1. Stoichiometry & Percent Yield Practice 2 Al + 6 HCl  2 AlCl 3 + 3 H 2 95 g of hydrochloric acid are reacted with excess aluminum producing 2.2 g of hydrogen gas. What is the percent yield? Solution: Calculate theoretical yield: Next, calculate % yield:

2. Stoichiometry & Percent Yield Practice 2 HgO  2 Hg + O 2 42 g of mercury(II) oxide are decomposed. If the % yield is 99.0%, what mass of oxygen gas will actually be produced? Solution: Begin like you are calculating the theoretical yield: Then, multiply by the % yield:

3. Stoichiometry & Percent Yield Practice 2 Na 2 O 2 + 2 H 2 O  4 NaOH + O 2 What mass of sodium peroxide is needed to produce 19 g of oxygen gas if the % yield is 96.0%? Solution: Begin by changing the actual yield into a theoretical yield by dividing by the % yield: Then, do a typical stoichiometric calculation:

4. Stoichiometry & Percent Yield Practice 4 Al + 3 O 2  2 Al 2 O 3 16 g of aluminum are reacted with excess oxygen gas producing 29 g of aluminum oxide. What is the percent yield? Solution: Calculate theoretical yield: Next, calculate % yield:

5. Stoichiometry & Percent Yield Practice FeCl 3 + 3 NH 4 OH  3 NH 4 Cl + Fe(OH) 3 13 g of iron(III) chloride are reacted with excess ammonium hydroxide. If the % yield is 95.5%, what mass of ammonium chloride will actually be produced? Solution: Begin like you are calculating the theoretical yield: Then, multiply by the % yield:

6. Stoichiometry & Percent Yield Practice 2 Na + Cl 2  2 NaCl What mass of chlorine is needed to produce 22 g of sodium chloride if the % yield is 97.0%? Solution: Begin by changing the actual yield into a theoretical yield by dividing by the % yield: Then, do a typical stoichiometric calculation: