Question

A mixture of f2, h2 and xe have mole fractions of 0.25, 0.65, and 0.10, respectively. what is the pressure of f2 if the total pressure of the mixture is 3.9 atm?

Answer 1

Answer : The pressure of $F_2$ is 0.975 atm.

Solution : Given,

Mole fraction of $F_2$ = 0.25

Mole fraction of $H_2$ = 0.65

Mole fraction of $Xe$ = 0.10

Total pressure of mixture = 3.9 atm

According to the Dalton's law of partial pressure, which tells that the partial pressure of a gas is directly proportional to the mole fraction of a gas.

$P_{gas}\propto X_{gas}$

$P_{gas}=X_{gas}\times P_{Total}$

where,

$P_{gas}$ = partial pressure of a gas

$X_{gas}$ = mole fraction of a gas

$P_{Total}$ = total pressure of gas

Now we have to calculate the partial pressure of $F_2$ gas.

Put all the given values in above formula, we get

$P_{F_2}=X_{F_2}\times P_{Total}=0.25\times 3.9atm=0.975atm$

The partial pressure of $F_2$ is 0.975 atm.