Chapter 10: Energy Changes in Chemical Reactions | Lecture 3 of 8
General Chemistry: The Complete College Lecture Series
This chapter covers energy and thermodynamics, the first law, heat and work, enthalpy, calorimetry, Hess’s law, standard enthalpies of formation, bond enthalpies, and the Born-Haber cycle and lattice energy.
Part 3 of Chapter 10 introduces enthalpy, the heat content of a system, and shows why chemists use delta H instead of internal energy for reactions run at constant pressure. Starting from delta U = q + w, Dr. Kunapareddy derives delta H = delta U + P delta V and shows that at constant pressure delta H equals the heat q. The lecture connects the sign of delta H to endothermic and exothermic processes, reads thermochemical equations (such as ice melting and methane combustion), and states the rules for enthalpy: it is an extensive property, physical states matter, and reversing a reaction changes the sign of delta H. A worked glucose example applies these rules.
These are comprehensive general chemistry lecture videos, built to help students succeed in the course, with clear step-by-step explanations, closed captions and practice quiz questions.
Timestamps:
0:00 Why we need enthalpy
1:20 Constant volume versus constant pressure
3:33 Deriving delta H = delta U + P delta V
6:49 Sign of delta H: endothermic and exothermic processes
8:11 Reading a thermochemical equation: melting ice
10:22 Enthalpy is an extensive property
13:03 Worked example: energy needed to make glucose
Part of: General Chemistry, Chapter 10
Keywords: enthalpy, delta H, thermochemical equation, constant pressure, extensive property, endothermic, exothermic, sign of delta H, general chemistry chapter 10
Related search terms: MCAT chemistry, DAT chemistry, OAT chemistry, PCAT chemistry, AP Chemistry, IB Chemistry, CLEP general chemistry, A-level chemistry, NEET chemistry, JAMB chemistry, community college chemistry, college general chemistry
#GeneralChemistry #Chapter10 #Enthalpy #Thermochemistry #DeltaH #DrKunapareddy
source