On a cold winter day when the temperature is -20 degrees celsius, what is the amount of heat needed to warm internal body temp(37) the .5 L of air exchanged with each breath? Specific heat of air is 1020 J/(kg K) and that 1.0L air has a mass of 1.3g.
Please help!! I don't know where to start
heat= mass*c*deltaTemp
=1.3/2 g*1.020J/gK*57K
38 Joules dude
To determine the amount of heat needed to warm the .5 L of air exchanged with each breath, we can use the formula:
Q = m * c * ΔT
Where:
Q is the amount of heat needed
m is the mass of the air
c is the specific heat of air
ΔT is the change in temperature
First, let's convert the volume of air to kilograms:
Given that 1.0 L of air has a mass of 1.3 g, we can convert .5 L to grams as follows:
.5 L * (1.3 g / 1.0 L) = 0.65 g
Next, let's convert grams to kilograms:
0.65 g * (1 kg / 1000 g) = 0.00065 kg
Now, we need to calculate the change in temperature, ΔT:
ΔT = Tfinal - Tinitial
Tfinal is the final temperature, which is the internal body temperature of 37 degrees Celsius.
Tinitial is the initial temperature, which is the outside temperature of -20 degrees Celsius.
Now, let's convert the temperatures to Kelvin:
Tfinal = 37 + 273 = 310 K
Tinitial = -20 + 273 = 253 K
Now, we have all the values we need to calculate the amount of heat, Q:
Q = 0.00065 kg * 1020 J/(kg K) * (310 K - 253 K)
Calculating:
Q = 0.00065 kg * 1020 J/(kg K) * 57 K
Q ≈ 38.1 J
Therefore, the amount of heat needed to warm the .5 L of air exchanged with each breath from -20 degrees Celsius to 37 degrees Celsius is approximately 38.1 Joules.