Question

e volume of gas produced? 4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) A 1.000 kg sample of nitroglycerine, C3H5N3O9, explodes and releases gases with a temperature of 1985°C at 1.100 atm. What is the volume of gas produced? 4 C3H5N3O9(s) → 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) 4730 L 5378 L 3525 L 742.2 L

Answer 1

Answer:

742.2 L

Explanation:

First we must find the number of moles of nitroglycerine reacted.

Molar mass of nitroglycerine= 227.0865 g/mol

Mass of nitroglycerine involved = 1×10^3 g

Number of moles of nitroglycerine= 1×10^3g/227.0865 g/mol

n= 4.40361 moles

T= 1985°C + 273= 2258K

P= 1.100atm

R= 0.082atmLmol-1K-1

Using the ideal gas equation:

PV= nRT

V= nRT/P

V= 4.40361× 0.082× 2258/1.1

V= 742 L