1. Balance the equation

___P2O2 + ___H2O —> __H3PO4

A) If 82.6 g of P2O5 reacts with 26.6 g of water, determine the theoretical yield phosphoric acid using the following steps: (Convert mass to moles for the reactants^^)

2. Determine the limiting reactant

3. Determine the mass of phosphoric acid (H3PO4) produced (the theoretical yield).

4. If the actual yield of H3PO4 was 80.6 g, determine the percent yield.

Limiting Reagent and Percent Yield Practice In a chemical reaction with more than one reactant, the limiting reagent is the reactant that is consumed first. This causes the reaction to stop. The other reagent is called the excess reagent. The theoretical vield is determined by the limiting reagent Percent yield is the actual yield divided by the theoretical yield, then convert to % by multiplying by 100 1. 35.6 g of Al is reacted with 99.3 g of iron(II) oxide to produce 66.28 g of iron according to the reaction below. Calculate the percent yield for this reaction. a) Balance the equation. b) Determine the moles of product (Fe for this reaction) made by both reagents. c) Whichever reagent produced fewer moles of product is the limiting reactant. What is the limiting reagent for this reaction? d) Calculate the theoretical yield in grams from the limiting reactant. e) Using your theoretical yield from c and the actual yield, determine the percent yield. 93