March 28, 2024, 12:30:30 PM
Forum Rules: Read This Before Posting


Topic: Chemical Kinetics rate of disappearance  (Read 20361 times)

0 Members and 1 Guest are viewing this topic.

Offline daylight

  • Regular Member
  • ***
  • Posts: 23
  • Mole Snacks: +0/-0
Chemical Kinetics rate of disappearance
« on: February 08, 2009, 03:27:01 PM »
I'm really not sure if I understand this, but here is the question.
The data in the following table is for the reacion, 2N2O5=4NO2 + O2
I have a chart of like time mol/l and secons, but I'll just use two as an example:
N2O5 (mol/L)  t (seconds)
0.0152             0
0.0113             10 

I'm not sure but is the formula  average rate= -:delta:(N2O5)/ :delta:t=-(N2O5)final - (N2O5)initial/tfinal-t initial 
so would I use that  to get the average rate of reaction for each set of data??
Thanks

Offline daylight

  • Regular Member
  • ***
  • Posts: 23
  • Mole Snacks: +0/-0
Re: Chemical Kinetics rate of disappearance
« Reply #1 on: February 08, 2009, 04:20:48 PM »
 I forgot to enter the actual probelm question and it won't let me edit for some reason...

Q: Write the equation for average rate of disappearance of dinitrogen pentoxide and calculate the average rate of reaction between each time interval.

Offline jotakabe

  • New Member
  • **
  • Posts: 3
  • Mole Snacks: +0/-0
Re: Chemical Kinetics rate of disappearance
« Reply #2 on: March 11, 2009, 08:21:29 PM »
The average rate is going to be delta [N2O5] / delta time.  Your rate should have units of M/s or mol/(L*s).  Since the reaction order is > 0, the average rate should be different between each data point.  Have fun!

Sponsored Links