A 616.1 mL with 1.92 g of nitroglycerin (C3H5N3O9) at 441 °C into CO2 (g), H20 (g), N2 (g), and 02 (g). What is pressure? 4C3H5N3O9 (l) 12 CO2 (g) + 10 H2O (g) + 6 N2 (g) + O2 (g)

Answer 1

4C₃H₅N₃O₉(l) ==> 12CO₂(g) + 10H₂O(g) + 6N₂(g) + O₂(g) .. balanced equation

Use the ideal gas law: PV = nRT and solve for P (pressure)

moles of gas present = n = 12 + 10 + 6 + 1 = 29 mols

Volume = V = 616.1 ml x 1 L / 1000 ml = 0.6161 L

Temperature in Kelvin = T = 441ºC + 273 = 714K

Gas constant = R = 0.0821 Latm/Kmol

P = pressure = ?

P = nRT / V = (29)(0.0821)(714) / 0.6161

P = 2759 atm = 2760 atm (3 sig. figs.)