For a chemical reaction represented by the overall equation , the experimentally observed rate law i — Chemical Kinetics Chemistry Question
Question
For a chemical reaction represented by the overall equation $aA + bB \rightarrow \text{Products}$, the experimentally observed rate law is $r = k[A]^x[B]^y$. Which of the following statements is/are generally true?
Answer: A,B
💡 Solution & Explanation
The overall order is defined as the sum of powers in the rate law ($x+y$). Molecularity is only defined for elementary reactions, where it equals the sum of reacting molecules ($x+y = a+b$). For complex reactions, overall molecularity has no meaning. Exponents $x$ and $y$ are found experimentally.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes