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
 

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

If 75 % of a first order reaction was completed in 90 minutes, 60 % of the same reaction would be completed in approximately (in minutes)-

(Take : log 2 = 0.30 ; log 2.5 = 0.40)

1. 50 min

2. 60 min

3. 70 min

4. 65 min

The rate of a reaction is decreased by 3.555 times when the temperature was changed from 40°C to 30°C. The activation energy (in kJ ${\mathrm{mol}}^{-1}$) of the reaction is- (Take R=8.314 J ${\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$ In 3.555=1.268)
1. 100 kJ/mol
2. 120 kJ/mol
3. 95 kJ/mol
4. 108 kJ/mol

For the non – stoichiometry reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiments (all at 298 K).

The rate law for the formation of C is:

1. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}{]}^2\right[\mathrm{B}]$

2. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right][\mathrm{B}{]}^2$

3. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]$

4. $\frac{\mathrm{dc}}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]\left[\mathrm{B}\right]$

The time for the half-life period of a certain reaction A → Products is 1 hour. When the initial concentration of the reactant 'A' is 2.0 mol L^-1, the time taken for its concentration to come from 0.50 to 0.25 mol L^-1 ,if it is a zero-order reaction, is-

1. 1h

2. 4 h

3. 0.5 h

4. 0.25 h

Consider the reaction, 2A + B → Products.
When concentration of B alone was doubled, the half-life did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:

1. L mol^–1 s^–1

2. no unit

3. mol L^–1s^–1

4. s^–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 a first-order reaction A → B the reaction rate at a reactant concentration of 0.01M is found to be $2.0\times {10}^{-5}\text{ mole }{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$. The half-life period of the reaction is:
1. 300s
2. 30s
3. 220s
4. 347s

Half-life of substance A following first order kinetics is 5 days. Starting with 100g of A, the amount left after 15 days will be: 

1.  25 g 

2. 50 g 

3. 12.5 g 

4. 6.25 g