Question

A mixture of Ar, CO₂ and Cl₂ has a pressure of 7.85 atm. if the ar has a mole fraction of 0.47 and CO₂ has a mole fraction of 0.23, what is the partial pressure of Cl₂?

Answer 1

The partial pressure of Cl₂ in the gas mixture with a total pressure of 7.85 atm, given the mole fractions of Ar and CO₂, is 2.355 atm.

Step-by-step explanation:

To calculate the partial pressure of Cl₂ in a mixture of Ar, CO₂, and Cl₂ with a total pressure of 7.85 atm, where Ar has a mole fraction of 0.47 and CO₂ has a mole fraction of 0.23, we can apply the formula PA = XA * Ptot, where PA is the partial pressure of the gas A, XA is the mole fraction of gas A, and Ptot is the total pressure of the gas mixture.

First, we must find the mole fraction of Cl₂ by knowing that the sum of mole fractions in a mixture equals 1:

Mole fraction of Cl₂ = 1 - (mole fraction of Ar + mole fraction of CO₂) = 1 - (0.47 + 0.23) = 1 - 0.70 = 0.30

Then, we calculate the partial pressure of Cl₂:

Partial pressure of Cl₂ = Mole fraction of Cl₂ * Total pressure = 0.30 * 7.85 atm = 2.355 atm