Q. No.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?
\((R=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \text { and } \log 2=0.301)\)
1.
\(53.6 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
2.
\(68.6 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
3.
\(59.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
4.
\(70.5 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
If 60 % of a first-order reaction is completed in 60 minutes, 50 % of the same reaction takes approximately:
(log4 = 0.60, log5 = 0.69)
| 1. | 55 min | 2. | 45 min |
| 3. | 60 min | 4. | 30 min |
For a reaction of the type 2A + B 2C, the rate of the reaction is given by . When the volume of the reaction vessel is reduced to th of the original volume, the rate of reaction changes by a factor of:
1. 0.25
2. 16
3. 64
4. 4
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:
| 1. | 324 | 2. | 279 |
| 3. | 40 | 4. | 100 |
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:
| Assertion (A): | At very high temperatures (approaches to infinity), the rate constant becomes equal to the collision frequency. |
| Reason (R): | The collision in which molecules collide with proper orientation is called an ineffective collision. |
| 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:
| 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 the statements below:
| Statement 1: | The overall order of a reaction is the sum of the powers of all the reactants in the rate expression. |
| Statement 2: |
Examples of higher-order reactions (order > 2) are abundant. |
| 1. |
Both Statement 1 and Statement 2 are true. |
| 2. |
Both Statement 1 and Statement 2 are false |
| 3. |
Statement 1 is true, but Statement 2 is false. |
| 4. |
Statement 1 is false, but Statement 2 is true. |
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
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
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