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The Bends. If deep-sea divers rise to the surface too quickly, nitrogen bubbles in their blood can expand and prove fatal. This phenomenon is known as the bends. If a scuba diver rises quickly from a depth of 25 m in Lake Michigan (which is fresh water), what will be the volume at the surface of an N2 bubble that occupied 1.0 mm3 in his blood at the lower depth? Does it seem that this difference is large enough to be a problem? (Assume that the pressure difference is due to only the changing water pressure, not to any temperature difference. This assumption is reasonable, since we are warm-blooded creatures.)

Short Answer

Expert verified

The volume of the bubble change from 1 mm3 to 3.4 mm3.

This is a large change in volume and would have a serious effect on the body of the divers.

Step by step solution

01

Step 1

The pressure at the bottom of the lake differs than the pressure at the top surface. So let's consider the pressure at the bottom p1 and at the top be p2. We would employ a relation betweenp1,V1,p2andV2

p1,V1,p2andV2

We were given the value of V1 but we want to calculate p1 and p2.

For p2, it is the same atmospheric pressure at the surface of the earth and equals 1.013 x 105 Pa.

For p1, there is a change in the pressure due to the depth of the lake h and the pressure increased as the drivers diving more depth so this change can be employed by:

p=ρgh

where ρ is the density of water, g is the gravity of acceleration and h is the lake depth.

p1=p2+ρgh=1.013×105Pa+1000kg/m3×9.8m/s2×25m=3.463×105Pa

02

Step 2

After calculating the pressure at the bottom of the lake p1 and at the surface p2 substitute with all the values of p1, p2 and given value of the volume of the bubble at the bottom of the lake v1 and solve for v2 to find the volume of the nitrogen bubble at the surface of the lake where

V2=p1V1p2=3.463×105Pa×1mm31.013×105Pa=3.4mm3

The volume of the bubble change from 1 mm3 to 3.4 mm3 and this is a large change in volume and would have a serious effect on the body of the divers.

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