Question

The partial pressure of fluorine gas in a 2.00 L container is 0.85 atm while the partial pressure in that same 2.00L container of argon gas is 1350 torr. a) What is the total pressure, in atm? b) What is the mole fraction of argon in the container?

Answer 1

Answer: The total pressure, in atm is 2.62

b. The mole fraction of argon in the container is 0.67.

Step-by-step explanation:

a) According to Dalton's law, the total pressure is the sum of individual pressures.

`p_(total)=p_A+p_B+p_C...`

Given :
`p_(total)` =total pressure of gases = ?

`p_(F_2)` = partial pressure of fluorine = 0.85 atm

`p_(Ar)` = partial pressure of Argon = 1350 torr = 1.77 atm ( 760 torr = 1atm)

putting in the values we get:

`p_(total)=0.85atm+1.77atm=2.62atm`

b) According to Raoult's law, the partial pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the total pressure.

`p_(Ar)=x_(Ar)p_(total)`

where, x = mole fraction

`1.77atm=x_(Ar)* 2.62atm`

`x_(Ar)=0.67`

The mole fraction of argon in the container is 0.67.