What is the partial pressure of N₂ in a mixture of 0.36 mole N₂, 0.15 mole Ne, and 0.75 mole of O₂ that has a total pressure of 3.18 atm?

Question

Quizplus · Accepted Answer

The partial pressure of a gas in a mixture can be calculated using Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. The partial pressure of a gas is proportional to its mole fraction in the mixture. The mole fraction is calculated by dividing the number of moles of the gas by the total number of moles of all gases in the mixture.Total moles = 0.36 (N₂) + 0.15 (Ne) + 0.75 (O₂) = 1.26 molesMole fraction of N₂ = 0.36 / 1.26Partial pressure of N₂ = Mole fraction of N₂ * Total pressure = (0.36 / 1.26) * 3.18 atm ≈ 0.91 atm.

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