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:
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
The ideal gas law reads:
PV = nRT
where P= the pressure, V= the volume, and n= the number of moles and T is temperature in degrees Kelvin.
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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