Top Posters
Since Sunday
7
6
o
5
b
4
s
3
j
3
b
3
m
3
K
3
g
3
L
3
w
3
New Topic  
adb005 adb005
wrote...
Posts: 103
Rep: 1 0
3 years ago
For the reaction: 2 N2O5(g) → 4 NO2(g) + O2(g) the rate law is:

= k[N2O5]

At 300 K, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2. At the time when N2O5 is being consumed at a rate of 1.2 × 10-4 M/s, what is the rate at which NO2 is being formed?

▸ 1.2 × 10-4 M/s

▸ 2.4 × 10-4 M/s

▸ 6.0 × 10-5 M/s

▸ 3.0 × 10-5 M/s

▸ 4.8 × 10-4 M/s
Textbook 
General Chemistry: Principles and Modern Applications

General Chemistry: Principles and Modern Applications


Edition: 11th
Authors:
Read 131 times
3 Replies
Replies
Answer verified by a subject expert
dravid11dravid11
wrote...
Posts: 75
Rep: 0 0
3 years ago
Sign in or Sign up in seconds to unlock everything for free
More solutions for this book are available here
This verified answer contains over 220 words.
1

Related Topics

Anonymous
wrote...
A month ago
Help! The answer is missing an explanation...
wrote...
A month ago
More details provided!
New Topic      
Explore
Post your homework questions and get free online help from our incredible volunteers
  1046 People Browsing
Related Images
  
 381
  
 85
  
 690
Your Opinion
Which industry do you think artificial intelligence (AI) will impact the most?
Votes: 405