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.

Select the correct option based on statements below:

Select the correct option based on statements below:

Select the correct option based on statements below:

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

For a reaction:-

${6\mathrm{H}}^{+}+<mspace\; width="1em"></mspace>5{\mathrm{Br}}^{-}+<mspace\; width="1em"></mspace>\mathrm{Br}{\mathrm{O}}_3^{-}\to 3{\mathrm{Br}}_2+<mspace\; width="1em"></mspace>6{\mathrm{H}}_2\mathrm{O}$

lf rate of consumption of BrO${{}_3}^{-}$ is x mol ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$. Then calculate the rate of formation of Br${}_2$:-

1. $\frac{x}{3}$

2. $\frac{2x}{3}$

3. $\frac{x}{4}$

4. 3x

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:

Which of the following is mismatched?

1.
2.
3.
4.

The half-life of the two samples is 0.1 and 0.4 seconds, respectively. Their concentrations are 200 and 50, respectively. The order of the reactions will be:

1. 0

2. 2

3. 1

4. 4

The rate constant for a first order reaction is $4.606\times {10}^{-3}<mspace\; width="1em"></mspace>s^{-1}$. The time required to reduce 2.0 g of the reactant to 0.2 g is: