Energy of an object due to the motion of the object. It is represented: KE=1/2mv2.
Enthalpy versus Entropy
Enthalpy (H) - heat of a system. Negative enthalpy means that the temperature increases. Entropy (S) - randomness of a substance.
Specific heat capacity - number of joules of heat needed to warm 1 gram of a substance by 1K. Water's specific heat, in case you didn't remember, is 4.184J/g.
First Law of Thermodynamics = Law of Conservation of energy
Second Law of Thermodynamics - spontaneous reactions increase entropy (randomness).
Gibb's Free Energy
ΔG = ΔH - T ΔS, where T is temperature in Kelvin. If ΔG is negative, a reaction is spontaneous. Note that some reactions are always spontaneous, some are never, and some depend on the temperature. Also, H is measured in kJ, and S in J.