You breathe in 6. 0 L of pure oxygen at 298 K and 1,000 kPa to fill your lungs. How many moles of oxygen did you take in? Use the ideal gas law: PV = nRT where R=8. 31 L−kPa/mol−K 0. 05 mole 0. 41 mole 2. 42 moles 20. 0 moles.

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You breathe in 6. 0 L of pure oxygen at 298 K and 1,000 kPa to fill your lungs. How many moles of oxygen did you take in? Use the ideal gas law: PV = nRT where R=8. 31 L−kPa/mol−K 0. 05 mole 0. 41 mole 2. 42 moles 20. 0 moles.

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Aliasger2709id Aliasger2709id · Answer 1

The ideal gas law is the generalized gas equation that depicts the state of the hypothetical gas condition. Moles of oxygen take in is 2.42 mol.

What is the Ideal gas equation?

The ideal gas equation gives the equation about the product of the pressure and the volume to be equal to that of the product of moles, temperature and the gas constant of the gas.

The formula for the ideal gas equation is:

[tex]\rm PV = nRT[/tex]

Where,

Pressure (P) = 1000 kPa
Volume (V) = 6.0 L
Ideal gas constant (R) = [tex]8. 31 \;\text{LkPa/mol K}[/tex]
Temperature (T) = 298 K
Number of moles = n

Substituting values in the equation:

[tex]\begin{aligned} 1000 \times 6 &= \rm n \times 8.31 \times 298\\\\\rm n &= \dfrac{1000 \times 6}{8.31 \times 298}\\\\& = 2.42\;\rm moles\end{aligned}[/tex]

Therefore, 2.42 moles of oxygen is taken in during the respiration process.

Learn more about the ideal gas equation here:

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