[Tbridwell]

I'm working on an online lab for my college chem class and am wondering why I am wrong on a certain stoichiometry problem.

Here's the balanced equation:
4 NH3 + 5 02 --> 4 NO + 6H2O

I'm given 7 moles O2 and 6 moles NH3.

The actual question: If 6.0 mol NH3 react with 7.0 mol O2, how many moles of reactions can be completed?

I know O2 is the limiting reactant, here's my work.

7 mol O2 x 4 mol NO / 5 mol O2 = 5.6 mol NO

7 mol O2 x 5 mol H2O / 5 mol O2 = 8.4 mol H2O

5.6 + 8.4 = 14, however the page says 14 is not the correct answer. I tried 5.6 and 8.4 to see if the question was actually asking for one of the individual reactant values, but neither were correct. Can someone help me find where I'm going wrong? I'd appreciate it. Apologies for any mistakes in the way I'm posting, this is my first time here.

[Borek]

"One mole of a reaction" typically means "reaction as written" - so I would expect it to mean here "how many portions of 4 moles of ammonia (or 5 moles of oxygen) reacted".

Concept of "moles of reaction" is not that important in stoichiometry, but it becomes an important convention in thermodynamics.