Solid xenon hexafluoride is prepared by allowing xenon gas and
fluorine gas to react.
Xe(g) + 3F2(g) - XeF6(s)
How many grams of fluorine are required to produce 10.0 g of XeF6..Please help i dont understand this at all

Question

Solid xenon hexafluoride is prepared by allowing xenon gas and
fluorine gas to react.
Xe(g) + 3F2(g) -> XeF6(s)
How many grams of fluorine are required to produce 10.0 g of XeF6..Please help i dont understand this at all

mani_jha · Answer

The equation simply tells you that 1 mole of Xe requires 3 moles of F2 gas to produce 1 mole of XeF6.
Do you know how to calculate no of moles?

anonymous · Answer

no thats what i dont get

mani_jha · Answer

The no of moles is actually equal to the mass divided by the molecular weight.
Mass of XeF6 given is 10g. Its Molecular weight is, say X. Then number of moles of XeF6 is 10/X.
Your first job is to find X.  It is the sum of the atomic weights of XeF6. The atomic weight of F is 19(Multiply that by 6). Find the atomic weight of X from the periodic table. Then add to find X.
Get it? Post as soon as you find X.