Practice: Ammonia, NH3, reacts with hypochlorite ion, OCl–, to produce hydrazine, N2H4. How many grams of hydrazine are produced from 115.0 g NH3 if the reaction has a 81.5% yield?
2 NH3 + OCl– → N2H4 + Cl– + H2O
The Percent Yield determines how successful the product yield is in a chemical reaction.
Percent Yield
Concept #1: Percent Yield
Example #1: Consider the following balanced chemical reaction:
2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (l)
If a 2.6 g sample of C6H6 reacted with excess O2 to produce 1.25 g of water, what is the percent yield of water?
Practice: The reduction of iron (III) oxide creates the following reaction:
Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H2O (g)
If the above reaction only went to 75% completion, how many moles of Fe2O3 were require to produce 0.850 moles of Fe?
