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.

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Md Ariful Islam · Answer 1 · Apr 23, 2024 15:00:48

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:

P_i = P_total × x_i

Therefore,

P(O₂) = P_total× 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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