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?

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

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

where pressure and temperature are the only varying parameters.

if we vary the constant K we arrive at

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

Substituting value into the generated equation, we have

multiply 2kg by latent heat of vap