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Air in the Lungs thermodynamics help!

  • Thread starter Nigzzzz
  • Start date
9
0
A submarine has run into trouble and is stuck at the bottom of the ocean. Several people are on board and must make their way to the surface without any diving gear. The air pressure aboard the submarine is 3.000 atm. The air temperature inside the submarine is 18.02 °C and you can take body temperature (inside the lungs) to be 36.04 °C.

1. The second person to leave also takes a breath as deep as possible by exhaling as far as possible (leaving a volume of 1.190 L in their lungs), and then slowly inhaling to increase their lung volume by 4.080 L. His body temperature is also 36.04 °C. This person breathes out all the way to the surface in order to maintain a constant lung volume. How many moles of gas remain in the lungs?


Relevant equations:
PV = nRT


The attempt at a solution:
i found the total volume of the lungs to be
Vtotal = 1.190L + 4.080L = 5.270L = 0.005270m^3

and using PV = nRT i found the number of moles at full capacity lungs
(3.00 x 101300)(0.005270) = n(8.314)(36.04+273.15)
n = 0.6230 moles

then i found the number of moles when the person exhales using PV = nRT
(3.00 x 101300)(0.004080 - 0.001190) = n(8.314)(36.04+273.15)
n = 0.365

∴ the change in moles is n = 0.6230 - 0.341 = 0.281mols

BUT the actual answer is 0.208 mols and i don't know what i'm doing wrong HELP!!
 

TSny

Homework Helper
Gold Member
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Hello, Nigzzzz.

What is volume of the lungs when the person reaches the surface?

What is the pressure of the air in the lungs at the surface?

What is the temperature of the air in the lungs at the surface?
 
9
0
have to assume that lung pressure is the same as air pressure as no other pressure is given so 3.00atm, and it's provided that lung temperature is at 36.04 °C, since the person exhaled all the way i would assume the remaining volume would be 1.190L
 

TSny

Homework Helper
Gold Member
11,978
2,590
have to assume that lung pressure is the same as air pressure as no other pressure is given so 3.00atm,
I think you can assume that the pressure inside the lungs will be the same as the pressure of the surroundings at the surface.

and it's provided that lung temperature is at 36.04 °C,
Yes, that sounds right.

since the person exhaled all the way i would assume the remaining volume would be 1.190L
Note that the problem stated that the volume of the lungs remains constant while going to the surface.
 
9
0
would that mean it remains at the inhaled capacity - 4.080L? or the difference between 2 volumes?
 

TSny

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What did you find for the total volume of the lungs after the inhale? That would be the volume of the lungs at the the start of the ascent to the surface.
 
9
0
it says that he slowly inhaled by 4.080L with a residual volume of 1.190L so after inhalation he would have 5.270L, would this be the volume constant in the ascend?
 

TSny

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That's how I interpret it.
 
9
0
but that would only be useful in giving me the number of moles in the lungs after inhalation? and it says that he exhaled to the surface to find the number of moles after exhalation?
 

TSny

Homework Helper
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But if you know the three quantities that I asked about in post #2, can you find the number of moles left in the lungs at the surface?
 
9
0
OHHH

so you use PV = nRT

101300 x 0.005270 = n(8.314)(36.04 + 273.15)

n = 0.208 moles

OK i think i get it! hahaha
 
Last edited:
9
0
thanks so much!
 

TSny

Homework Helper
Gold Member
11,978
2,590
OK, good. (But it's a little strange the way you wrote your last equation. The amount on the far left of the equation does not equal the amount in the middle or the amount on the right. :smile:)
 
9
0
woops forgot the n thats why
 

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