Steven W. answered 08/29/16
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Hi Rachel!
It looks like we are meant to make a few assumptions in this problem:
1. The air in the submarine is an ideal gas
2. No molecules or moles of air escape the bubble after the submarine breaks
3. The temperature at the depth of the submarine stays constant during this process
If this is the case, then we can use the ideal gas law.
PV = nRT
where
n = number of moles of gas
R = ideal gas constant
T = temperature
P = pressure
V = volume
I always like to start, when using this law, what the constant quantities are, and gather them on one side of the equation. Given the assumptions stated above, during this process, the entire right side of this equation is constant. This means that the product of P and V will be constant during this process. This, the product of P and V at any point in the process equals the product of P and V at any other point. We can write this mathematically as:
P1V1 = P2V2
So, as long as we use the same units for P and V in each case, we can relate P times V at one point in the process to P times V at any other point. So, before the submarine breaks, we have:
P1V1 = (1.2 atm)(15,000 L)
Then, after the submarine has broken, we have:
P2V2 = (250 atm)V2
with V2 being the volume of the resulting air bubble that we are trying to solve for. Then we can use:
P1V1 = P2V2 --> (1.2 atm)(15,000 L) = (250 atm)(V2)
This can be solved for V2 in liters.
Now, due to buoyancy and other factors, this bubble would not last long as is. It would float up, be subject to reduced pressure, expand, have shearing forces act on it, experience changes in temperature, and all sorts of things. But we would need much more information to deal with that. I think this idealized picture of what happens right after the submarine breaks is what they are looking for.
I hope this helps! Let me know if you have other questions about this or similar topics.