# Ideal Gas Question

1. Aug 4, 2009

### Perrin

1. The problem statement, all variables and given/known data

An air bubble of volume 1cm^3 is located at a depth of 50m beneath the surface where the temperature is 17C. When the bubble goes up to the surface where the temperature is 27C, how much will its volume be? Take the atmospheric pressure to be 1atm. Assume the pressure increases 1atm for every 10 meters.

2. Relevant equations

Ideal Gas Law:
pV=nRT

3. The attempt at a solution

$$p_{1}v_{1}/T_{1}=p_{2}v_{2}/T_{2}$$

I plugged in:

$$5\times10^{5}\times1\times10^{-6}/290=1\times10^{5}\times V_{2}/300$$

Solving for V2, I get 5.2cm^3, but according to the solutions, that's not the answer...
I'd like to know what I'm doing wrong.
Thanks for the help!

Last edited: Aug 4, 2009
2. Aug 4, 2009

### ideasrule

At 50 m, the pressure due to the water is 5 atm. You still have to add in the atmospheric pressure.

Last edited: Aug 4, 2009