{2 \mathrm{k}}$

• ${\mathrm{t}}_{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.} = \frac{2 \left[{\mathrm{A}}_0\right]}{\mathrm{k}}$

Half-life period of a first order reaction, A → product is 6.93 h. What is the value of rate constant?

• 1.596 h^-1

• 0.1 h^-1

• 4.802 h^-1

• 10 h^-1

Which among the following reactions is an example of pseudo first order reaction?

• Inversion of cane sugar

• Decomposition of H₂O₂

• Conversion of cyclopropane to propene

• Decomposition of N₂O₅

The rate constant for a first order reaction is 7.0 × 10^-4 s^-1. If initial concentration of reactant is 0.080 M, what is the half life of reaction?

• 990 s

• 79.2 s

• 12375 s

• 10.10 × 10^-4 s

The rate constant of the reaction, 2N₂O₅ → 4NO₂ + O₂ at 300 K is 3 × 10^-5 s^-1. If the rate of the reaction at the same temperature is 2.4 × 10^-5 mol dm^-3 s^-1, then the molar concentration of N₂O₅ is

• 0.4 M

• 0.8 M

• 0.04 M

• 0.08 M

In the reaction, A → Products, when the concentration of A was reduced from 2.4 × 10^-2 M to 1.2 × 10^-2 M, the rate decreased 8 times at the same temperature; The order of the reaction is

• 0

• 1

• 2

• 3

The half-life period of a first order reaction having rate constant k = 0.231 × 10^-10 s^-1  will be

• 32 × 10¹⁰ s

• 2 × 10¹⁰ s

• 3 × 10¹⁰ s

• 2 × 10^-10 s

For the reaction X → Y, the concentrations of 'X' are 1.2 M, 0.6 M, 0.3 Mand 0.15 M at 0, 1, 2 and 3 hours respectively. The order of the reaction is

• zero

• half

• one

• two

In a reaction, 2A + B → 3C, the concentration of A decreases from 0.5 mol L^-1 to 0.3 mol L^-1 in 10 minutes. The rate of production of 'C' during this period is

• 0.01 mol L^-1 min^-1

• 0.04 mol L^-1 min^-1

• 0.05 mol L^-1 min^-1

• 0.03 mol L^-1 min^-1