The decomposition of N₂O₅ in CCl₄ at 318K has been studied by monitoring the concentration of N₂O₅ in the solution. Initially, the concentration of N₂O₅ is 2.33 mol L^–1 and after 184 minutes, it is reduced to 2.08 mol L^–1. The reaction takes place according to the equation

2 N₂O₅ (g) → 4 NO₂ (g) + O₂ (g)

The rate of production of NO₂ during this period is-

1. 5.72 × 10^–3 mol L^–1 min^–1
2. 2.72 × 10^–3 mol L^–1 min^–1
3. 1.72 × 10^–5 mol L^–1 min^–1
4. 6.72 × 10^–4 mol L^–1 min^–1

The rate equation for the reaction 2A+B→C is found to be:
rate = k [A] [B]
The correct statement in relation to this reaction is that the:

For the reaction, 2A → B, rates= k[A]². If the concentration of reactant is doubled, then the:

Identify the set of correct statements & choose the correct answer from the options given below:

The rate constant for a reaction of zero-order in A is 0.0030 mol L^-1 s^-1. How long will it take for the initial concentration of A to fall from 0.10 M to 0.075 M?

1. 8.3 sec

2. 0.83 sec

3. 83 sec

4. 10.3 sec