CaptainOfSmug
Harmless
Posts: 36
Registered: 3-5-2012
Location: In the Nightside Eclipse
Member Is Offline
Mood: No Mood
|
|
Gas Generating Problems
Okay, I know it says this forum isn't a text book substitute, but my professor hasn't gotten back to me and some of these problems are driving me
bonkers...
So, for example:
Magnesium nitride decomposes in water and releases ammonia gas. If 335 mL of ammonia is produced at STP, what is the mass of magnesium nitride that
reacted?
I know how to solve these problems I think by using PV=nRT and I'm solving for n in this case I believe. However, whats throwing me off is the STP
part. Do I need to find the partial pressure of ammonia gas first and convert it to atmospheres? I know the rate is 0.0821 but would the temperature
just be 273K? I have a hard time believing the gas is generated at room temperature...
Thanks in advance for the help! And I hope this goes without saying but please don't just give me the answer, I want to actually be able to solve
these and a nudge in the right direction would help me greatly!
[Edited on 15-3-2013 by CaptainOfSmug]
|
|
|
DraconicAcid
International Hazard
Posts: 4334
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
STP is standard temperature and pressure. It doesn't matter what temperature the gas was generated at, it's heated or cooled (and expanded or
pressurized) until it's at STP and the volume is measured.
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.
|
|
|
MrHomeScientist
International Hazard
Posts: 1806
Registered: 24-10-2010
Location: Flerovium
Member Is Offline
Mood: No Mood
|
|
The way I would go about it is first determine n from the gas law, as you said. Then, find the equation for magnesium nitride's reaction with water.
You can use that and the results from the first step to get to your answer. Good luck!
And kudos for not asking for spoonfeeding! There seems to be quite a bit of that lately. That might get you your answer short term, but you won't get
far if you don't actually understand where the answer came from. The best way to understand is to do it yourself!
|
|
|
CaptainOfSmug
Harmless
Posts: 36
Registered: 3-5-2012
Location: In the Nightside Eclipse
Member Is Offline
Mood: No Mood
|
|
Okay thanks much! So I figured the equation is Mg3N2 + 6H2O --> Mg(OH)2 + 2NH3
So, would my equation essentially be (1)(.335)=n(0.0821)(273) so n =0.015 moles of NH3?
So the mass would then be 0.757g of magnesium nitride?
This seems logical to me and makes sense but just double checking. Thanks again for the help!
|
|
|
MrHomeScientist
International Hazard
Posts: 1806
Registered: 24-10-2010
Location: Flerovium
Member Is Offline
Mood: No Mood
|
|
Looks correct to me! It looks like you accounted for it in the math, but forgot to include the coefficient of 3 on the Mg(OH)2 in your post.
|
|
|
DraconicAcid
International Hazard
Posts: 4334
Registered: 1-2-2013
Location: The tiniest college campus ever....
Member Is Offline
Mood: Semi-victorious.
|
|
Quote: Originally posted by MrHomeScientist  | | Looks correct to me! It looks like you accounted for it in the math, but forgot to include the coefficient of 3 on the Mg(OH)2 in your post.
|
Doesn't matter- you only use the NH3/Mg3N2 coefficient in the calculation.
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.
|
|
|
MrHomeScientist
International Hazard
Posts: 1806
Registered: 24-10-2010
Location: Flerovium
Member Is Offline
Mood: No Mood
|
|
Ah, well... of course 
Just making sure the full equation was correct!
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
