Select the correct option based on statements below:
| Assertion (A): | The rate constant determined from the Arrhenius equation is fairly accurate for simple as well as complex molecules. |
| Reason (R): | Reactant molecules undergo chemical change irrespective of their orientation during a 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. |
Both the assertion (A) and reason (R) are false.
Assertion (A): While the Arrhenius equation is accurate for simple molecules, there are deviations for complex molecules. This is because complex molecules often involve additional factors, such as steric effects and specific orientations during collisions, which are not fully accounted for by the Arrhenius equation. Therefore, the rate constant determined from the equation may not always be precise for complex reactions.
Reason (R): This statement is incorrect because the orientation of reactant molecules during collisions is crucial for a chemical reaction to occur. Not all collisions lead to a reaction; only those with the correct orientation and sufficient energy can overcome the activation energy barrier and result in a successful chemical transformation.
Thus, the assertion overstates the accuracy of the Arrhenius equation for complex molecules, and the reason is that it misunderstands the role of molecular orientation in chemical reactions.
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