Complete Question
The complete question is shown on the first and second uploaded image
Answer:
a
Now the ratio of the gases in Gabor's lungs at the depth of 15m to that at
the surface is 
b
The number of moles of gas that must be released is
Explanation:
We are told from the question that the pressure at the surface is 1 atm and for each depth of 10m below the surface the pressure increase by 1 atm
This means that the pressure at the depth of the surface would be
![P_d = [\frac{15m}{10m} ] (1 atm) + 1 atm](https://tex.z-dn.net/?f=P_d%20%3D%20%5B%5Cfrac%7B15m%7D%7B10m%7D%20%5D%20%281%20atm%29%20%2B%201%20atm)

The ideal gas equation is mathematically represented as

Where P is pressure at the surface
V is the volume
R is the gas constant = 8.314 J/mol. K
making n the subject we have

Considering at the surface of the water the number of moles at the surface would be

Substituting
for
,
for volume , 8.314 J/mol. K for R , (37° +273) K for T into the equation

To obtain the number of moles at the depth of the water we use

Where
are pressure and no of moles at the depth of the water
Substituting values we have


Now to obtain the number of moles released we have



The molar concentration at the surface of water is
![[\frac{n}{V} ]_{surface} = \frac{0.2359mol}{6*10^-3m^3}](https://tex.z-dn.net/?f=%5B%5Cfrac%7Bn%7D%7BV%7D%20%5D_%7Bsurface%7D%20%3D%20%5Cfrac%7B0.2359mol%7D%7B6%2A10%5E-3m%5E3%7D)

The molar concentration at the depth of water is
![[\frac{n}{V} ]_{15m} = \frac{0.5897}{6*10^{-3}}](https://tex.z-dn.net/?f=%5B%5Cfrac%7Bn%7D%7BV%7D%20%5D_%7B15m%7D%20%3D%20%5Cfrac%7B0.5897%7D%7B6%2A10%5E%7B-3%7D%7D)

Now the ratio of the gases in Gabor's lungs at the depth of 15m to that at the surface is
