Select the correct option based on statements below:

Assertion (A):	For elementary reactions, the law of mass action and the rate of law expression are generally the same.
Reason (R):	The molecularity of an elementary reaction is always one.

 

1.	Both (A) and (R) are true and (R) is the correct explanation of (A).
2.	Both (A) and (R) are true but (R) is not the correct explanation of (A).
3.	(A) is true but (R) is false.
4.	Both (A) and (R) are false.

For a reaction A → B, the Arrhenius equation is given as  \(log_{e}k \ = \ 4 \ - \ \frac{1000}{T}\) the activation energy in J/mol for the given reaction will be:

1. 8314

2. 2000

3. 2814

4. 3412

If a reaction A + B → C is exothermic to the extent of 30 kJ mol⁻¹ and the forward reaction has an activation energy of 249 kJ mol⁻¹, the activation energy for the reverse reaction in kJ mol^-1 will be:

For the reaction 2A + B → 2C, Rate = k[A]²[B].
Find the factor by which the rate changes when the vessel volume is reduced to one-fourth.

1. 0.25                                                          

2. 16

3. 64                                                             

4. 4.0

When the temperature of a reaction increases from 300 K to 310 K, the rate of the reaction doubles. What is the activation energy for this reaction?

 \((R=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \text { and } \log 2=0.301)\)

The rate constant for a first-order reaction is $4.606\times {10}^{-3}$ $s^{-1}$. The time required to reduce 2.0 g of the reactant to 0.2 g will be:

For a general reaction A $\to$ B, the plot of the concentration of A vs. time is given in the figure.
 

The slope of the curve will be:

The decomposition of hydrocarbons follows the equation: k = (4.5 × 10¹¹s^–1) e^–28000K/T

The activation energy (E_a) for the reaction would be:
1. 232.79 kJ mol^–1
2. 245.86 kJ mol^–1
3. 126.12 kJ mol^–1
4. 242.51 kJ mol^–1

The role of a catalyst is to change: 

The correct statement based on the graph below is: