Answer to Question #275523 in Organic Chemistry for HERO109

Question

Acetone peroxide, C₉H₁₈O₆(s), is a powerful but highly unstable explosive that does not contain nitrogen. It can pass undetected through scanners designed to detect the presence of nitrogen in explosives like TNT (trinitrotoluene, C₇H₅N₃O₆) or ammonium nitrate. Write a balanced equation for the combustion (burning in oxygen) of acetone peroxide producing steam and carbon dioxide. What pressure is generated in a 2.00-L bottle when 4.00 g of acetone peroxide is ignited to 555°C and burned in air? Assume 100% combustion.

Answer 1

The balanced equation for combustion of acetone peroxide is;

2C9H18O6 + 21O2 → 18CO2 + 18H2O

Pressure generated the bottle

Given that;

PV = nRT, hence

$P= \dfrac{nRT}{V}$

n = moles of acetone =$\frac{5g}{222.24g/mol(dimer)}$ =0.0225mol

R = 0.08206L*atm*mol-1K-1

T = 555oC + 273K = 828K

$\frac{0.0225molx0.08206Latmmol − 1K − 1x828K }{2L}$

= 0.76423 atm