Question

A gaseous mixture of O2 and N2 contains 36.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 585 Torr ?

Answer #1

**let total mass be 100 g**

**mass of N2 = 36.8 g**

**mass of O2 = 100 - 36.8 = 63.2 g**

**Molar mass of N2 = 28.02 g/mol**

**Molar mass of O2 = 32 g/mol**

**n(N2) = mass of N2/molar mass of N2**

**= 36.8/28.02**

**= 1.3133**

**n(O2) = mass of O2/molar mass of O2**

**= 63.2/32.0**

**= 1.975**

**n(N2),n1 = 1.3133 mol**

**n(O2),n2 = 1.975 mol**

**Total number of mol = n1+n2**

**= 1.3133 + 1.975**

**= 3.2883 mol**

**Partial pressure of each components are**

**p(N2),p1 = (n1*Ptotal)/total mol**

**= (1.3133 * 585)/3.2883**

**= 234 torr**

**p(O2),p2 = (n2*Ptotal)/total mol**

**= (1.975 * 585)/3.2883**

**= 351 torr**

**Answer:**

**partial pressure of N2 = 234 torr**

**partial pressure of O2 = 351 torr**

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Part B
A gaseous mixture of O2 and N2 contains 40.8 % nitrogen by mass.
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Express you answer numerically in millimeters of mercury.
Hints
Poxygen =
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