1. Chapter 3 Review

2. Old Stuff…
Review Gold Foil and Cathode Ray Tube experiments.

3. Old Stuff… Write the chemical formula for: Potassium oxide
Diphosphorous pentaoxide
Nickel (III) chloride

4. Basic Stoichiometry
According to the reaction below, how many grams of Na are needed to displace 3.25 mol of H2 gas? (answer = 149g)
2Na + 2H2O → H NaOH

5. Basic Stoichiometry
How many moles of Na are needed to produce 8 moles of NaOH if the reaction vessel contains 12 moles of water? (answer = 8 mol)
2Na + 2H2O → H NaOH

6. Basic Stoichiometry
How many moles of water are produced when 83 g of H2 react with an excess of oxygen? (answer = 41.5 mol)
2 H2 + O2 → 2H2O

7. Empirical Formula
What is the empirical formula of a compound that contains 0.36 mol of potassium, 0.12 mol of phosphorous, and 0.48 mol of oxygen? (answer = K3PO4)

8. Empirical Formula
A compound is found to contain 94.12% oxygen by mass and 5.88% H by mass. What is the empirical formula for the compound? (answer = OH)

9. Empirical Formula
A gram sample of a compound containing only carbon, hydrogen and oxygen is burned in excess oxygen gas g of carbon dioxide and g of water were produced. Find the empirical formula. (answer = C21H30O2)

10. Continued
Find the molecular formula for this compound if the molar mass is known to be g/mol. (answer = C42H60O4)

11. % Abundance
Chlorine has an average atomic mass of amu. The only two naturally occurring isotopes of chlorine are Cl-35 ( amu) and Cl-37 ( amu). What is the percent abundance of each isotope of chlorine? (Answer = Cl % and Cl %)

12. Limiting Reactant
A 56.8g sample of sodium chloride reacts with 27.3g of fluorine gas according to the following equation:
2NaCl + F NaF + Cl2
What is the limiting reactant?
Answer = NaCl
Determine the maximum mass of NaF that can be produced in this reaction.
Answer = 40.81g
If the actual yield is found to be 18.2g of NaF what is the percent yield?
Answer = 44.6%