Problem 15.11 A diver observes a bubble of air rising from the bottom of a lake

Question

Problem 15.11

A diver observes a bubble of air rising from the bottom of a lake (where the absolute pressure is 3.40 atm ) to the surface (where the pressure is 1.00 atm). The temperature at the bottom is 4.0 C and the temperature at the surface is 23.0 C.

Part A

What is the ratio of the volume of the bubble as it reaches the surface to its volume at the bottom?

Part B

Would it be safe for the diver to hold his breath while ascending from the bottom of the lake to the surface? Why or why not?

A. There would be no change in volume in the lungs so it would not be dangerous. B. This increase in the pressure of the air in the lungs would be dangerous. C. This decrease in the volume of air in the lungs would be dangerous. D. This increase in volume of air in the lungs would be dangerous.

Explanation / Answer

gas equation

PV=nRT

we use it for surafec and bottom bcause we want to find ratio of volume

Since temperatures are not same, we can solve for temperature, then equate the two equations.
so Pbottom*Vbottom=nRT

Vbottom=nRTbottom/Pbottom

Vtop=(nRTtop)/Ptop

Vtop/Vbottom ={(nRTtop)/Ptop} / {(nRTbottom)/Pbottom)}

Vtop/Vbottom =( Ttop*Pbottom )/ (Ptop* Tbottom)

Pbottom=absolute+surface=1+3.4=4.4atm

Ptop=1atm

Vtop/Vbottom= 296K*4.4atm /277K*1atm=4.7018

part b

Free diving is when you are going down from the surface and then coming back up. In that case, the volume of the air that you start with at the surface is safe for your lungs to hold and won't hurt them when you are ascending.

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---