ScubaInChicago
Contributor
Will you lay off the gotchas? Of course we add "a volume" of air. Any amount of gas takes up a volume. Now, let me try once more before giving up on you and assume that you're just trolling:
Imagine you're diving a DS. You're on the surface. Your undergarments are comfortably lofted, but you don't have excessive air in your suit. The volume of that air is V.
Now descend to 10m/33ft without adding air to the suit. P has doubled, so V is half of what it was on the surface. Boyle's law.
You're uncomfortably squeezed, cold as Hel and you have problems reaching your chest inflator because you're shrink-wrapped in your trilam suit. All because V is now reduced to V/2. It's not constant any more. Boyle's law.
You manage to reach the inflator, and you add air to your suit. That air of course has a volume. So yes, you add "a volume of gas" to your DS. You add just enough to increase the volume of air inside your suit back to V.
Your undergarments are comfortably lofted, but you don't have excessive air in your suit. V on the surface, V at 10m/33ft. Constant volume. But the amount of air molecules taking up V is now the double. Double pressure, double the amount of air, constant volume. PV=nRT. Ideal gas law.
I'll leave it up to the student to work out what happens on ascent. Hint: To avoid a runaway ascent you want constant buoyancy. Since your weight is practically constant, what do you want your volume to be? The same, i.e. constant. Constant volume.
So if we need a volume of .25 cf of gas to be comfortable at the surface, we would need a volume equal to .5 cf @ 2 ATAs, and .75 cf @ 3 ATAs. That in no way shape or form sounds like a constant volume when we're adding additional volume on decent. PV=nRT sounds great in a closed system which a drysuit is not.