A mixture of N2 and Ar gases in a cylinder contains 7 g of N2 and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of N2 is: [Use atomic masses (in g mol⁻¹): N = 14, Ar = 40]

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12 bar. First, calculate the moles of N2 (7 g / 28 g/mol = 0.25 mol) and Ar (8 g / 40 g/mol = 0.2 mol). The mole fraction of N2 is 0.25 / (0.25 + 0.2) = 0.555. The partial pressure of N2 is 0.555 × 27 bar = 15 bar.

A mixture of N2 and Ar gases in a cylinder contains 7 g of N2 and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of N2 is: [Use atomic masses (in g mol⁻¹): N = 14, Ar = 40]

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