Write a balanced chemical equation, including physical state symbols, for the decomposition of liquid nitroglycerin () into gaseous dinitrogen, gaseous dioxygen, gaseous water and gaseous carbon dioxide. 2. Suppose of carbon dioxide gas are produced by this reaction, at a temperature of and pressure of exactly . Calculate the mass of nitroglycerin that must have reacted. Round your answer to significant digits.

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

Balanced reaction equation:

4C3H5N3O9 > 12CO2 + 10H2O + 6N2 + O2

Mass of nitroglycerine= 838g of nitroglycerine

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

am i too late?

explanation: