An air bubble of 32 cu. cm. volume is at the bottom of a lake 10 m deep where the temperature is 5C. The bubble rises to the surface where the temperature is 20C. What is the volume of the bubble just before it reaches the surface?
I know it can't be Charles' Law because pressure doesn't remain constant. I thought it may have been the Ideal Gas Law, but I don't know what to use for pressure.
Any insight to help me along? Thanks!
2006-12-07 11:37:08 · 3 answers · asked by alonso_fan85 1 in Science & Mathematics ➔ Physics
I don't think it would be Boyle's because 1.) temperature doesn't remain constant and 2.) I don't know what the value for pressure would be. I could be wrong though.
2006-12-07 11:47:53 · update #1
Use the ideal gas law after you have calculated the pressures. The pressure at the surface is atmospheric pressure, at 10 meters deep it is atmoshperic plus 5m*9810newtons/meter cubed (or atmos. plus 5m * 1000kg/m3 * 9.81 m/s2
2006-12-07 11:46:16 · answer #1 · answered by Cardinal Rule 3 · 0⤊ 0⤋
PV=nRT
T is in Kelvin. V is in litres.
You have to use the correct units for pressure. I assume atmosphere.
The pressure in water is a function of height. P = density * height, in Pascals (kg/m^2). Don't forget to add one atmosphere of pressure each time (for the barometric pressure).
1 atm = 101325 Pa. Density of water = 1000 kg/m^3.
2006-12-07 11:56:33 · answer #2 · answered by daedgewood 4 · 0⤊ 0⤋
It could be Boyle's!?
2006-12-07 11:44:49 · answer #3 · answered by Golden Ivy 7 · 0⤊ 0⤋