How many grams of fluorine are required to produce 10.0 g of XeF6?

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asked Jun 20, 2018 196k views

1 Answer

Chris Hamilton · Answer 1 · 2018-06-25T01:10:06+0000

moles XeF6 = 10.0 g/ 245.28 g/mol=0.0408

the ratio between F2 and XeF6 is 3 : 1

moles F2 required = 3 x 0.0408=0.122

mass F2 = 0.122 mol x 37.9968 g/mol=4.64 g

How many grams of fluorine are required to produce 10.0 g of XeF6?

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