Combustion of carbon would give carbon dioxide: C + O_{2} → CO_{2}

The general plan would be to start with the mass of carbon, then calculate the moles of carbon, then use the mole ratio in the balanced equation to find the moles of carbon dioxide.

kg C → g C → mol C → mol CO_{2}

At this point it is necessary to know the pressure and temperature of the container that would hold the CO_{2}, which is a gas. If we assume that CO_{2} is an ideal gas under "STP conditions" (standard temperature and pressure; P = 1 atm and T = 273 K), then we can use the fact that one mole of an ideal gas at STP has a volume of 22. 4 liters, and the final conversion is

mol CO_{2} → Liters CO_{2}

Given the above plan, the calculation goes like this:

1 kg C x (1000 g C/1 kg C) x (1 mol C/12.01 g C) x (1 mol CO_{2}/1 mol C) x (22.4 L/1 mol CO_{2})

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The above solution gets you the volume of oxygen needed, but then you need to account for the fact that air is not 100% O2. So the total volume of air needed for complete combustion is greater than that value by the proportion of air that is not oxygen.