|
|
|
|
||||
|
Welcome to the GoFuckYourself.com - Adult Webmaster Forum forums. You are currently viewing our boards as a guest which gives you limited access to view most discussions and access our other features. By joining our free community you will have access to post topics, communicate privately with other members (PM), respond to polls, upload content and access many other special features. Registration is fast, simple and absolutely free so please, join our community today! If you have any problems with the registration process or your account login, please contact us. |
 |
|
|||||||
| Discuss what's fucking going on, and which programs are best and worst. One-time "program" announcements from "established" webmasters are allowed. |
|
|
Thread Tools |
03-04-2004, 08:03 PM
|
#1 |
|
Confirmed User
Join Date: Jul 2003
Posts: 437
|
College chem.
I hate lab reports....
Im stumped on this question, what mathematical function might decribe the relationship between reaction rate and solution concentration... Any idea?  |
|
|
|
03-04-2004, 08:06 PM
|
#2 |
|
Confirmed User
Join Date: Aug 2002
Location: East Coast.
Posts: 2,251
|
Rate is Proportional to Concentration.
You need to also include a rate constant. Let me know specifially what you need. |
|
|
|
|
03-04-2004, 08:08 PM
|
#3 |
|
No commissions, no fees.
Industry Role:
Join Date: Apr 2003
Location: USA
Posts: 17,706
|
College Sucks!
|
|
|
|
|
03-04-2004, 09:07 PM
|
#4 |
|
Confirmed User
Join Date: Oct 2001
Posts: 3,545
|
Reaction Rate = K (rate constant) * [X]^x * [Y]^y
where [X] is the concetration of X raised to the power of x and [Y] is the concentration of Y raised to the power of y. The powers are determined experimentally and decide the order of the reaction. If x=1 and y=1, then the reaction is second order, which means that it depends on the concentrations of X+Y. Hope this helps. |
|
|
|
|
03-04-2004, 10:27 PM
|
#5 |
|
Confirmed User
Join Date: May 2002
Location: Seat 1A
Posts: 2,483
|
It's all about the molarity baby yeah!
Man I miss college. |
|
|
|
|
03-04-2004, 10:29 PM
|
#6 |
|
Confirmed User
Join Date: Feb 2004
Location: Canadian this !!!
Posts: 8,532
|
yup, college rocks
__________________
sig for sale. ICQ :338213644 |
|
|
|
|
03-04-2004, 10:33 PM
|
#7 |
|
I am cool
Join Date: Jul 2003
Posts: 14,494
|
Great..I have that next semester..I am dying with peacewise functions :-x
|
|
|
|
|
03-04-2004, 10:37 PM
|
#8 |
|
Confirmed User
Join Date: May 2002
Location: Seat 1A
Posts: 2,483
|
As I recall, it's a curve - the more reactants are used the more the reaction slows. There are also three ways to calculate reaction rates - at the beginning, a specified point in time, or average. There was some calculus required to get the tangential rate along the curve. There's also a temperature factor too but Lev's formula definately brings back memories.
Man this is coming back and it hurts. |
|
|
|
|
03-04-2004, 10:37 PM
|
#9 | |
|
Confirmed User
Join Date: Dec 2003
Posts: 2,181
|
Quote:
|
|
|
|
|
|
03-04-2004, 10:41 PM
|
#10 | |
|
Confirmed User
Join Date: Aug 2003
Location: Chicago
Posts: 568
|
Quote:
 |
|
|
|
|
|
03-04-2004, 10:44 PM
|
#11 |
|
Too lazy to set a custom title
Join Date: Jan 2004
Location: Bluffville
Posts: 6,253
|
I hate that subject!
|
|
|
|
