Ideal Gas Law Question: Solving for Volume at Surface

[Borat321]

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?

 

[ponjavic]

seems right, what's the correct answer?

 

[Kurdt]

Should be fine, all you have to do is rearrange the final equation you wrote for the second volume and plug the numbers in.