Chapter 3 Review

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

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

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 → H2 + 2NaOH

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 → H2 + 2NaOH

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

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)

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)

Empirical Formula A 1.0857 gram sample of a compound containing only carbon, hydrogen and oxygen is burned in excess oxygen gas. 3.190g of carbon dioxide and 0.9360g of water were produced. Find the empirical formula. (answer = C21H30O2)

Continued Find the molecular formula for this compound if the molar mass is known to be 628.1 g/mol. (answer = C42H60O4)

% Abundance Chlorine has an average atomic mass of 35.453 amu. The only two naturally occurring isotopes of chlorine are Cl-35 (34.969 amu) and Cl-37 (36.956 amu). What is the percent abundance of each isotope of chlorine? (Answer = Cl-35 75.6% and Cl-37 24.4%)

Limiting Reactant A 56.8g sample of sodium chloride reacts with 27.3g of fluorine gas according to the following equation: 2NaCl + F2 2NaF + 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%