To find the volume of 84.7 g of O2 at 1.07 atm and 37.4 °C, we can use the Ideal Gas Law:
PV = nRT
First, we need to convert the mass of O2 into moles. The molar mass of O2 is 32 g/mol.
84.7 g / 32 g/mol = 2.646875 mol
Next, we can plug in the values into the Ideal Gas Law formula:
V = (nRT) / P
V = (2.646875 mol * 0.0821 L atm/mol K * 310.4 K) / 1.07 atm
V = 68.244 L
Therefore, the volume of 84.7 g of O2 at 1.07 atm and 37.4 °C is 68.244 liters. In scientific notation, this is expressed as 6.8244 x 10^1 L.
If a person inhales 84.7 g of O2 in an hour, what volume (in L) does this amount occupy at 1.07 atm and 37.4 °C? Be sure your answer has the correct number
of significant figures.
Note: Reference the Fundamental constants table for additional information.
what is the answer can you write it in scientific notation
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