| 1010 - Efficiency & Spontaneity |
| 1010 - Recognize energy is neither created nor destroyed (its conversved). FIRST LAW |
| 1020 - Know some energy liberated from a chemical reaction will be lost to surroundings (as heat). |
| 1030 - Know any energy transfer has some inefficiency (heat loss). |
| 1040 - Define spontaneity and identify processes that are either spontaneous or non-spontaneous. |
| 1050 - Recognize spontaneity is controlled by thermodynamics while speed is a result of kinetics. |
| 1020 - Distributing Energy |
| 1010 - Recognize exothermic processes are often, but not always, spontaneous. |
| 1020 - Define entropy. Know Boltzmanns equation ( S = kb ln w ) and constank (kb = R/Na = 1.38 x10^-23 J/K). |
| 1030 - Understand the difference between macrostates and microstates. |
| 1040 - Recognize states with more equivalent microstates are entropically favored. |
| 1050 - Predict and explain the sign of ΔS of a phase change or other common processes. |
| 1030 - Heat Transfer |
| 1010 - Understand a loss of heat from a system is a gain in entropy for its surroundings. |
| 1020 - Know entropy of an isolated system never decreases. SECOND LAW |
| 1030 - Because the univserse is an isolated system, its entropy can only increase. |
| 1040 - Know a net increase in the entropy of the universe is the driving force for spontaneity. |
| 1050 - Know temperature (T) relates a systems enthalpy change (q) to the entropy change (ΔS) of its surroundings. |
| 1060 - Explain why temperature relates q_sys to ΔSsurr. |