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
anor277
Nov 29, 2016

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.

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