Studied by 4 peopleEnergy
The ability to do work or transfer heat.
Change in Energy
\Delta E=E_{final}-E_{initial}
Thermodynamics
The study of energy and its transformations.
Thermochemistry
The study of chemical reactions and the energy changes involving heat.
First Law of Thermodynamics
Energy cannot be created or destroyed, only converted from one form to another.
Systems and Surroundings
The system is the portion of the universe under study, while the surroundings are everything else.
Types of Systems
Open System, Closed System, Isolated System.
Internal Energy
The sum of kinetic and potential energies of a system's components.
Changes in Internal Energy
Positive and negative changes indicate energy absorption or release.
\Delta E=q+w
Heat (q)
Energy exchanged between the system and surroundings.
Work (w)
Energy exchanged as work during a process.
Exchange of Heat Between System and Surroundings
Endothermic and exothermic processes.
State Functions
Internal energy is independent of the path taken to reach a state.
Work
Mechanical work associated with changes in gas volume.
Enthalpy
Internal energy plus the product of pressure and volume.
H=E+PV
Amount of Heat
q=mc\Delta T
Enthalpy of Reaction
Heat of reaction, dependent on reactants' and products' states.
Calorimetry
Measurement of heat flow.
Hess’s Law
Enthalpy change for an overall reaction equals the sum of changes for individual steps.
\Delta H=\sum n\Delta H_{f,products}-\sum m\Delta H_{f,reactan ts}^{°}
Enthalpies of Formation
Enthalpy change for forming a compound from its elements.
Bond Enthalpy
Energy required to break chemical bonds.
Bond Enthalpies and Enthalpy of Reaction
Predicting endothermic or exothermic reactions using bond energies.
\Delta H_{rxn}=\sum bonds\:broken-\sum bonds\:formed
Note 
Flashcard (22)