Name: Chapter 9 Review

Name: Chapter 9 Review 1. Calculate the molar mass of the following: (units are grams/mole or g/mol) a. NaOH b. Na c. H2O d. H2 2. 4NH3 + 6NO  5N2 + 6H2O a. What is the mole ratio of NO to H2O? b. What is the mole ratio of N2 to NH3? c. How many moles of N2 are needed to react with 0.553 moles of NH3?

3. 2KClO3  2KCl + 3O2 How many moles of KCl form when 5.5 mol KClO3 decomposes?

4. 2Na + 2H2O  2NaOH + H2 How many grams of NaOH are produced if 20.0 g Na reacts with excess H2O?

5. Calculate percent yield if you have an actual yield of 22 g and the theoretical yield is 25 g.

6. 6.0 mol of N2 are mixed with 12.0 mol of H2 according to the following equation: N2 + 3H2  2 NH3 a. What is your limiting reactant?

b. What is the theoretical yield of NH3 in moles?

c. What is the percent yield if your actual yield is 6.4 moles of NH3?

7. 0.050 mol of Ca(OH)2 are combined with 0.080 mol of HCl according to the following equation: Ca(OH)2 + 2 HCl  CaCl2 + 2 H2O a. How many moles of HCl are required to neutralize all 0.050 mol of Ca(OH)2?

b. What is the limiting reactant in this neutralization reaction?

c. How many grams of water will form in this reaction?

d. If Mrs. Washburn formed 1.38 g of water, what was her percent yield?