If a person exhales 32.5 g of CO2 in an hour, what volume (in L) does this amount occupy at 1.04 atm and 36.9 C? Be sure your answer has the correct
number of significant figures.
Note: Reference the Fundamental constants table for additional information.
To solve this problem, we can use the ideal gas law:
PV = nRT
where:
P = pressure = 1.04 atm
V = volume (to be calculated)
n = number of moles of CO2
R = ideal gas constant = 0.08206 L·atm/mol·K
T = temperature = 36.9 + 273.15 K
First, we need to calculate the number of moles of CO2:
molar mass of CO2 = 12.01 g/mol (C) + 2(16.00 g/mol) = 44.01 g/mol
n = mass / molar mass
n = 32.5 g / 44.01 g/mol
n ≈ 0.739 moles
Now we can calculate the volume using the ideal gas law:
V = nRT / P
V = (0.739 mol)(0.08206 L·atm/mol·K)(36.9 + 273.15 K) / 1.04 atm
V ≈ 19.8 L
Therefore, the volume of 32.5 g of CO2 at 1.04 atm and 36.9 C is approximately 19.8 L.