A 28.3-g mixture of oxygen and argon is found to occupy a volume of 17.2 L when measured at 882.7 mmHg and 39.3^oC.What is the partial pressure of oxygen in this mixture? A)369 mmHg B)441 mmHg C)512 mmHg D)418 mmHg E)464 mmHg

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Quizplus · Accepted Answer

To find the partial pressure of oxygen, we can use Dalton's Law of Partial Pressures and the Ideal Gas Law. First, we convert the temperature to Kelvin (39.3°C + 273.15 = 312.45 K) and pressure to atm (882.7 mmHg / 760 = 1.161 atm). The total moles of gas can be found using PV = nRT, rearranged to n = PV/RT. Substituting the values (P = 1.161 atm, V = 17.2 L, R = 0.0821 L·atm/(mol·K), T = 312.45 K), we find the total moles of gas. Then, knowing the molar masses of oxygen (32.00 g/mol) and argon (39.95 g/mol), we can calculate the mass fraction of oxygen in the mixture and thus its mole fraction. Finally, the partial pressure of oxygen is found by multiplying the total pressure by the mole fraction of oxygen. This calculation results in a partial pressure of oxygen close to 418 mmHg.

A 283-G Mixture of Oxygen and Argon Is Found to Occupy