To solve this problem, we can use the ideal gas law equation:
PV = nRT
First, we need to calculate the number of moles of CO2 exhaled by the person. We are given the mass of CO2 (27.0 g) and the molar mass of CO2 (44.01 g/mol). We can use these values to find the number of moles:
n = mass / molar mass
n = 27.0 g / 44.01 g/mol
n = 0.6136 mol
Now we can use the ideal gas law to find the volume occupied by this amount of CO2:
V = (nRT) / P
V = (0.6136 mol * 0.08206 L.atm/mol.K * 309.05 K) / 1.07 atm
V = 15.58 L
Therefore, the volume of 27.0 g of CO2 at 1.07 atm and 36.9 °C is 15.58 L. Be sure to report your answer with the correct number of significant figures, in this case, 3 significant figures.
If a person exhales 27.0 g of CO2 in an hour, what volume (in L) does this amount occupy at 1.07 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.
1 answer