Answer:
Mass percent XeF₄: 13.78%
Mass percent XeF₆: 86.22%
Explanation:
Moles of Xe are equal to moles of XeF₄ + Moles XeF₆:
<em>Moles Xe:</em>
1.85x10⁻⁴mol - 9.00x10⁻⁶ mol = 1.76x10⁻⁴ moles Xe reacted:
1.76x10⁻⁴ moles = Moles of XeF₄ + Moles XeF₆ <em>(1)</em>
<em> </em>
Moles of F₂ = 1/2 Moles XeF₄ + 1/3 Moles XeF₆
5x10⁻⁴ = 2 Moles XeF₄ + 3 Moles XeF₆ (2)
Replacing (1) in (2):
5x10⁻⁴ = 2 Moles XeF₄ + 3 Moles XeF₆
5x10⁻⁴ = 2 (1.76x10⁻⁴ moles - 1 Mol XeF₆) + 3 Moles XeF₆
5x10⁻⁴ = 3.52x10⁻⁴ - 2 Mol XeF₆ + 3 XeF₆
1.48x10⁻⁴ = Mol XeF₆
And moles XeF₄:
Moles XeF₄ = 1.76x10⁻⁴ moles - 1.48x10⁻⁴ moles = 2.8x10⁻⁵ moles
In grams (Molar mass XeF₄: 207.28g/mol: XeF₆: 245.28g/mol):
Mass XeF₄: 2.8x10⁻⁵ mol * (207.28g / mol) = 5.8x10⁻³g
Mass XeF₆: 1.48x10⁻⁴ mol * (245.28g / mol) = 0.0363g
Mass percent XeF₄:
5.8x10⁻³g / (5.8x10⁻³g + 0.0363g) * 100 = 13.78%
Mass Percent XeF₆:
0.0363g / (5.8x10⁻³g + 0.0363g) * 100 = 86.22%
