1.  What is the formula for finding heat?  What are the two units of heat?  The temperature of a sample of iron with a mass of 10.0 g changed from 50.4 o C to 25.0 o C. If the specific heat of iron is 0.449 J/g x o C, how much heat was released?  A 4.50 g nugget of pure gold absorbed 276 J of heat. What was the final temperature of the gold if the initial temperature was 25 o C? The specific heat of gold is 0.129 J/(g x o C).

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3.  Calorimeter  Uses insulated material to measure heat absorbed or released.  Usually has water in it  Can determine specific heats  Whatever heat is gained by the water, it is lost by the substance in the water

4.  Thermochemistry- study of heat changes that accompany chemical reactions and phase changes  Two parts are changing in a reaction  system and surroundings  Universe = system + surroundings  Ex. Hand warmers  If exothermic, heat is a product  If endothermic, heat is a reactant

5.  the heat content of a system at constant pressure  Cant actually measure the actual energy or enthalpy of a substance but you can measure change  ΔH rxn = H products – H reactants  Exothermic = negative (released to the surroundings)  Endothermic (absorbed by the system) = postive  Written: 4Fe + 3O 2  2Fe 2 O 3 + 1625 kJ  4Fe + 3O 2  2Fe 2 O 3 ΔH rxn = -1625 kJ  q= ΔH rxn

6.  Can not just rely on exo and endo to tell  Ex. CH 4 +2O 2  CO 2 + H 2 O ΔH rxn = -891 kJ  Molecules would rather exists in a high state of disorder (called entropy)  Second law of thermodynamics  entropy in spontaneous process will always increase  Entropy = ΔS (products – reactants)  If entropy increases, ΔS is positive  Ex. Water changing from solid to liquid to gas  Ex. Decrease in temperature

7.  Can use the Gibbs free energy equation to determine if a reaction will be spontaneous  ΔG system = ΔH system – TΔS system  Temp in Kelvin, H in Joules  If G is negative- reaction is spontaneous  If G is positive- reaction is nonspontaneous  Ex. For a process, ΔH sys = 145 kJ and ΔS sys = 322 J/K. Is the process spontaneous at 382 K?

8.  Determine if the following process is spontaneous or nonspontaneous:  ΔH sys = -75.9 kJ, T = 273 K, ΔS sys = 138 J/K  Is it an endothermic reaction or exothermic?

9.  Atoms, ions, and molecules must collide in order to react  Only a small fraction of particles actually collide  Must collide in the correct orientation  Once they collide, they make an intermediate molecule called an activated complex  exist in the transition state  Must also have the right amount of energy (called activation energy)  If a reaction has a high E a, few collision  low E a, high collisions

10.  Exothermic- molecules collide with enough energy to overcome the E a and produce products at a lower energy level  Endothermic- reactants lie at a low energy level and must absorb energy to overcome the E a.