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ratelena [41]
3 years ago
12

On a chilly 12∘C day, you quickly take a deep breath--all your lungs can hold, 4.0 L. The air warms to your body temperature of

37∘C.
If the air starts at a pressure of 1.0 atm, and you hold the volume of your lungs constant (a good approximation) and the number of molecules in your lungs stays constant as well (also a good approximation), what is the increase in pressure inside your lungs?
Physics
1 answer:
laiz [17]3 years ago
7 0

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

∴ \frac{P}{T} = k

Then,

\frac{P_{1} }{T_{1} } = \frac{P_{2} }{T_{2} }

From the question, P_{1} = 1.0 atm

{T_{1} = 12 °C = (12 + 273.15) K = 285.15K

{T_{2} = 37 °C = (37 + 273.15) K = 310.15K

Therefore,

\frac{1.0}{285.15} = \frac{P_{2} }{310.15}

P_{2} = \frac{1.0 \times 310.15}{285.15}

P_{2} = 1.09 atm

Increase in pressure = P_{2} - P_{1} = 1.09 atm - 1.0 atm

Increase in pressure = 0.09 atm

Hence, the increase in pressure inside the lungs is 0.09 atm

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Answer:

218.93 km

Explanation:

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Electron: Its electrical charge is -1, its mass is negligible, it's found outside the nucleus

Explanation:

Atoms consist of three types of particles:

  • Proton: the proton is found in the nucleus of the atom, and it has a positive electric charge, equal to +1.6\cdot 10^{-19}C (expressed in units of fundamental charge, it has a charge of +1). Its mass is 1.67\cdot 10^{-27}kg, while its mass expressed in atomic mass units is 1 a.m.u
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Meanwhile, the horizontal component of the ball's position vector is

x=x_0+v_{0x}t+\dfrac12a_xt^2

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