What is the maximum amount of #IF_7# that can be obtained from 25.0 g fluorine in the equation #I_2 + F_2 -> IF_7#?

1 Answer
Nov 29, 2016

Answer:

You need a stoichiometric equation. You can make a mass of approx. #50*g#

Explanation:

#1/2I_2(g) + 7/2F_2(g)rarr IF_7#

I introduced the half-coefficient because it makes the arithmetic a little bit easier. I am certainly free to do so. The stoichiometry dictates that 1 equiv of diiodine reacts with 7 squiv difluorine.

#"Moles of difluorine"# #=# #(25.0*g)/(2xx19*g*mol^-1)=0.658*mol#.

Given stoichiometric iodine, we can form #2/7# equiv of the interhalogen, i.e. #2/7xx0.658*mol=0.188*mol#.

And thus a mass of #0.188*molxx259.90*g*mol^-1=??#.

It would not be my choice to do this reaction. I am too fond of my 10 fingers, and 2 eyes.