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Thermochemistry
The study of heat energy.
Radiant energy
Energy that comes from the sun; Earth’s primary energy source
Thermal Energy
Energy associated with the random motion of atoms and molecules.
Chemical Energy
Energy stored within the bond of chemical substances.
Nuclear energy
Energy stored within the collection of neutrons and protons in the atom.
Potential Energy
Energy stored within the collection of neutrons and protons in the atom.
Exothermic Process
Gives off heat; transfers thermal energy from system to surroundings.
Endothermic Process
Heat has to be supplied to the system from the surroundings
Thermodynamics
The study of intervention of heat and other kinds of energy
State Functions
Properties that are determined by the state of the system, regardless of how that condition was achieved.
ΔU = Uf - Ui
ΔV = Vf - Vi
ΔT = Tf - Ti
PΔV = nRT
First Law of Thermodynamics
Energy can be converted from one form to another, but cannot be created or destroyed.
ΔUsystem + ΔUsurroundings = 0
ΔUsystem = q + w
Work done by the System on the Surrounding
w = -P ΔV
Conversion factor between L·atm and J
101.3 J / 1
Enthalphy
Used to quantify the heat flow in or out of the system in a process that occurs at constant pressure.
ΔH
ΔH = Hproducts - Hreactants
ΔH>0, system absorbs heat
Endothermic
ΔH<0, system gives off heat
Exothermic
Specific Heat (s)
The amount of heat (q) required to raise one gram of the substance by one degree Celsius.
Heat Capacity (C)
The amount of heat (q) required to raise the temperature of a given quantity (m) of the substance by one degree Celsius.
Heat Capacity (C)
C =
Heat (q)
q = msΔt
q = CΔt
Entropy (S)
The measure of how spread out or how dispersed the system’s energy is.
