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

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