December 22, 2024, 11:21:25 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Rate Law  (Read 4153 times)

0 Members and 1 Guest are viewing this topic.

Offline TEA1

  • Regular Member
  • ***
  • Posts: 16
  • Mole Snacks: +0/-1
Rate Law
« on: April 27, 2008, 01:11:34 PM »
I had to derive a formula for a reaction order of -1 in A.  The reaction is A arrow B.
Then had to sketch a graph.

I already did the math and all but wanted to know what the formula is.
Also the graph I have is a straigt line going up becuase of positive k value.  Just want to know if I am on the right track. 
Logged

Offline Yggdrasil

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 3215
  • Mole Snacks: +485/-21
  • Gender: Male
  • Physical Biochemist
Re: Rate Law
« Reply #1 on: April 27, 2008, 01:27:04 PM »
That's not right.  What is the differential rate law that you're starting with?
Logged

Offline TEA1

  • Regular Member
  • ***
  • Posts: 16
  • Mole Snacks: +0/-1
Re: Rate Law
« Reply #2 on: April 27, 2008, 01:35:45 PM »
Basically I have to derive a formulat that indicates the linear dependence of concentration as a function of time for the reaction
A → B that has a reaction order of -1 in A.

I used-
Rate = k[A]-1 (-1 is exponent)

Rate = -d[A]/dt
Logged

Offline Yggdrasil

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 3215
  • Mole Snacks: +485/-21
  • Gender: Male
  • Physical Biochemist
Re: Rate Law
« Reply #3 on: April 27, 2008, 01:50:52 PM »
That equation is correct, but when I solve that differential equation, I don't get a linear relation between [A] and t.
Logged
Pages: [1]   Go Up
« previous next »
Sponsored Links