The pressure of O₂ in a 15.0 L flask is 322 mm Hg at 44 $\circ$ C.What mass of O₂ is in the flask? (R = 0.08206 L.atm/mol.K) A) 0.244 g B) 5.80 g C) 7.82 g D) 15.2 g E) 56.3 g

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Using the ideal gas law, PV = nRT, we can solve for n (moles of O2). Convert pressure to atm (322 mm Hg = 0.4237 atm) and temperature to Kelvin (44°C = 317 K). Then, n = (0.4237 atm * 15.0 L) / (0.08206 L.atm/mol.K * 317 K) = 0.244 moles. The molar mass of O2 is 32.00 g/mol, so mass = 0.244 moles * 32.00 g/mol = 7.82 g.

The Pressure of O2 in a 15 ∘\circ∘ CWhat Mass of O2 Is in the Flask? (R =

The Pressure of O₂ in a 15 $\circ$ CWhat Mass of O₂ Is in the Flask? (R =