Question

A chemical reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g) in gas phase was carried out in a closed vessel. The concentration of NO₂ was found to increase by 5 × 10⁻³ mol L⁻¹ in 10 seconds. Calculate:

For the reaction 2N₂O₅(g) → 4NO₂(g) + O₂(g) at 318 K calculate the rate of reaction if rate of disappearance of N₂O₅(g) is 1.4 × 10⁻³ m s⁻¹.

For a first order reaction derive the relationship t₉₉% = 2t₉₀%

In the given reaction N₂(g) + 3H₂(g) → 2NH₃(g) the rate of formation of NH₃ is 3·6 × 10⁻⁴ mol L⁻¹ s⁻¹. Calculate the

Read the following passage and answer the questions that follow : The rate of reaction is concerned with decrease in concentration of reactants or increase in the concentration of products per unit time. It can be expressed as instantaneous rate at a particular instant of time and average rate over a large interval of time. A number of factors such as temperature, concentration of reactants, catalyst affect the rate of reaction. Mathematical representation of rate of a reaction is given by rate law : Rate = k[A]^x [B]^y x and y indicate how sensitive the rate is to the change in concentration of A and B. Sum of x + y gives the overall order of a reaction. When a sequence of elementary reactions gives us the products, the reactions are called complex reactions. Molecularity and order of an elementary reaction are same. Zero order reactions are relatively uncommon but they occur under special conditions. All natural and artificial radioactive decay of unstable nuclei take place by first order kinetics.