Solution Found!
Consider the following mechanism:(1) (2) (3) (a) What is
Chapter 16, Problem 62P(choose chapter or problem)
Consider the following mechanism:
(a) What is the overall equation?
(b) Identify the intermediate(s), if any.
(c) What are the molecularity and the rate law for each step?
(d) Is the mechanism consistent with the actual rate law:
\(\text { rate }=k\left[\mathrm{ClO}^{-}\right]\left[\mathrm{I}^{-}\right] ?\)
Equation Transcription:
Text Transcription:
rate=k[ClO^-][I^-]?
Questions & Answers
QUESTION:
Consider the following mechanism:
(a) What is the overall equation?
(b) Identify the intermediate(s), if any.
(c) What are the molecularity and the rate law for each step?
(d) Is the mechanism consistent with the actual rate law:
\(\text { rate }=k\left[\mathrm{ClO}^{-}\right]\left[\mathrm{I}^{-}\right] ?\)
Equation Transcription:
Text Transcription:
rate=k[ClO^-][I^-]?
ANSWER:Solution 62P
Step 1
(a) We have to write the overall equation.
In order to write the overall reaction, we have to add all the three equations.
(1) ClO-(aq) + H2O(l) ⇆ HClO(aq) + OH-(aq) [fast]
(2) I-(aq) + HClO(aq) → HIO (aq) + Cl-(aq) [slow]
(3) OH-(aq) + HIO (aq) → H2O(l) + IO-(aq) [fast]
ClO-(aq) + I-(aq) → Cl-(aq) + IO-(aq)
Thus the overall reaction is found to be,
ClO-(aq) + I-(aq) → Cl-(aq) + IO-(aq)