1. If you are traveling at 65 mi/h how long will it take to travel 112 km? If your car gets 28 miles per gallon how many liters of gas will it take to travel the 112 km? Dimensional Analysis

2. Density What is the mass of a piece of gold with a Volume of 1.0 L? The density of gold is 19.32 g/cm 3

3. Kinetic Molecular Theory for an Ideal Gas 1.The particles are so small compared to the distances between them that the volume of the particles can be assumed to be negligible. (i.e. Particles have no volume) 2.Particles are in constant random motion. The collisions of the particles with the walls of the containers are the cause of the pressure exerted by the gas. 3.Particles are assumed to exert no forces on each other. They neither attract nor repel each other. 4.The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas. (KE avg = (3/2)RT

4. What is the effect on the volume of one mole of an ideal gas if the pressure is doubled and the Kelvin temperature is halved?

5. Dalton’s Law of Partial Pressures A sample of KClO 3 (s) is decomposed by heating it in a test tube. The oxygen gas produced is collected over water at 22 °C and a total pressure of 754 torr. The volume of the gas collected is 0.650 L and the vapor pressure of water at 22 °C is 21 torr. Calculate the number of moles of oxygen collected. Also see ch. 5 # 67, 68, 103

6. 0.30 g of a gas occupied a volume of 82.0 mL at 3.00 atm and 27 °C. Calculate the molar mass of the gas.

7. Calculate the density of SF 6 at 1.0 atm and 0.0 °C.

8. At 0 °C and 1.0 atm, 1.0 L of Br 2 reacts completely (i.e. exactly) with 3.0 L of F 2 producing 2.0 L of a product. What is the formula of the product?

9. Lung capacity for a typical person is 2.0 L. If air at 20.0 °C and 1.0 atm fills the lungs, how many molecules of air are present?

10. An atomic bomb needs 4.0 moles of Uranium. How many grams of U are needed? Atoms?

11. Determine mass % Al and O in aluminum oxide.

12. A certain gas contains 81.10% boron and 18.90 % hydrogen by mass. The molar mass of the gas is 53.4 g/mol. Determine the empirical formula and molecular formula of the gas.

13. Glucose contains only C, H and O. When 1.00 g of glucose is combusted it yields 1.47 g of CO 2 and 0.600 g of H 2 O. Glucose has a molar mass of 180.16 g/mol. What is The molecular formula of glucose? What is the mass % of C, H, and O?

14. Stoichiometry – using a balanced chemical Equation to determine how much reactant or product is consumed or produced in a chemical reaction.

15. C 12 H 22 O 11 + H 2 O 2  H 2 O + CO 2

16. How many grams of CO 2 are produced from The combustion, in air, of 10.00 mL of benzene (C 6 H 6 )? The density of benzene is 0.879 g/mL

17. 3 A + B  C + 2 D If 4.0 mol of A are reacted with 2.0 mol of B What is the limiting reactant? How many Moles of C and D can be produced?

18. Fe 2 O 3 (s) + CO(g)  Fe(s) + CO 2 (g) If 2.0 kg of Fe 2 O 3 and 1.5 kg of CO are reacted what is the maximum amount of iron that could be produced? If the actual yield of iron is 650 g what is the percent yield?

19. Solubility Rules 1.Most nitrate salts are soluble. 2.Most salts of alkali metals and ammonium cations are soluble. 3.Most chloride, bromide, and iodide salts are soluble. Exceptions: salts containing Ag +, Pb 2+, and Hg 2 2+ ions are insoluble. 4.Most sulfate salts are soluble. Exceptions: salts containing Ca 2+, Ba 2+, Pb 2+, and Hg 2 2+ ions are insoluble. 5.Most hydroxide salts are insoluble. Exceptions: hydroxides containing alkali metals, Ba 2+, Sr 2+ and Ca 2+ ions are soluble. 6.Most sulfide, carbonate, chromate, and phosphate salts are insoluble. Exceptions: salts of alkali metals and ammonium cations are soluble.

20. How many moles of ions are present in a 2.0 L solution of 1.0 M Ca(OH) 2 ?

21. How much H 2 O is needed to dilute 5.0 L of a 2.0 M solution of NaCl to 0.50 M?

22. A 0.6025 g sample of a compound containing chloride ion was dissolved in H 2 O and the chloride precipitated by adding excess silver nitrate. The precipitant of silver chloride was found to weigh 0.7134 g. Calculate the mass % of chloride in the sample.

23. What volume of 0.050 M sodium phosphate Solution is needed to react completely with 30.0 mL of 0.10 M silver nitrate?

24. What mass of precipitant would form from 30.0 mL of 0.10 M AgNO 3 using excess Na 3 PO 4 solution?

25. What volume of 0.200 M HCl is needed to titrate 20.0 mL of 0.350 M NaOH?

26. When titrating 0.150 M HCl with a calcium hydroxide solution of an unknown concentration, 25.0 mL of the base are required to neutralize 35.0 mL of the acid. Calculate the molarity of the base.

27. A chemist dissolves 0.300 g of an unknown monoprotic acid in a convenient volume of water. She finds that 14.60 mL of 0.426 M sodium hydroxide are required to neutralize the acid. What is the molar mass of the acid?