• We’re currently investigating an issue related to the forum theme and styling that is impacting page layout and visual formatting. The problem has been identified, and we are actively working on a resolution. There is no impact to user data or functionality, this is strictly a front-end display issue. We’ll post an update once the fix has been deployed. Thanks for your patience while we get this sorted.

Did I do this gas temperature chem volume problem correctly?

T

Techie333

Platinum Member
Ammonium nitrate can decompose explosively when heated according to the equation
2NH4NO3(s) ---> 2N2(g) + 4H2O(g) + O2(g)
How many liters of gas would be formed at 552°C and 1.00 atm pressure by explosion of 239 g of NH4NO3?

So, the mol mass of NH4NO3 is 80g so 239/80 = 2.9875mol. 552C = 825K so now n1t1 = n2t2 so, (2.9875g) x (273 K) = (X) x (825 K). X = .98859mol and then u mutliply by 22.4 and get 22.144 L gas!??!?
 
methinks wrong, i'm not shure whaqt you did, but

239g * (1 mol solid/80g) * (1 mol reaction/2 mol solig) * ( 7 mol final gas/ 1 mol reaction) = 10.456 mol gas
use pv=nrt v=nrt/p = (10.456*8.314*825)/1atm=69111 L (check to see if this is the right R value for atm, it's been a while)
 
You must log in or register to reply here.

TRENDING THREADS

Back
Top