Question

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?

Answer 1

Answer:

the question is incomplete, here is the complete question.

"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?

1.09 atm

Explanation:

the question addresses an ideal gas. where the relationship between the volume(v),pressure(p),temperature(T) and nos of molecules(n) is expressed as

$PV=nRT$

Where R us the ideal gas constant.

From the question,the number of molecules,volume are constant, we can now re-write the equation as

       $P=KT$

where pressure and temperature are the only varying parameters.

if we vary the constant K we arrive at

$\frac{P_{1} }{T_{1}}=\frac{P_{1} }{T_{1}}=...=\frac{P_{n} }{T_{N}}$

since  the Temprature must be in absolute temperature, we add 273k to it Celsius value.

$T_{1} =12+273=285k\\T_{2} =37+273=310k\\P_{1} =1 atm$

Substituting value into the generated equation, we have

$P_{2}=\frac{310*1}{285} \\P_{2}=1.09 atm.$