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
 

Consider the two rate laws:

(I) Rate = k [A]^1/2 [B]^3/2

(II) Rate = k [A]^3/2 [B]^–1

The correct statement among the following is-
 

Consider the following values of rate constant:

(i) k = 2.3 × 10^–5 L mol^–1 s^–1

(ii) k = 3 × 10^–4 s^–1

The correct statement among the following is-

The initial concentration of N₂O₅ in the following first-order reaction N₂O₅(g) → 2 NO₂(g) + 1/2 O₂ (g) was 1.24 × 10^–2 mol L^–1 at 318 K. The concentration of N₂O₅ after 60 minutes was 0.20 × 10^–2 mol L^–1. The rate constant value at 318 K is-

 1. 0.304 min^-1
2. 0.00304 min^-1
3. 0.0304 min^-1
4. 3.04 min^-1

The following data were obtained during the first order thermal decomposition of N₂O₅ (g) at constant volume:

$2N_2{O}_5\left(g\right) \to 2N_2{O}_4\left(g\right) + O_2\left(g\right)$
 

The rate constant value is-

1. \(5.98\times 10^{-4}\) sec^-1
2. \(4.98\times 10^{-4}\) sec^-1
3. \(6.98\times 10^{-4}\) sec^-1
4. \(7.98\times 10^{-4}\) sec^-1

A first-order reaction is found to have a rate constant, k = 5.5 × 10^-14 s^-1. The half-life of the reaction is-

1. 1.66 × 10¹³ s
2.  1.46 × 10¹³ s
3. 1.36 × 10¹³ s
4. 1.26 × 10¹³ s



 

In a first order reaction, time required for completion of 99.9% is X times of half-life (t_1/2) of the reaction. When reaction is completed 99.9%, [R]_n = [R]₀ – 0.999[R]₀ .The value of X is-

1. 5
2. 10
3. 15
4. 20

The rate constants of a reaction at 500K and 700K are 0.02s^–1 and 0.07s^–1 respectively. The values of E_a is-

1. 15.6 kJ
2. 13.7 kJ
3. 18.2 kJ
4. 17.5 kJ

The first-order rate constant for the decomposition of ethyl iodide by the reaction

C₂H₅I(g) → C₂H₄ (g) + HI(g)

at 600K is 1.60 × 10^–5 s^–1. Its energy of activation is 209 kJ/mol. The rate constant of the reaction at 700K is-

1. 7.56 × 10^–3 s^–1
2. 6.36 × 10^–3 s^–1
3. 5.16 × 10^–3 s^–1
4. 5.76 × 10^–3 s^–1