The partial pressure of F2 in a mixture of gases where the total pressure is 1.00 atm is 300 torr. The mole fraction is 0.149.
We need to calculate the mole fraction. The mole fraction is defined as the ratio of the number of moles of a component in a mixture to the total number of moles of all components in the mixture.The partial pressure of F2 is given to be 300 torr.
The total pressure is given to be 1.00 atm.
Partial pressure is the pressure exerted by one of the components of the mixture. It is defined as the product of the mole fraction and the total pressure.
The formula for mole fraction is:
nF2 / ntotal = partial pressure of F2 / total pressure
The mole fraction of F2 is given by:
nF2 / ntotal = (300 torr) / (1.00 atm) = 0.316
This is the mole fraction of F2. We need to find the mole fraction of the mixture.
The mole fraction of the mixture is given by:
nF2 + nO2 / ntotal
= partial pressure of F2 + partial pressure of O2 / total pressurenO2 / ntotal
= (1.00 atm - 300 torr) / (1.00 atm)
= 0.70nF2 / ntotal + 0.70 = 1.00nF2 / ntotal
= 0.30
The mole fraction of F2 is:nF2 / ntotal = 0.30
The mole fraction of the mixture is:
nF2 + nO2 / ntotal = nF2 / ntotal + nO2 / ntotal = 0.30 + 0.70 = 1.00
Therefore, the mole fraction of the mixture is 1.00. The mole fraction of F2 is 0.30. The mole fraction of O2 is 0.70.