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
The partial pressure of Cl₂ in the flask is 0.70 atm
Partial pressure can be derived through the following:
Total pressure of a gas mixture = sum of the partial pressures of individual gases
P(total) = P(f₂) + P(cl₂)
Partial pressure = Mole fraction × Total pressure
Let us represent the mass of each gas as m.
Number of moles of F₂ = m/38 (molar mass of Fl₂) = 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
Partial pressure of Cl₂ = 0.35 × 2 = 0.70 atm
Partial Pressure of F₂ = 0.65 × 2 = 1.30 atm
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