1. Honors Stoichiometry Examples

2. Example 1 What mass of carbon dioxide in grams is needed to react with 3.00mol of H 2 O in the following photosynthetic reaction? 6CO 2 + 6HOH  C 6 H 12 O 6 +6O 2

3. Answer 132g CO 2

4. Example 2 The disinfectant hydrogen peroxide H 2 O 2 decomposes to form water and oxygen gas. How many moles of oxygen will result from the decomposition of 5.0 mol of hydrogen peroxide?

5. Answer 2.5mol O 2

6. Example 3 When sodium azide is activated in an automobile airbag, nitrogen gas and sodium are produced according to the equation: 2NaN 3  2Na + 3N 2 If 0.500mol of NaN 3 react what mass in grams of nitrogen would result?

7. Answer 21.0gN 2

8. Percent Yield Actual yield x 100 = % yield Actual yield x 100 = % yield theoretical yield theoretical yield

9. Example 4 In a certain experiment, the expected yield is 1.352g. The actual yield was 1.279g. Determine the percent yield. In a certain experiment, the expected yield is 1.352g. The actual yield was 1.279g. Determine the percent yield.

10. Answer 94.60%

11. Example 5 How many moles of mercury (II) oxide are needed to produce 125g of oxygen and mercury?

12. Answer 7.81mol HgO

13. Example 6 When magnesium burns in air, it combines with oxygen to form magnesium oxide according to the following equation. 2Mg+O 2  2MgO What mass in grams of magnesium oxide is produced from 2.00mol of magnesium?

14. Answer 80.0g MgO

15. Example 7 Ammonia is widely used as a fertilizer and in many household cleaners. How many moles of ammonia are produced when 6 mol of hydrogen gas react with excess nitrogen gas?

16. Answers 4 mol

17. Example 8 Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO+2H 2  CH 3 OH If 75.0g of CO reacts to produce 68.4g CH 3 OH, what is the percent yield of CH 3 OH?

18. Answer 79.8%