How much H2O could you get if you used 8.00 moles NH3 and all of the oxygen needed. That will give you
8.00 x (6 moles H2O/4 moles NH3) = about 12.
Now how much H2O would be produced if you used 14.0 moles Oxygen and all of the NH3 needed. That will be 14.0 moles O2 x (6 moles H2O/7 moles O2) = 12
aha!. They are the same so you would get 12 moles H2O. What if they weren't the same. In that case you have a limiting reagent problem, the SMALLER value is the one you choose and the reagent producing the smaller value is the limiting reagent.
If 8.00 moles of NH3 reacted with 14.0 moles of O2, how many moles of H2O will be produced?
4NH3 (g) + 7O2 (g) --> 4NO2 + 6H2O (g)
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