What is the mass of a sample of O₂ gas, which has a pressure of 740. mmHg, at a temperature of 25 °C, in a volume of 250. mL?

Question

What is the mass of a sample of O₂ gas, which has a pressure of 740. mmHg, at a temperature of 25 °C, in a volume of 250. mL? A)320. g B)292 g C)0.318 g D)201 g E)3.82 g

Quizplus · Accepted Answer

To use the ideal gas law equation (PV = nRT), we need to convert the pressure to atm and the volume to liters, and use the R constant in appropriate units (0.0821 L·atm/mol·K). 740 mmHg = 0.973 atm 250 mL = 0.25 L Plugging these values into the equation: (0.973 atm) x (0.25 L) = n x (0.0821 L·atm/mol·K) x (25 + 273 K) n = 0.0131 mol To find the mass, we need to use the molar mass of O₂ gas. This is not a real compound or molecule name, so we cannot find its molar mass. Therefore, we cannot use the molar mass to directly convert moles to grams. The only reasonable choice among the options is C, which is the only answer close to the expected range of mass for a gas in a small volume at standard conditions. The actual mass of the gas cannot be determined without more information.

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