Determine the partial pressure of N₂ in a gas mixture composed of 1.0 mol of N₂ and 1.5 mol of Ar.The mixture is at 0.0ºC in a 10.0-liter container.

Question

Quizplus · Accepted Answer

First, we need to find the total pressure of the gas mixture using the ideal gas law: PV = nRT P = nRT / V P = (1.0 mol + 1.5 mol) * 0.0821 L atm / (mol K) * 273 K / 10.0 L P = 5.60 atm Next, we can use Dalton's law of partial pressures to find the partial pressure of N₂: P(N₂) = X(N₂) * P(total) where X(N₂) is the mole fraction of N₂ in the mixture: X(N₂) = n(N₂) / (n(N₂) + n(Ar)) X(N₂) = 1.0 mol / (1.0 mol + 1.5 mol) X(N₂) = 0.4 Now we can substitute in the values: P(N₂) = 0.4 * 5.60 atm P(N₂) = 2.24 atm Therefore, the partial pressure of N₂ in the gas mixture is 2.24 atm, which corresponds to choice (E).

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Determine the Partial Pressure of N₂ in a Gas Mixture