Answer:
Partial pressure O₂ → 2.74 atm
Explanation:
Let's analyse the data given:
Volume → 3L
In the bottle there is a mixture of gases that contains, O₂, N₂ and CO₂.
Total pressure is 4.80 atm
Let's apply the Ideal Gases Law to determine the total moles of the mixture
P . V = n . R. T
4.80 atm . 3L = n . 0.082 . 273K
n = 4.80 atm . 3L / 0.082 . 273K → 0.643 moles
We apply the concept of mole fraction:
Mole fraction of a gas X = moles of gas X / Total moles
Mole fraction of a gas X = Partial pressure X / Total pressure
In a mixture, sum of mole fraction of each gas = 1
We determine mole fraction of N₂ → 0.230 / 0.643 = 0.357
We determine mole fraction of CO₂ → 0.350 atm / 4.80 atm = 0.0729
1 - mole fraction N₂ - mole fraction CO₂ = mole fraction O₂
1 - 0.357 - 0.0729 = 0.5701 → mole fraction O₂
We replace in the formula: Mole fraction O₂ = Partial pressure O₂ / 4.80 atm
0.5701 . 4.80 atm = Partial pressure O₂ → 2.74 atm
