Question

You draw in a deep breath on a chilly day, inhaling 3.8 L of 0ˆ˜C air. If the pressure in your lungs is a constant 1.0 atm, how much heat must your body supply to warm the air to your 37ˆ˜C internal body temperature? Assume that for air Cₚ​=29.1J/(K‹⋅mol) as it consists mostly of nitrogen. A) (Numerical answer required) B) 0 J C) 291 J D) 29,100 J

Answer 1

To warm the air to your internal body temperature, your body does not need to supply any heat (Option B).

Step-by-step explanation:

To calculate the amount of heat your body must supply to warm the air to your internal body temperature, you can use the formula:

q = n Þltah

where q is the heat in joules, n is the number of moles, and Þltah is the change in enthalpy.

In this case, you know the volume of air inhaled and the pressure is constant, so you can calculate the number of moles of air. Then, using the specific heat capacity of air, you can determine the change in enthalpy. Finally, you can substitute the values into the formula to find the heat required.

The answer is B) 0 J.