Match the statements in Column I and Column II :

Column I		Column II
A.	Catalyst alters the rate of reaction	1.	Proper orientation is not there always
B.	${\mathrm{e}}^{-{\mathrm{E}}_{\mathrm{a}}/\mathrm{RT}}$	2.	By lowering the activation energy
C.	Energetically favorable reactions are sometimes slow	3.	Total probability is one
D.	Area under the Maxwell-Boltzmann curve is constant	4.	Refers to the fraction of molecules with energy equal to or greater than the activation energy

Codes

	A	B	C	D
1.	2	4	1	3
2.	3	1	4	2
3.	1	4	3	2
4.	3	4	1	2

Select the correct option based on statements below:

The correct graphical representation of first-order reaction is:

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

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

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

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