Select the correct option based on statements below:

Assertion (A):	Base catalyzed hydrolysis of ethyl acetate is a first-order reversible reaction.
Reason (R):	The order of reaction always depends on the stoichiometry of the reaction.

 

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:-

${6\mathrm{H}}^{+}+ 5{\mathrm{Br}}^{-}+ \mathrm{Br}{\mathrm{O}}_3^{-}\to 3{\mathrm{Br}}_2+ 6{\mathrm{H}}_2\mathrm{O}$

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 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 $4.606\times {10}^{-3} s^{-1}$. The time required to reduce 2.0 g of the reactant to 0.2 g is: