Question

You breathe in 12.0 L of pure oxygen at 298 K and 1,000 kPa to fill your lungs. How many moles of oxygen did you take in. Can you also show me how to solve this please?

Answer 1

We are given with
V = 12L
T = 298 K
P = 1000 kPa

We are asked to get the number of moles, n

We can solve this using the ideal gas law
PV = nRT
n = PV / RT
Simply substitute the values and use the appropriate value for R.

Answer 2

Answer:

Your question must be at 1.000kPa not 1,000KPa... That's ~10Atms, or 10x atmospheric pressure we as humans are used to breathing... So the following calculation is for 1.000kPa or 0.987Atms. => 0.482 mole O₂(g). If your problem is at 1,000kPa then multiply mole answer by 10.

Explanation:

Using the Ideal Gas Law PV = nRT solve for n = PV/RT

n = moles of O₂(g)

P = Pressure = 1.000KPa = 0.987Atm

V = Volume in liters = 12L

R = Universal Gas Constant = 0.08206 L·Atm/mol·K

T = Temperature in Kelvin = 298K

n = P·V/R·T = (0.987Atm)(12L)/(0.08206 L·Atm/mol·K)(298K) = 0.482 mole O₂(g)