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A scuba diver ascends too quickly and develops the bends. A nitrogen bubble has formed in the patient's elbow. At a depth of 61 ft, where the pressure is 2.85 atm, the bubble had a volume of 0.019 mL. Assuming a constant temperature and number of moles of nitrogen in the bubble, what volume did the bubble increase to at the surface, where the pressure is 1.00 atm? bubble volume at surface: mL The scuba diver is placed into a hyperbaric oxygen chamber where the pressure is 3.62 atm. What is the volume of this same nitrogen bubble while the patient is in the hyperbaric chamber? bubble volume in chamber: mL

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Rachita129

Assuming that the nitrogen, which can and does dissolve in the blood, does not.

How much bigger did the bubble get at the surface?

  • Boyle's law can be used to calculate the pressure times the volume under one set of conditions equals the pressure times the volume under the other set of conditions
  • Assuming that the nitrogen does not dissolve in the blood, which it can and does.
  • To compute the volume under different circumstances, we shall set the value to equal p 1 v 1 over p 2 and not 2.70 atmospheres.
  • The pressure at 56 feet was 2.70 atmospheres, and the bubble's volume was 0.018 milliliters; at 1 atmosphere, it would have been 0.0486 milliliters.
  • This group of divers was subsequently placed in a hyperbaric oxygen room at 3.64 atmospheres.
  • The nitrogen bubble's volume will remain unchanged.
  • The volume of.018 milliliters is determined by the calculation of 2.70 atmospheres.
  • In this case, 3.64 atmospheres will equal 0.0134 milliliters when we divide that by the new volume or the new pressure.
  • This is assuming that the nitrogen doesn't dissolve into the blood under these extreme pressures, which it might.

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