AP Chemistry
Chapter 16/17 Outline 7th ed.
________________________________
Name
Chapter 16:___________________________________________________
16.1_____________________________________
1. spontaneous processes2. entropy(S)3. positional probability*Study sample exercise 16.1 and do text exercise 16.23:
*Study sample exercise 16.2 and do text exercise 16.24:
16.2_____________________________________
1. Second Law of Thermodynamics2. Suniv 3. Ssys 4. Ssurr 5. +Suniv 6. Suniv 7. zeroSuniv -
16.3__________________________________________.......READ CAREFULLY!
1. What factor determines whether or not an endothermic process will be spontaneous?
2. Ssurr 3. Ssurr -
16.4____________________
1. free energy2. for a process at constant temperature and pressure, G =
3. Circle one: a process is spontaneous in the direction in which the free energy
(decreases/increases).
4. Summarize table 16.5 on page 761:
*Study sample exercise 16.5 and do text exercise 16.31:
16.5_________________________________________
*Study sample exercise 16.6 and do text exercise 16.34
1. Third Law of Thermodynamics
2. Sreaction =
*Study sample exercises 16.7 and 16.8 and do text exercise 16.38:
16.6__________________________________________
1.
Standard free energy change-
2. Why is it useful to know G for a given chemical rxn?
*Study sample exercise 16.9 and do text exercise 16.46:
*Study sample exercise 16.10 and do text exercise 16.52:
3.
Standard free energy of formation (Gf)-
*Study sample exercise 16.11 and do text exercise 16.54:
*Study sample exercise 16.12 and do text exercise 16.56:
16.7__________________________________________
*Note the derivation of the following equation in section 16.7:
G = G + RTLN(Q)
From equilibrium the reaction quotient (Q) = [C]c [D]d / [A]a [B]b , where aA + bB  cC + dD
1. G 2. G -
3. Summarize (100 words minimum) the last portion of section 16.7, “the meaning of G for a
reaction” :
16.8___________________________________
1. Equilibrium position2. Equilibrium point*Study section 16.8 carefully and note the derivation of the following equation:
G = RTLN(K)
Where at equilibrium the reaction quotient (Q) = K and G = 0
3. Summarize the information in table 16.6 on page 775:
*Study sample exercises 16.14 and 16.15 and do text exercise 16.62:
16.9___________________________________
1. reversible process-
2. irreversible process3. The first two laws of thermodynamics have been paraphrased in this section of the text as; “you
can’t win, you can only break even”, and “you can’t break even”. What do these statements
mean, how would you interpret them?
Chapter 17:________________________________
17.1___________________________________
1. redox reaction2. reducing agent3. oxidizing agent4. salt bridge5. galvanic cell6. anode7. cathode8. cell potential9. volt-
17.2___________________________________
1. standard hydrogen electrode-
2. standard reduction potentials*Study sample exercise 17.1 and do text exercise 17.26 and 17.28:
*Study sample exercise 17.2 and do text exercises 17.30:
17.3___________________________________
1. Why is the work predicted from the flow of electrical current always more than measured?
2. w = qE =
3. faraday*Note the derivation of the following equation is section 17.3:
G = nFE
3. What does “n” represent in the equation above?
4. How does Ecell relate to G?
17.4___________________________________
1. concentration cell-
2. What is a “dead” battery?
*Study sample exercise 17.7 and do text exercises 17.56 and 17.58:
3. glass electrode4. ion-selective electrode-
17.5___________________________________
1. battery2. lead storage battery3. dry cell battery-
4. alkaline battery5. nickel-cadmium battery6. fuel cell-
17.6___________________________________
1. corrosion-
2. Why is the corrosion of most metals spontaneous?
3. According to the thermodynamics of the oxidation of aluminum, a jumbo jet could dissolve in a
rainstorm. Why doesn’t it?
4. Summarize the processes involved in the corrosion of iron:
5. galvanizing6. cathodic protection-
17.7___________________________________
1. electrolytic cell-
2. electrolysis3. ampere*Study sample exercise 17.9 and do text exercise 17.80:
17.8___________________________________
1. Briefly describe the Hall-Heroult process-
2. Briefly describe the process of electrorefining-
3. Briefly describe the process of metal plating-
4. Down’s cell-
5. mercury cell-
6. chlor-alkali process-
7. A copper penny can be dissolved in nitric acid but not in hydrochloric acid. Using reduction
potentials from the text or reference tables, show why this is so. What are the products of this
reaction?