Homework Help

How many grams of xenon are required to form 20.0 g of xenon hexafluoride? What is the...

user profile pic

takenotes | Student, Grade 9 | (Level 1) Honors

Posted May 9, 2013 at 8:51 PM via web

dislike 1 like

How many grams of xenon are required to form 20.0 g of xenon hexafluoride?

What is the balanced equation for this reaction? I am unsure of how to find the mass without the right equation.

Please explain.

1 Answer | Add Yours

user profile pic

jerichorayel | College Teacher | (Level 1) Senior Educator

Posted May 10, 2013 at 12:04 AM (Answer #1)

dislike 1 like

The balanced equation for the reaction can be written as:

`Xe + 3 F_2 -> XeF_6`

The balanced equation shows that one mole of xenon and three moles of fluorine gas is needed to form one mole of xenon hexafluoride. Fluorine is a diatomic molecule which normally exists as `F_2` .We can find the amount of xenon needed using stoichiometry.

`20.0 g XeF_6 * (1 mol e XeF_6)/(245.28 grams XeF_6) * (1 mol e Xe)/(1mol e XeF_6) * (131.293 grams Xe)/(1mol e Xe)`

= 10.7 grams Xe is required to form the xenon hexafluoride compound. 

Sources:

Join to answer this question

Join a community of thousands of dedicated teachers and students.

Join eNotes