Question

Given the chemical equation, Cl2 + F2 2ClF, how many moles of ClF are produced in the reaction, if 1.50 moles Cl2 are made to react with 1.75 moles F2 ?

I got the answer 3.50 moles but it was wrong. Can anyone help me please.

Answer 1

Cl2 + F2 -> 2ClF

Answer 2

You only have 1.50 mol of Cl2 so you are only going to get 3.00 mol of ClF

You have 0.25 mol of excess F2 left over.

Answer 3

Sorry but I still don't understand your explaining. Can you explain more briefly please. Thanks.

Answer 4

This is a limiting reagent problem (LR) and you know that because amounts are given for BOTH reactants.
Your 1.50 mols Cl2 will produce 2*1.50 = 3.00 mols ClF if all of the Cl2 reacts and you have an excess of F2.
Your 1.75 mols F2 will produce 2*1.75 = 3.50 mols ClF if you use all of the F2 and have an excess of Cl2. But you don't have an excess of Cl2. You have ONLY 1.50 mols so the yield is determined by the one that will produce the LEAST product. That is Cl2. You can get 3.00 mols ClF and you will have some F2 left over as Damon suggested.

Answer 5

Thanks both of your replied. I got it now :)