Question

A mixture of oxygen and xenon gases, at a total pressure of 755 mm Hg, contains 8.10 grams of oxygen and 13.7 grams of xenon. What is the partial pressure of each gas in the mixture? mm Hg Po2 mm Hg Pxe

Answer 1

1)

Molar mass of O2 = 32 g/mol

Molar mass of Xe = 131.3 g/mol

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

= 8.1/32

= 0.2531

n(Xe) = mass of Xe/molar mass of Xe

= 13.7/131.3

= 0.1043

n(O2),n1 = 0.2531 mol

n(Xe),n2 = 0.1043 mol

Total number of mol = n1+n2

= 0.2531 + 0.1043

= 0.3575 mol

a)

Partial pressure of each components are

p(O2),p1 = (n1*Ptotal)/total mol

= (0.2531 * 755)/0.3575

= 535 mmHg

Answer: 535 mmHg

b)

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

= (0.1043 * 755)/0.3575

= 220. mmHg

Answer: 220. mmHg

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