Question

A mixture of nitrogen and xenon gases contains nitrogen at a partial pressure of 417 mm Hg and xenon at a partial pressure of 427 mm Hg. What is the mole fraction of each gas in the mixture

Answer 1

0.4941, 0.5059

Step-by-step explanation:

`P_N` = Partial pressure of nitrogen = 417 mm Hg

`P_(Xe)` = Partial pressure of xenon = 427 mm Hg

Total pressure in the system is given by

`P=P_N+P_(Xe)\\\Rightarrow P=417+427=844\ \text{mm Hg}`

Mole fraction is given by

`X_N=(P_N)/(P)\\\Rightarrow X_N=(417)/(844)\\\Rightarrow X_(N)=0.4941`

For xenon

`X_(Xe)=1-0.4941=0.5059`

or

`X_(Xe)=(P_(Xe))/(P)\\\Rightarrow X_(Xe)=(427)/(844)\\\Rightarrow X_(Xe)=0.5059`

So, mole fraction of nitrogen is 0.4941 and xenon is 0.5059.