A 2.0 dm³ container contains 0.15 mol of N₂ gas and 0.20 mol of O₂ gas under a total pressure of 100 kNm⁻². Calculate the partial pressure of O₂ gas in the mixture.
Solution:
Calculate the mole fraction (x) of O2 gas in the mixture:
x(O2) = number moles of O2 / total number moles of gas
Total number moles of gas = Moles of N2 + Moles of O2 = 0.15 mol + 0.20 mol = 0.35 mol
Therefore,
x(O2) = (0.20 mol) / (0.35 mol) = 0.57
The partial pressure of one individual gas within the overall mixtures can be expressed as follows:
Pi = Ptotal × xi
Therefore,
P(O2) = Ptotal × x(O2)
P(O2) = (100 kN m-2) × (0.57) = 57 kN m-2
P(O2) = 57 kN m-2
Answer: The partial pressure of O2 gas in the mixture is 57 kN m-2
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