The balanced equation for combustion of acetone peroxide is;
2C9H18O6 + 21O2 "\\to" 18CO2 + 18H2O
Pressure generated the bottle
Given that;
PV = nRT, hence
P= "\\dfrac{nRT}{V}"
n = moles of acetone = "\\dfrac{mass}{molar mass of a gas} =" "\\dfrac{5g}{222.24g\/mol(dimer)}" = 0.0225mol
R = 0.08206L*atm*mol-1K-1
T = 555oC + 273K = 828K
P = "\\dfrac{0.0225mol x 0.08206Latmmol^-1K^-1 x 828K}{2.00L}" = 0.76423 atm
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