Answer:
Partial Pressure of F₂ = 1.30 atm
Partial pressure of Cl₂ = 0.70 atm
Explanation:
Partial pressure for gases are given by Daltons law.
Total pressure of a gas mixture = sum of the partial pressures of individual gases
Pt = P(f₂) + P(cl₂)
Partial pressure = mole fraction × total pressure
Let the mass of each gas present be m
Number of moles of F₂ = m/38 (molar mass of fluorine = 38 g/Lol
Number of moles of Cl₂ = m/71 (molar mass of Cl₂)
Mole fraction of F₂ = (m/38)/((m/38) + (m/71)) = 0.65
Mole fraction of Cl₂ = (m/71)/((m/38) + (m/71)) = 0.35 or just 1 - 0.65 = 0.35
Partial Pressure of F₂ = 0.65 × 2 = 1.30 atm
Partial pressure of Cl₂ = 0.35 × 2 = 0.70 atm
