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This is a cool question. With all the talk about trillions of dollars, I have been thinking about this also. What volume of air in an equilateral cube, or other volume format.

1 atmosphere of pressure at room temperature. PV=nRT

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12y ago
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12y ago

There's a couple problems with this question:

There is no specific molecule for "air". It is a mixture of several different gases, the vast majority of which is Nitrogen (about 78%), along with Oxygen (about 21%), and several other trace elements.

Also, with any gas, the volume of space taken is equal to the volume of the container holding the gas. This means that any number of gas molecules can fill any amount of space.

However, since you're probably looking for a number instead of a cop-out science jargon answer, I'll just pretend we're working under STP: standard temperature (273 degrees Kelvin) and pressure (1 atmosphere).

Applying the ever-so-useful ideal gas equation, PV=nRT we calculate:

6.02x1023 molecules = 1 mole, therefore

1x1010 molecules = 1.66x10-14 moles

1 atm * x liters = 1.66x10-14 moles * 0.0821 * 273 K

x = 3.72x10-13 liters

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Q: How much space does one trillion molecules of air take up?
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