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Solution:. Stoichiometry & Percent Yield Practice 2 Al + 6 HCl 2 AlCl 3 + 3 H 2. Calculate theoretical yield:. 95 g of hydrochloric acid are reacted with excess aluminum producing 2.2 g of hydrogen gas. What is the percent yield?. Next, calculate % yield:. Solution:.
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Solution: Stoichiometry & Percent Yield Practice2 Al + 6 HCl 2 AlCl3 + 3 H2 Calculate theoretical yield: 95 g of hydrochloric acid are reacted with excess aluminum producing 2.2 g of hydrogen gas. What is the percent yield? Next, calculate % yield:
Solution: Stoichiometry & Percent Yield Practice2 HgO 2 Hg + O2 Begin like you are calculating the theoretical yield: 42 g of mercury(II) oxide are decomposed. If the % yield is 99.0%, what mass of oxygen gas will actually be produced? Then, multiply by the % yield:
Solution: Stoichiometry & Percent Yield Practice2 Na2O2 + 2 H2O 4 NaOH + O2 Begin by changing the actual yield into a theoretical yield by dividing by the % yield: What mass of sodium peroxide is needed to produce 19 g of oxygen gas if the % yield is 96.0%? Then, do a typical stoichiometric calculation:
Solution: Stoichiometry & Percent Yield Practice4 Al + 3 O2 2 Al2O3 Calculate theoretical yield: 16 g of aluminum are reacted with excess oxygen gas producing 29 g of aluminum oxide. What is the percent yield? Next, calculate % yield:
Solution: Stoichiometry & Percent Yield PracticeFeCl3 + 3 NH4OH 3 NH4Cl + Fe(OH)3 Begin like you are calculating the theoretical yield: 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? Then, multiply by the % yield:
Solution: Stoichiometry & Percent Yield Practice2 Na + Cl2 2 NaCl Begin by changing the actual yield into a theoretical yield by dividing by the % yield: What mass of chlorine is needed to produce 22 g of sodium chloride if the % yield is 97.0%? Then, do a typical stoichiometric calculation:
