CHM 1046

Review Test 2

1. Terminology: State functions (examples), system, surroundings, exothermic, endothermic process, spontaneous process, enthalpy, entropy, free energy, rates of reaction, reaction mechanisms, catalysts, etc.

2. Thermo
1. DE =q + w and 1st Law of thermo-  watch out for signs of q and w
2. DE =DH +DnRT (= DH +PDV) Start with a balanced reaction!  Dn applies to gases only
3. DH Hess' law calculations: (2 ways) Hess' Law of summation using tables and adding thermochemical reactions.
4. Use Bond Energy values and calculate  DH or viceversa
5. Second Law and Third Law of thermo:
6. DS: meaning of entropy, signs (+ = more disorder; - =more order) and calculations of DS using tables
7. DG meaning of spontaneous reaction, signs for spontaneous or non spontaneous reactions, reactions at equilibrium, calculations of DG using tables  and 
8. DG=DH-TDS (watch your units when you use this equation!!!) and find temperature range for spontaneous reactions to occur.

3. Kinetics

a. Rate expressions in an overall reaction as a function of reactants and products

b. Graphs of Energy vs reaction coordinates; Energy of Activation (forward and reverse reactions) 

c. Collision theory: Transition State, effective and ineffective collision, bimolecular collisions, termolecular collisions

d. Variables that affect the rate of a reaction, temperature, concentration, catalyst, etc

e. Effect of a Catalyst

f. Calculations of the rate law expression, order of each reactant and kinetics rate constant (watch out for the units of k)

g. Meaning of first order, second order, overall order

h. INTEGRATED Rate equation and half life

i. Reaction mechanisms: meaning of intermediates, RDS=slow step; coefficients in the RDS equal the orders of reactants in the rate law,  (never the coefficients of the balanced reaction are taken as the order)

k. Arrhenius Equation and temperature dependency on the rate.

STUDY HARD and Have a Good Night sleep before your test!!!