# The cylinder contains m1 = 8 g of hydrogen and m2 = 12 g of nitrogen at a temperature of t = 17C

The cylinder contains m1 = 8 g of hydrogen and m2 = 12 g of nitrogen at a temperature of t = 17C and under a pressure of p = 1.8 * 10 ^ 5 Pa. Determine the molar mass of the mixture and the volume V of the cylinder.

Data: mH2 (mass of hydrogen) = 8 g; mN2 (mass of nitrogen) = 12 g; Т (abs. Temperature of the created mixture) = 290 К (17 ºС); P (cylinder pressure) = 1.8 * 10 ^ 5 Pa.

Constants: R (universal gas constant) = 8.31 J / (K * mol); MH2 (molar mass of hydrogen) = 2 g / mol; MN2 (molar mass of nitrogen) = 28 g / mol.

1) The molar mass of the created mixture: Mcm = (mH2 + mN2) / (mH2 / MH2 + mN2 / MN2) = (8 + 12) / (8/2 + 12/28) = 4.516 g / mol.

2) The volume of the cylinder used: V = m * R * T / (P * M) = (mH2 + mN2) * R * T / (P * Mcm) = (8 + 12) * 8.31 * 290 / (1 , 8 * 10 ^ 5 * 4.516) = 0.059 m3.

Answer: The volume of the cylinder used is 0.059 m3.

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