A closed flask contains 0.25 mol of O₂ that exerts a pressure of 0.50 atm. Calculate the partial pressure of oxygen when 0.75 mol of CO₂ is added to the container. A) 0.50 atm B) 1.0 atm C) 1.5 atm D) 2.0 atm

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Quizplus · Accepted Answer

The total moles of gas after adding CO2 is 0.25 + 0.75 = 1.0 mol. Since both gases behave ideally, the partial pressure of each gas is proportional to its mole fraction. The mole fraction of O2 is 0.25/1.0 = 0.25. The total pressure remains 0.50 atm, so the partial pressure of O2 is 0.25 * 0.50 atm = 0.125 atm. However, without the options matching this calculation, and assuming a misunderstanding in the interpretation, the initial condition suggests the pressure of O2 remains unchanged if we consider the total pressure to be distributed equally among the gases without additional information on volume or temperature changes. Thus, the closest answer provided is 0.50 atm, assuming no change in the initial conditions of O2 specifically.

A Closed Flask Contains 0