Respuesta :
Answer:
The increase in pressure inside the lungs is 0.09 atm
Explanation:
From the Pressure law
Pressure law states that the volume of a fixed mass of gas is directly proportional to the absolute temperature provided that the volume remains constant.
That is,
P ∝ T
Where P is the Pressure and T is the temperature.
Then, we can write that
P = kT
Where k is the proportionality constant
∴ [tex]\frac{P}{T} = k[/tex]
Then,
[tex]\frac{P_{1} }{T_{1} } = \frac{P_{2} }{T_{2} }[/tex]
From the question, [tex]P_{1}[/tex] = 1.0 atm
[tex]{T_{1}[/tex] = 12 °C = (12 + 273.15) K = 285.15K
[tex]{T_{2}[/tex] = 37 °C = (37 + 273.15) K = 310.15K
Therefore,
[tex]\frac{1.0}{285.15} = \frac{P_{2} }{310.15}[/tex]
[tex]P_{2} = \frac{1.0 \times 310.15}{285.15}[/tex]
[tex]P_{2} = 1.09[/tex] atm
Increase in pressure = [tex]P_{2} - P_{1}[/tex] = 1.09 atm - 1.0 atm
Increase in pressure = 0.09 atm
Hence, the increase in pressure inside the lungs is 0.09 atm
At constant volume, pressure of the gas is directly proportional to the temperature of the gas. The increased pressure inside the lungs is 0.9 atm.
From Gas law,
[tex]\bold {\dfrac {P_1} {T_1 } = \dfrac {P_2} {T_2 } }[/tex]
Where,
P1 - initial pressure = 0.1 atm
P2 - final pressure = ?
T1 - initial temperature = 12 °C = (12 + 273.15) K = 285.15 K
T2 - final temperature = 37 °C = (37 + 273.15) K = 310.15 K
Put the values in the formula,
[tex]\bold {\dfrac {1.0} {285.15 } = \dfrac {P_2} {310.15 } }[/tex]
[tex]\bold {P_2 = 1.09\ atm}[/tex]
Thus, increased pressure in the lungs
= 1.9 - 1.0
= 0.9 atm
Therefore, the increased pressure inside the lungs is 0.9 atm.
To know more about Pressure,
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