Chapter 5 Review Topics

Chapter 5:  Thermochemistry

Definitions:  Thermodynamics, thermochemistry

Kinetic Energy:   E_k = ½ mV² 

Potential Energy:   E_p = mgh

Force of gravity:   9.81 m/s²

Joule = 1Kgm²/s²

Calorie = 4.184 J (exactly)

Watt = 1J/s

BTU

System vs. surroundings

Heat, work, force (w=fxd), (f = ma)

Energy:   capacity to do work or transfer heat

1^st Law of Thermodynamics  (Law of Conservation of Energy)

ΔE = E_final – E_initial

ΔE = q + w

System wants less energy; one of the 2 driving forces in nature.

State function

Enthalpy (H)

ΔE = ΔH when nor work done, or work done at constant pressure

Exothermic = - ΔH;  Endothermic = + ΔH

Graphing a ΔH reaction

ΔH is an extensive property

Stoichiometry calculations with ΔH

Calorimetry:  calorimeter, specific heat, heat capacity, molar heat capacity,

    constant pressure calorimetry

Hess’ Law: 

     writing heat of formation equations, Standard State conditions,

     computations using Hess’ Law and the Heats of Formation table (Appendix C)

     to find ΔH^o for a reaction: a) the long way by adding equations; b) the short

     way by using only the Heats of Formation.

Food as fuel