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ChemistryChemistry
16 August, 07:19

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) 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

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  1. 16 August, 08:15
    0
    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
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Home » Chemistry » 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) A 1.
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