Question

Please help fast

A person breathes in 6.0 L of pure oxygen at 298 K and
1,000 kPa to fill their lungs
How many moles of oxygen did they take in?
Use the ideal gas law: PV = nRT where R = 8.31 L – kPa /mol – K

A) 0.05 mole
B) 0.41 mole
C) 2.42 moles
D) 20.0 moles

Answer 1

Moles of Oxygen they took in : C. 2.42

Further explanation

The gas equation can be written

`\large{\boxed{\bold{PV=nRT}}}`

where

P = pressure, atm

V = volume, liter

n = number of moles

R = gas constant = 0.08205 l.atm / mol K

T = temperature, Kelvin

P=1000 kPa

V = 6 L

T = 298 K

moles of Oxygen :

`\tt n=(PV)/(RT)\\\\n=(1000* 6)/(8.31* 298)\\\\n=2.42~moles`