To solve this problem, we can rearrange the ideal gas law equation to solve for the number of moles of oxygen (n):
n = PV / RT
Given:
P = 1000 kPa
V = 12.0 L
R = 8.31 L*kPa/mol*K
T = 298 K
Substituting these values into the equation, we get:
n = (1000 kPa) * (12.0 L) / (8.31 L*kPa/mol*K) * (298 K)
Simplifying the equation, we find:
n = 1211.28 / 2466.78
n = 0.491 moles
Therefore, you took in approximately 0.49 moles of oxygen.
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?
Use the ideal gas law: PV = nRT where R=8.31 L*kPa/mol*K
Question 7 options:
0.05 mole
1.21 moles
2.42 moles
4.84 moles
1 answer
1 answer