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

Question

Everett Goodwin

Chemistry

23 February, 15:39

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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Answers (1)

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Moran · Answer 1

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