Question

why is it important for a deep sea diver to ensure the pressure of the gas in the lungs is the same as the surrounding water in both ascent an descent ?

How does the diver accomplish this?

Answer #1

Hydrostatic pressure matters here. In the deep sea, the more water above diver and greater the weight of water. In this situation, the weight affects diver from all sides in same amount and incrases pressure per foot of seawater. At a depth about 10.1 m, the magnitude of hydrostatic pressure and atmospheric pressure is same.

At greater depths, the beating gas become heavier as its density increases. In this case, the diver should perform

greate efforts to breath. This limits the abiility of diver to ventilate the lungs adequately,

A scuba diver is at a depth of 385 m, where the pressure is 39.5
atm. What should be the mole fraction of O2 in the gas mixture the
diver breathes in order to have the same partial pressure of oxygen
in his lungs as he would at sea level? Note that the mole fraction
of oxygen at sea level is 0.209.

A scuba diver at a depth of 41.0 m below the surface of the sea
off the shores of Panama City, where the temperature is
5.00C, releases an air bubble with volume 19.0
cm3. The bubble rises to the surface where the
temperature is 23.00C. What is the volume of the bubble
immediately before it breaks the surface? The specific gravity for
seawater is 1.025.
(Hint: Remember that both pressure and temperature
change. Also, don't forget that the diver is...

4. The diver in Problem 2, while underwater at a depth of 20.0
m, breathes from the tank so that the air entering the diver’s
lungs is at the same pressure as that of the surrounding water. If
each breath fills the diver’s lungs to a volume of 3.70 L, and the
air he breathes warms to a temperature of 30.0OC, how many breaths
can the diver take before the air remaining in the tank drops to a
pressure of...

The solubility of N2 in
blood at 37°C and at a partial pressure of 0.80
atm is5.6 × 10−4 mol/L. A deep-sea
diver breathes compressed air with the partial pressure of
N2 equal to 5.0 atm. Assume that the
total volume of blood in the body is 5.2 L. Calculate the amount of
N2 gas released (in liters at
37°C and 1.00 atm) when the diver returns to the
surface of the water, where the partial pressure of
N2 is...

The solubility of N2 in blood at 37°C and at a partial pressure
of 0.80 atm is 5.6 × 10−4 mol/L. A deep-sea diver breathes
compressed air with the partial pressure of N2 equal to 4.5 atm.
Assume that the total volume of blood in the body is 5.2 L.
Calculate the amount of N2 gas released (in liters at 37°C and 1.00
atm) when the diver returns to the surface of the water, where the
partial pressure of N2...

A diver on Earth
(where the atmospheric pressure is 1.00 atm and the acceleration
due to gravity is 9.80 ms-2) descends in salty sea water
with a density of 1026 kgm-3. The diver is holding a
balloon close to him and the volume of the balloon is V at the
surface of water is 3.76 × 10-3 m3.
What pressure does the
diver experience at a depth of 19.4 m?
Answer atm
Question 15
Not complete
Marked out of 1.00...

How does the pressure exerted by a liquid change with the
depth of the liquid?
How does the pressure exerted by a liquid change as the
density of the liquid changes?
Discounting the pressure of the atmosphere, if you swim
twice as deep in water, how much more water pressure is exerted on
your ears?
In a deep dive, a whale is appreciably compressed by the
pressure of the surrounding water. What happens to the whale’s
density?
If water faucets...

When scuba diving, it is important to come back to the surface
of the water from deep dives slowly. If this does not happen, then
the diver can get the "bends."
a.) Using Henry's law constants, determine the moles of N2 and
O2 dissolved in 7.5 L of blood (assume it is water) at 298 K at the
surface of the water before the dive and again at a depth of 100.0
ft below the surface.
b.) If the diver...

1. scuba diver 40 ft below the ocean surface inhales 45.0 mL of
compressed air from a scuba tank at a pressure of 2.90 atm and a
temperature of 8 ∘ C . What is the final pressure of the air, in
atmospheres, in the lungs when the gas expands to 145.0 mL at a
body temperature of 37 ∘ C , and the amount of gas does not
change?
2. Consider 4.70 L of a gas at 365 mmHg...

Why is equity an important framework in program implementation
and how does an equity framework ensure population inclusion
impact? Please support your claims with one to two current
professional, published.

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