Assertion (A): Order of reaction is applicable to elementary as well as complex reactions.
Reason (R): Order of a reaction is an experimental quantity.
Show Hint
- Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of Assertion (A).
- Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of Assertion (A).
- Assertion (A) is true, but Reason (R) is false.
- Assertion (A) is false, but Reason (R) is true.
The Correct Option is A
Solution and Explanation
Order of reaction is the sum of powers of concentration terms in the experimentally determined rate law. For example: \[ Rate=k[A]^m[B]^n \] Then: \[ \text{Order}=m+n \] Order is not necessarily equal to stoichiometric coefficients.
Step 1: Check the Assertion.
Order of reaction can be defined for elementary reactions. It can also be defined for complex reactions because every reaction can have an experimentally determined rate law. Therefore, Assertion is true.
Step 2: Check the Reason.
Order of reaction is determined experimentally. It cannot always be predicted from the balanced chemical equation. Therefore, Reason is true.
Step 3: Check whether Reason explains Assertion.
Since order is based on experimentally obtained rate law, it can be applied to both elementary and complex reactions. So Reason correctly explains Assertion. Hence: \[ \boxed{\text{(A)}} \]
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- Write IUPAC names of the following coordination entities:
(a) \( [Fe(en)_2Cl_2]^+ \)
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} Write IUPAC names of the following coordination entities:
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(c) \( [Ni(CN)_4]^{2-} \)- Assertion (A): Order of reaction is applicable to elementary as well as complex reactions.
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