00:03
This is a limiting reactant problem, which you know because you were given the masses of each of the reactants.
00:10
This way we don't know which reactants is going to run out first, and we need to determine that before we can find how much product is made.
00:17
In order to make this comparison, we need moles of each reactants.
00:21
So we're going to divide through by the molar mass first.
00:25
For c2h4, we're going to divide by 28 .05 grams in every one mole of c2h4.
00:36
This is equal to 0 .549 moles of this reactants.
00:44
Same process for cl2, but here the molar mass is 70 .91 grams in every one mole.
00:54
This is equal to 0 .0527 moles.
01:02
Notice that these are reacting with 1 to 1 mole ratios, so you need equal number of moles of each.
01:08
You can see that you have a lot fewer moles of chlorine gas.
01:17
So this 0 .0527 moles of co2 need by the multiple -mole ratio, 0 .052 to 7 moles of c2h4...