# Propane and Oxygen Combustion Question

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Problem: We desire to learn how much oxygen is needed to completely consume a certain quantity of propane gas.

Our hydrocarbon and oxygen combustion question follows the basic reaction path,

C3H8 + 5 O2 → 4 H2O + 3 CO2

If we have the following conditions:

• Temperature = 75 Celsius (348 Kelvin)
• Pressure = 720 / 760 mm = 0.95 atm
• Moles propane = 40.8 grams / 44.1 grams molecular weight = 0.93 moles
• ## How Much Oxygen to Burn the Propane?

What volume of oxygen is needed to accomplish the burning of the 0.93 moles of the hydrocarbon?

5 times 0.93 moles of C3H8 burned = 4.65 moles of oxygen

PV = nRT

where P= the pressure, V= the volume, and n= the number of moles and T is temperature in degrees Kelvin.

I calculate:

0.95 atm (V liters) = 4.65 (0.082 liter-atmospheres per mole per degree Kelvin) (348 degrees Kelvin)

V = 4.65 (348) / 0.95 = 1700

The answer is: To burn the hydrocarbon, 1700 liters of oxygen gas is needed.

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