Top Posters
Since Sunday
y
2
m
2
m
2
u
2
m
2
B
2
M
2
e
2
k
2
N
2
y
2
m
2
Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
New Topic  
dacia79 dacia79
wrote...
Go to Answer
Posts: 22
Rep: 0 0
10 years ago
The rate constant for the reaction is 0.540 M–1·s–1 at 200 °C.

If the initial concentration of A is 0.00250 M, what will be the concentration after 965 s?

I know that you have to use the integrated rate equation, but I don't understand the meaning behind the equation.  I also can't determine the reaction order.  Please help.  Thank you. 
Read 701 times
3 Replies
Replies
wrote...
#1
Staff Member
Educator
10 years ago
HI

Here's a similar question, hope it helps

Question
The rate constant for the reaction is 0.540 M–1·s–1 at 200 °C.

A--> products

If the initial concentration of A is 0.00640 M, what will be the concentration after 835 s?

Answer
The units of k tell you that this is a second order reaction. So, to solve this, you need to use the integrated rate law for a 2nd order reaction:

1/[A] = kt + 1/[A]o
1/[A] = 0.540/Ms (835 s) + 1/0.00640
1/[A] = 607
[A] = 1.65X10^-3 M
Mastering in Nutritional Biology
Tralalalala Slight Smile
dacia79 Author
wrote...
#2
10 years ago
Thank you but how did you get from 607 to 1.65 x 10^-3? 
Answer accepted by topic starter
padrepadre
wrote...
#3
Staff Member
Educator
Top Poster
Posts: 21611
Rep: 4541 17
10 years ago
Sign in or Sign up in seconds to unlock everything for free
1
Mastering in Nutritional Biology
Tralalalala Slight Smile

Related Topics
New Topic      
Quick Reply
Explore
Post your homework questions and get free online help from our incredible volunteers
  499 People Browsing
Start New Topic Take the Tour CoursesNew Study Tools Topics Trending Browse by Textbook
Live Chat
Related Images
  
 1289
  
 834
  
 444
Your Opinion
Where do you get your textbooks?
Votes: 447
Previous poll results: Does a gender wage gap exist in America?