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

The reaction of hydrogen and iodine monochloride is given as: 
H₂(g) + 2ICl(g) → 2HCl(g) + I₂(g) 
This reaction is of first order with respect to H₂(g) and ICl(g), for which of the following proposed mechanisms:
Mechanism A: 
H₂(g) + 2ICl(g) → 2HCl(g) + I₂(g) 
Mechanism B: 
H₂(g) + ICl(g) →HCl(g) + HI(g); slow 
HI(g) + ICl(g) →HCl(g) + I₂(g); fast

1. B Only

2. A and B both

3. Neither A nor B

4. A only

If 'a' is the initial concentration of a substance that reacts according to zero-order kinetics and k is the rate constant, then the time for the reaction to go to completion is:
1. a/k
2. 2/ka
3. k/a
4. 2k/a

Consider the first-order gas-phase decomposition reaction given below.

A(g) → B(g) + C(g)

The initial pressure of the system before the decomposition of A was ${\mathrm{P}}_{\mathrm{i}}$. After the lapse of time t, the total pressure of the system increased by X units and became ${\mathrm{P}}_{\mathrm{t}}$. The rate constant k for the reaction is:

1. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{P_{\mathrm{i}}-\mathrm{x}}$

2. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{2P_{\mathrm{i}}-P_{\mathrm{t}}}$

3. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{2P_{\mathrm{i}}+P_{\mathrm{t}}}$

4. $\mathrm{k}=\frac{2.303}{\mathrm{t}}\log \frac{P_{\mathrm{i}}}{P_{\mathrm{i}}+\mathrm{x}}$

The correct graphical representation of first-order reaction is:

(a)		(b)
(c)		(d)

Codes

Select the correct option based on statements below:

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

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