stoichiometry & percent yield practice 2 al + 6 hcl 2 alcl 3 + 3 h 2
DESCRIPTION
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:. - PowerPoint PPT PresentationTRANSCRIPT
Stoichiometry & Percent Yield Practice2 Al + 6 HCl 2 AlCl3 + 3 H2
95 g of hydrochloric acid are reacted with excess aluminum producing 2.2 g of hydrogen gas. What is the percent yield?
Solution:
23 mol H6 mol HCl
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
1 mol HCl95 g HCl36.46 g HCl⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2
2
2.016 g H1 mol H
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2= 2.6 g H
Calculate theoretical yield:
Next, calculate % yield:
Stoichiometry & Percent Yield Practice2 HgO 2 Hg + O2
42 g of mercury(II) oxide are decomposed. If the % yield is 99.0%, what mass of oxygen gas will actually be produced?
Solution:
21 mol O2 mol HgO
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
1 mol HgO42 g HgO216.59 g HgO⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2
2
32.00 g O1 mol O
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
Begin like you are calculating the theoretical yield:
Then, multiply by the % yield:
99100⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠ 2= 3.1 g O
Stoichiometry & Percent Yield Practice2 Na2O2 + 2 H2O 4 NaOH + O2
What mass of sodium peroxide is needed to produce 19 g of oxygen gas if the % yield is 96.0%?
Solution:
2
2
1 mol O32.00 g O
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
210019 g O96
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2 2
2
2 mol Na O1 mol O
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
Begin by changing the actual yield into a theoretical yield by dividing by the % yield:
Then, do a typical stoichiometric calculation:
2 2
2 2
77.98 g Na O1 mol Na O
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2 2= 96 g Na O
Stoichiometry & Percent Yield Practice4 Al + 3 O2 2 Al2O3
16 g of aluminum are reacted with excess oxygen gas producing 29 g of aluminum oxide. What is the percent yield?
Solution:
2 32 mol Al O4 mol Al
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
1 mol Al16 g Al26.98 g Al⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2 3
2 3
101.96 g Al O1 mol Al O
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2 3= 30. g Al O
Calculate theoretical yield:
Next, calculate % yield:
2 3
2 3
29 g Al Oactual%Yield = ?100 = ?100 = 96.7 % Yieldtheoretical 30. g Al O
Stoichiometry & Percent Yield PracticeFeCl3 + 3 NH4OH 3 NH4Cl + 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:
4
3
3 mol NH Cl1 mol FeCl
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
33
3
1 mol FeCl13 g FeCl
162.2 g FeCl
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
4
4
53.49 g NH Cl1 mol NH Cl
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
Begin like you are calculating the theoretical yield:
Then, multiply by the % yield:
95.5100
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
4NH Cl= 12 g
Stoichiometry & Percent Yield Practice2 Na + Cl2 2 NaCl
What mass of chlorine is needed to produce 22 g of sodium chloride if the % yield is 97.0%?
Solution:
1 mol NaCl58.44 g NaCl⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
210022 g O97
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
21 mol Cl2 mol NaCl
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
Begin by changing the actual yield into a theoretical yield by dividing by the % yield:
Then, do a typical stoichiometric calculation:
2
2
70.91 g Cl1 mol Cl
⎛ ⎞⎜ ⎟⎜ ⎟⎝ ⎠
2= 14 g Cl