Question

A 1.000 kg sample of an organic compound, C₃H₅N₃O₉, explodes and releases gases with a temperature of 1985°C at 836.0 atm. What is the volume of gas produced? (always balance equations) C₃H₅N₃O₉(s) → CO₂(g) + H₂O(g) + N₂(g) + O₂(g)

The listed answers are: 5378 L, 742.2 L, 3525 L, 4730 L, 352.5 L

My answer:
We have:
1.000 kg --> 1.000x10^3 g =1,000 g C3H5N3O9
T= 1985C --> 1985C+273= 2258K
P= 836.0 atm
V=?

Balanced equation: 4C₃H₅N₃O₉-->12CO₂+10H₂O+6N₂+O₂

C= 3*12.0107 = 36.0321g
H= 5*1.00794 = 5.0397g
N= 3*14.00674 = 42.02022g
O= 9*15.9994 = 143.9946g

C₃H₅N₃O₉ = 227.08662 g/mol

1,000g*(1 mol/277.08662g) = 4.404 mol C₃H₅N₃O₉

CO₂:
4.404 C₃H₅N₃O₉ * 12 mol CO₂/4 mol C₃H₅N₃O₉ = 13.212 mol CO₂
H₂O:
4.404 C₃H₅N₃O₉ * 10 mol H₂O/4 mol C₃H₅N₃O₉ = 11.01 mol H₂O
N₂:
4.404 C₃H₅N₃O₉ * 6 mol N₂/4 mol C₃H₅N₃O₉ = 6.606 mol N₂
O₂:
4.404 C₃H₅N₃O₉ * 1 mol O₂/4 mol C₃H₅N₃O₉ = 1.101 mol O₂

Sum of mol of gasses: 13.212+11.01+6.606+1.101= 31.929 mol gasses

Ideal gas law: PV=nRT; to find V=nRT/P

V=[31.929 mol * 0.082058 (L*atm/K*mol) * 2258K]/ 836.0 atm
V= 7.077 L obviously isn't one of my possible answer choices, am I doing something wrong?

Answer 1

Mass & org. comod - lio kg. a Molar mass of Eats N30g = 3x12.0107 + 5*1.00794 + 3x 14.00574 + gx 15.gggu = 227.08562 gl mole For the reacth 4 CzHs N309 (5) ZER +10H2O +6N2 & O2 HO. O moles Cz Hs N30g = 10ong ZR9.00662 = 4.403505 mole as per reaction no. of moles If cos torooduced 12x 4.403606 13.210819 mole ho. I moles of Hoo Produod = 10 x 4.403506 = 13og mole no. of moles of Na brothyced 5 X 4. 403505 = 5.60541 mole no. of moles # 02 too cluesd x 4.403506 = 100g 015 mole Total no. of moles gas produced = 13. R10819 + 11.00 +6.60SU1 + 1.1009015 - 31.9261295 mole ne 31.92613 mole PV = nRT R = 0.08 Rosa Liat mk. mole TE 1985 +23:15 = 2259.15 R P= 335.0 beth

For ideal gas Pu= MRT NRT V= P = 0 31.92613 *0.0820GX Z258.15 835 - 7.0755 L vol. f gas produced = 7:0768 7:07.72 Ans
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