March 29, 2024, 02:15:55 AM
Forum Rules: Read This Before Posting


Topic: Why does this happen in the rate law  (Read 1369 times)

0 Members and 1 Guest are viewing this topic.

Offline sodium.dioxid

  • Regular Member
  • ***
  • Posts: 72
  • Mole Snacks: +1/-3
Why does this happen in the rate law
« on: May 11, 2012, 03:01:35 PM »
In a nutshell, this ---> rate = k [A]2 <--- doesn't make sense


Consider a bimolecular reaction in which a molecule has to collide with one of its own kind to form a product. That is, one for which the rate is k[A]2

The way I seem to understand this process is by breaking up A into two halves and considering them to be two different species (I am pretending to dress up half of the A molecules and disguise them as another species)

So, A = B + C, where B=A/2 and C=A/2. Thus, rate law becomes k*B*C

Why do these two rate laws give different results?

Basically, why isn't the rate law k[A/2]2 instead of k[A]2?



EDIT: Sorry, I see my fallacy now.
« Last Edit: May 11, 2012, 03:31:16 PM by sodium.dioxid »

Sponsored Links