November 01, 2024, 12:36:44 PM
Forum Rules: Read This Before Posting


Topic: Kinetics! 1st order vs second order irregularity  (Read 3009 times)

0 Members and 1 Guest are viewing this topic.

Offline Shadow

  • Full Member
  • ****
  • Posts: 227
  • Mole Snacks: +5/-11
Kinetics! 1st order vs second order irregularity
« on: December 08, 2014, 12:27:08 PM »
Why is the concentration drop for a first order reaction bigger than for a second order reaction?

Offline Babcock_Hall

  • Chemist
  • Sr. Member
  • *
  • Posts: 5688
  • Mole Snacks: +329/-24
Re: Kinetics! 1st order vs second order irregularity
« Reply #1 on: December 08, 2014, 12:35:13 PM »
The general forum rule is that you must show an attempt before anyone can help you.  However, in this case, you might start by rephrasing this question.  What do you mean by concentration drop?  Over what time period?

Offline Shadow

  • Full Member
  • ****
  • Posts: 227
  • Mole Snacks: +5/-11
Re: Kinetics! 1st order vs second order irregularity
« Reply #2 on: December 08, 2014, 02:39:39 PM »
Over the whole course of  a reaction.

Offline Babcock_Hall

  • Chemist
  • Sr. Member
  • *
  • Posts: 5688
  • Mole Snacks: +329/-24
Re: Kinetics! 1st order vs second order irregularity
« Reply #3 on: December 08, 2014, 04:14:21 PM »
Over the whole course of a reaction, the reactant drops from its initial concentration to is equilibrium concentration, regardless of the order of the reaction.  I have to suspect that I don't yet understand your question.

Offline Shadow

  • Full Member
  • ****
  • Posts: 227
  • Mole Snacks: +5/-11

Offline Corribus

  • Chemist
  • Sr. Member
  • *
  • Posts: 3540
  • Mole Snacks: +542/-23
  • Gender: Male
  • A lover of spectroscopy and chocolate.
Re: Kinetics! 1st order vs second order irregularity
« Reply #5 on: December 09, 2014, 01:45:39 PM »
Compare the two reactions:

A :rarrow: P
A + A :rarrow: P

In the second order reaction, a collision is required between two A molecules in order for one product conversion to take place. As A is converted into P, there is less A in the reaction vessel, so the probability of a collision becomes lower and lower. The reaction rate is very slow as the concentration of A becomes vanishingly small. 

In the first order reaction, no collision is required. The probability per unit time of a successful conversion event still decreases as time elapses, because there is still less A in the reaction vessel at later times, but this drop in the reaction probability is not as severe as it is where a collision is required.

The amount of A left in the reaction vessel per unit time is inversely dependent on the reaction probability per unit time. This is why the concentration of A drops faster in the first order case than it does in the second order case.
What men are poets who can speak of Jupiter if he were like a man, but if he is an immense spinning sphere of methane and ammonia must be silent?  - Richard P. Feynman

Offline Shadow

  • Full Member
  • ****
  • Posts: 227
  • Mole Snacks: +5/-11
Re: Kinetics! 1st order vs second order irregularity
« Reply #6 on: December 09, 2014, 01:57:24 PM »
Thank you very much sir.

Sponsored Links