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
[tex]PV=nRT\\[/tex]
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
[tex]P=KT\\[/tex]
where pressure and temperature are the only varying parameters.
if we vary the constant K we arrive at
[tex]\frac{P_{1} }{T_{1}}=\frac{P_{1} }{T_{1}}=...=\frac{P_{n} }{T_{N}}\\[/tex]
since the Temprature must be in absolute temperature, we add 273k to it Celsius value.
[tex]T_{1} =12+273=285k\\T_{2} =37+273=310k\\P_{1} =1 atm\\[/tex]
Substituting value into the generated equation, we have
[tex]P_{2}=\frac{310*1}{285} \\P_{2}=1.09 atm.\\[/tex]
