100 Points + Brainliest. I need a thorough response to this assignment. Please do not answer without a correct, in depth and well written explanation! Thank you! :) If a diver inhales from their air tank on surface level, the pressure in their lungs will be at 1 atm. If they inhale air from their tank at a depth of 70 m (~230 ft), the pressure in their lungs will be 8 atm. (for every 10 meters below the water, pressure increases
by 1 atm). Assume the diver's lung volume is 1 L. If a diver at 70 m has 1 L of air at a pressure of 8 atm in her lungs and ascends to the surface (1 atm) while holding her breath, what happens to the diver’s lungs? (total lung capacity is 6.0 L)

Explain what is going on, in a molecular level inside the diver’s lungs, in terms of collisions, volume, and pressure.

If a diver inhales from their air tank on surface level, the pressure in their lungs will be at 1 atm. If they inhale air from their tank at a depth of 70 m (~230 ft), the pressure in their lungs will be 8 atm. (for every 10 meters below the water, pressure increases

by 1 atm). Assume the diver's lung volume is 1 L. If a diver at 70 m has 1 L of air at a pressure of 8 atm in her lungs and ascends to the surface (1 atm) while holding her breath, what happens to the diver’s lungs? (total lung capacity is 6.0 L)

Explain what is going on, in a molecular level inside the diver’s lungs, in terms of collisions, volume, and pressure.Dry air is composed of roughly 21% oxygen, 78% nitrogen, and 1% other gases. According to Dalton’s law the partial pressure of oxygen at any depth will be 21% of the total pressure exerted by the air and the partial pressure of nitrogen will be 78% of total pressure.

Gases dissolve in the liquid with which they are in contact. Nitrogen is fat soluble and at sea level we have several litres dissolved in our bodies. If the partial pressure of nitrogen is doubled (by breathing air at 10 m depth) for long enough for equilibration to take place we will contain twice as many dissolved nitrogen molecules as at sea level.

The effect of the increased partial pressures of oxygen is more complex. Doubling our inspired partial pressure of oxygen doubles the amount of oxygen in solution but does not double the amount of oxygen in the body since a large part of our oxygen content is bound to oxygen carrying pigments. The haemoglobin in arterial blood is virtually saturated at an inspired partial pressure of oxygen (Fio2) of 21 kPa, and increasing the partial pressure of oxygen has little effect on the amount of oxygen bound to haemoglobin.

Explanation: i hope this helps

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

8 m/s because for him to get the same amount of energy as ray is putting out, bobby, who weighs half as much as ray, needs to run twice as fast.