25heat
Harmless
Posts: 6
Registered: 19-2-2014
Location: United States
Member Is Offline
Mood: No Mood
|
|
Rate constant and compound decomposition
Gaseous azomethane, CH3N=NCH3, decomposes in a first-order reaction when heated:
CH3N=NCH3(g) → N2(g) + C2H6(g)
The rate constant for this reaction at 600K is 0.0216 min-1. If the initial quantity of azomethane in the flask is 13.71 grams, how much remains after
3.00 minutes?
What quantity of nitrogen is formed in 3.00 minutes?
Ok so for the first part I simply used the equation for first order: (lnAf/lnAo)=-KT and got 12.85.
I know that is correct, but I am confused as how to find how much nitrogen is formed. I feel like it is simple but I cant figure it out. Please help!
|
|
|
DraconicAcid
International Hazard
Posts: 4334
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
I f you know how much azomethane reacted, then you can find out how much nitrogen was formed through stoich.
Please remember: "Filtrate" is not a verb.
Write up your lab reports the way your instructor wants them, not the way your ex-instructor wants them.
|
|
|
25heat
Harmless
Posts: 6
Registered: 19-2-2014
Location: United States
Member Is Offline
Mood: No Mood
|
|
Preciate it I knew it had to be simple
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
