Here's an ideal gas law question: 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?