Answer:
Total pressure is 1189 atm
Explanation:
This is the reaction:
4C₃H₅(NO₃)₃ → 6N₂ + O₂ + 12CO₂ + 10H₂O
As we have the volume of TNT, we must know the density to find out the mass and then, apply molar mass to calculate mole.
TNT density = 1.654 g/mL
Density = mass / volume
1.654 g/mL = TNT mass / 50mL
1.654 g/mL . 50mL = TNT mass → 82.7 g
Mass / Molar mass = Mol → 82.7 g / 227.1 g/m = 0.364 mole
Now, we can calculate all the mole for the formed gases.
4 mole of TNT produce 6 mole N₂ ___ 1 mol O₂ __ 12 mole dioxide __ 10 mole of water
0.364 mole of TNT will produce:
- (0.364 . 6) /4 = 0.546 mole of produced nitrogen
- (0.364 . 1) /4 = 0.091 mole of produced oxygen
- (0.364 . 12) /4 = 1.092 mole of produced dioxide
- (0.364 . 10) /4 = 0.91 mole of produced vapour of water.
Total mole = 0.564 + 0.091 + 1.092 + 0.91 = 2.657 mole
Let's apply the Ideal Gases Law to find the total pressure, at STP
In STP, pressure is 1 atm for 1 mole at 273K, in a volume of 22.4 mL
But we have a volume of 50mL, and we have 2.657 total mole
Don't forget to convert 50 mL to L, cause the units for R
50 mL = 0.050L
P . 0.050L = 2.657 mol . 0.082L.atm/mol.K . 273K
P = (2.657 mol . 0.082L.atm/mol.K . 273K) / 0.050L
P = 1189 atm
