00:03
Hi there.
00:04
In this question, we are given this equation, and if we check, it is already balanced, there's one cesium on each side, there are seven fluorine on each side, and one xenon on each side.
00:15
I've omitted the states of matter because those are not necessary for what we're doing.
00:18
What we're doing is using this equation to give us the mole ratio.
00:22
In other words, the ratio in which the reactants react and the products are formed.
00:27
And we give this from the coefficients in a balanced equation.
00:30
Well, since no coefficients were needed, that means it's understood that each of these is a one.
00:36
So what that tells us is that for every mole of cesium fluoride, we need one mole of the xef6, the xenon hexafluoride.
00:51
And in turn, this is going to produce one mole of the product.
00:57
Okay, so what we notice, or what we're given in the problem, rather, is that we are reacting 14 .0.
01:06
Moles of the csf with 14 .0 moles of the xef6...