I have the first two parts answered but I don't know how to do
the last part please help! Human lung capacity varies from about
4.0L to 6.0L, so we shall use an average of 5.0L. The air enters
at the ambient temperature of the atmosphere and must be heated
to internal body temperature at an approximately constant
pressure of 1.00 atm in our model. Suppose you are outside on a
winter day when the temperature is -2.00F. Part A How many moles
of air does your lung hold if the 5.0 L is at the internal body
temperature of 37 C? n = .196 mol Part B How much heat must your
body have supplied to get the 5.0 L of air up to internal body
temperature, assuming that the atmosphere is all N2? Q = 320 J
Part C Suppose instead that you manage to inhale the full 5.0 L
of air in one breath and hold it in your lungs without expanding
(or contracting) them. How much heat would your body have had to
supply in that case to raise the air up to internal body
temperature? Q = _____ J