Here's an ideal gas law question:(adsbygoogle = window.adsbygoogle || []).push({});

A scuba diver is 32 m below the surface of a lake, where the temperature is 5°C. He releases an air bubble with a volume of 12 cm^3. The bubble rises to the surface, where the temperature is 25°C. What is the volume of the bubble right before it breaks the surface? (Hint: Remember that the pressure also changes.)

I thought it would be the following:

Initial:

Pressure @ 32m = 4.2atm, since 10m=1atm under water

12cm^3=.012 litres

5C= 278K

Final:

Pressure @ 0m = 1atm

V= unknown

25C= 298K

Then, use PV/T=PV/T... but apparently it's wrong - does anyone know why?

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# Homework Help: Ideal gas question

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