Determine the total pressure of all gases (at stp) formed when 50.0 ml of tnt (c3h5(no3)3, , molar mass = 227.10 g/mol) reacts according to the following reaction. 4 c3h5(no3)3(l) → 6 n2(g) + o2(g) + 12 co2(g) + 10 h2o(g)

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

the answer is   c.) 1575 j.

explanation:

air

in a tire you fill a tire with air

then a couple days later you check the air pressure in the tire

hope this mark me brainliest