1. Applied General Chemistry

2. Temperature (T): Kelvin. 0 F, R. 0 C Volume (V): Liters, m3, Lt/mol # of Molecules (n): mole Pressure (P): kPa, Pa, bars, psi, mmHg, atm, torr Density (p): lb/litre

3. Pressure:Conversions: Pa1 atm = 760 mm Hg torr1 torr = 1 mm Hg mm of Hg1 bar = 1 x 10 5 Pa atm1 atm = 101,325 Pa bar STP-Standard Temperature & Pressure: 1 atm & 25 o C T= 273K, P= 101.3 kPa, V= 22.4 L/mol

4. Boyle’s Law: P 1 V 1 = P 2 V 2 (T, n constant) Charles’ Law: V 1 /T 1 = V 2 /T 2 (P, n constant) Combined Gas Law: PV = nRT or P 1 V 1/ T 1 = P 2 V 2/ T 2

5. 1.00 L of a gas at standard temperature and pressure is compressed to 0.473 mL. What is the new pressure of the gas?

6. If we assume that T does not change, i.e constant. If this is true, then P1V1 = P2V2 (Boyle's Law) P1 = 1 atm (standard pressure) V1 = 1 L P2 = ? V2 =.473L P2 = 2.11 atm

7. The temperature inside my refrigerator is about 4 0 Celsius. If I place a balloon in my fridge that initially has a temperature of 22 0 C and a volume of 0.5 liters, what will be the volume of the balloon when it is fully cooled by my refrigerator?

8. Since P does not change, it is constant; V1 / T1 = V2 / T2 (Charles’s Law) 0.5 L / (273.15 + 22) = V2 / (273.15 + 4) [0.5 L / 295.15] * 277.15 = V2 V2 = 0.47 L

9. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas?

10. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? PV=nRT or P 1 V 1/ T 1 = P 2 V 2/ T 2 plug in initial conditions in one side and final in the other. if the value is not mentioned assume it is constant. (12atm x 23Lt)/ 200 K = (14atm x V2)/ 300 K 29.5 Lt

11. Calculate the number of moles in a deep breath of air whose volume is 2.50 L at body temperature, 37 o C, and a pressure of 735 torr.

12. PV = nRT R = 0.0821 L * atm / mol * K (ideal gas constant) First, convert 735 torr to atm; Divide by 760. (1 atm = 760 torr) 735 torr * 1 atm / 760 torr = 0.967 atm Then, convert 37 C to Kelvin. Just add 273. 37 C = 310K Derive the formula for n to solve the number of moles. n = PV / RT = (0.967)(2.50) / (0.0821)(310) = 0.095 mol

16. 1. Elements 2. Periodic Table 3. Dalton’s Atomic Theory 4. Compound Formula 5. Structure of an Atom 6. Modern Concept of Atomic Structure

19. 1. Identify the parts of the Periodic Table a. Element name & symbol b. Periods c. Groups (family) d. Metal, Metalloid, & Non-metal

20. 1c. Groups (family) i. Alkali Metal ii. Alkaline Earth iii. Halogens iv. Noble (Inert) Gases v. Transition Metals vi. Lanthanides vii. Actinides

21.  Alkali Metal:

22.  Alkaline Earth Metal:

23.  Halogens

24.  Inert (Noble) Gases

25.  Transition Metals

26.  Lanthanides

27.  Actinides

31.  Law of Conservation of Mass (matter): Mass is neither created nor destroyed in chemical reactions.

32.  Law of Definite Proportions: Different samples of a pure chemical substance always contain the same proportion of elements by mass.

33. The raw materials (reactants) are placed on the left side. As the reactants are mixed together, they yield predictable products. Products are placed on the right side of the equation. C + O 2 = CO 2 (reactants) (products) 1 Carbon = 1 Carbon 2 Oxygen = 2 Oxygen

34. Rule of thumb: ‘What goes in must come out’… H 3 PO 4 + 3NaOH = Na 3 PO 4 +3H 2 O 18 tons 10 tons (28 total tons) If you change H 3 PO 4 to 1800 tons; What must the (3NaOH) weight be to balance the equations?

35.  Technicians use this method to determine the exact amount of reactants needed to produce the specific products. Proper proportions avoids waste. Determine weight of each molecule Ensure reactant total weight is equal to product total weight Determine relative numbers of reactant atoms or ions Example: List the reactant elements. Is this equation balanced? H 3 PO 4 = H 2 O + H 4 P 2 O 38

36. Exothermic: heat released Endothermic: Energy is absorbed Replacement: removes +ions and – ions Neutralization: removes hydrogen ions (acid) or hydroxyl ions (base) from a liquid. Combustion: Exothermic reactions that require fuel, oxygen and and heat to occur.

37. Mixtures and Solutions A mixture is composed of two or more substances that are only mixed physically (not chemically combined) and can be separated through a physical means such as boiling.

38.  A chemical compound that contains H and C such as crude oil. The simplest is called ‘methane’ or natural gas, it has 1 carbon atom and 4 hydrogen atoms.  Each carbon atom has 4 bonds (valence electrons) with which it attaches to the hydrogen bonds. These bonds must be filled for it to be stable.  Chemists have divided these hydrocarbons into 2 large families: alkanes and olefins

39. Alkanesmolecular Formula molecular WeightBoiling Point (C) MethaneCH416-164 EthaneC2H630-89 PropaneC3H844-42 ButaneC4H1058-0.5 PentaneC5H127236 HexaneC6H148669 HeptaneC7H1610098 OctaneC8H18114126 NonaneC9H20128151 DecaneC10H22142174

42.  Distillation: Separation of various fractions of a mixture by their individual boiling points.

43.  The process of changing (breaking) long chain hydrocarbons into short chain hydrocarbons which are more useful. A barrel of oil produces ~20% gasoline. Cracking increases the yield by up to 50% by splitting the kerosene and heating oil fractions of the crude.