Volume of Bubble: Solve for V2 at Depth of 30 m

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A bubble with an initial volume of 1.00 cm³ at a depth of 30 m in a lake, where the temperature is 20°C, rises to the surface where the temperature increases to 35°C. The pressure at the bottom is calculated to be 3.943 atm, while at the surface it is 1 atm. Using the ideal gas law and the correct absolute temperatures, the volume of the bubble just before it breaks the surface is determined to be approximately 4.14 cm³. The initial calculation error was due to using Celsius instead of absolute temperature. The final volume reflects the changes in pressure and temperature as the bubble ascends.
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Homework Statement



A bubble with a volume of 1.00 cm3 forms at the bottom of a lake that is 30 m deep. The temperature at the bottom of the lake is 20°C. The bubble rises to the surface where the water temperature is 35°C. Assume that the bubble is small enough that its temperature always matches that of its surroundings. What is the volume of the bubble just before it breaks the surface of the water? Ignore surface tension.

Homework Equations



PV=nRT

P1V1/T1 = P2V2/T2

The Attempt at a Solution



P2 = 1atm
P1 = 1 atm + 1000 * 9.81 * 30 => 3.943atm

3.943atm*1cm3/20C = 1atm*V2/35C
V2=6.9cm3

This value for V2 is way too big, where did I screw up? Thanks
 
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You've used celcius instead of absolute temperature.
 
ahh

so,

3.943/293 = V2/308
V2=4.1448cm3?
 
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