2.1. 1st Law of Thermodynamics

Lecture on the first law of thermodynamics and its applications in ideal gas processes and thermochemistry.

Outline:

0:32 INTRODUCTION: Definition of Thermodynamics
2:33 System and Surroundings
4:16 Extensive vs. Intensive Properties
7:14 Definition of energy
16:34 Statement of the First Law of Thermodynamics
17:19 State vs. Non-state functions

23:49 Work: pressure-volume work, example of work as isothermal irreversible and reversible PV work
54:14 Heat
56:16 Heat Capacity

1:12:30 IDEAL GAS PROCESSES
1:13:19 Isochoric Process
1:17:37 Isobaric Process
1:25:35 Definition of Enthalpy
1:29:55 Cp vs Cv
1:31:43 Cp and Cv of monatomic and diatomic gases
1:35:14 Isothermal Process: irreversible and reversible
1:44:31 Adiabatic Process: irreversible and reversible
2:12:04 Summary of Ideal Gas Processes

2:29:52 THERMOCHEMSITRY
2:33:30 Relationship between enthalpy and internal energy
2:38:14 Calorimetry
2:44:54 Hess's Law
2:51:13 Temperature Dependence of Enthalpy Changes: Phase Changes, Chemical Changes and Kirchoff's Rule

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[kylecatman]

At 2:23:49 there is no work being done so U = Q and they should be equal, you only use enthalpy if there's boundary or flow work. Remember that H = U + PdV, and there's no PdV here. -12, 471 Joules is the final answer.

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