The question is incomplete, the complete question is:
Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin (C_3H_5(NO_3)_3) into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. Suppose 81.0 L of carbon dioxide gas are produced by this reaction, at a temperature of - 5.0 degree C and pressure of exactly 1 atm. Calculate the mass of nitroglycerin that must have reacted. Be sure your answer has the correct number of significant digits. g
Answer:
Balanced reaction equation:
4C3H5N3O9 ---------> 12CO2 + 10H2O + 6N2 + O2
Mass of nitroglycerine= 838g of nitroglycerine
Step-by-step explanation:
Now, given the parameters we have in the question:
Volume of carbon dioxide V= 81.0 L
Temperature T= -5°C +273= 268K
Pressure= 1 atm
R=0.082 atmLmol-1K-1
Number of moles of nitroglycerine= n
From PV= nRT
n= PV/RT
n= 1×81.0/0.082×268
n= 3.69 moles
To obtain the mass of nitroglycerine reacted:
Number of moles of nitroglycerine × molar mass of nitroglycerine
Mass of nitroglycerine= 3.69moles × 227.0865 g/mol
Mass of nitroglycerine= 838g of nitroglycerine