How many moles of gas are contained in a human breath that occupies 94.0 L and has a pressure of 746. mmHg at 38. °C? Be sure your answer has the correct
number of significant figures.
Note: Reference the Fundamental constants and Conversion factors for non-SI units table for additional information.
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure = 746 mmHg = 746/760 atm = 0.98289474 atm
V = volume = 94.0 L
n = number of moles of gas
R = ideal gas constant = 0.0821 L.atm/mol.K
T = temperature = 38 + 273 = 311 K
Now we can rearrange the ideal gas law equation to solve for n:
n = (P * V) / (R * T)
n = (0.98289474 atm * 94.0 L) / (0.0821 L.atm/mol.K * 311 K)
n = (92.30631556 atm*L) / (25.5231 L.atm/mol)
n = 3.616 mol
Therefore, there are approximately 3.62 moles of gas in a human breath that occupies 94.0 L at a pressure of 746 mmHg and a temperature of 38. °C.