is the study of the transfers of energy as heat that accompany chemical reactions and physical changes.
the energy absorbed or released as heat in a chemical or physical change is measured
is a measure of the average kinetic enrgy of the particles in a sample of matter
is the SI unit of heat as well as all other forms of energy
can be thought of as the energy transferred between samples of matter because of a difference in their temperatures
is the amount of energy required to raise the temperature of one gram of a substance by one celsius degree
is th eamount of energy absorbed by a system as heat during a process at constant pressure
Enthalpy of Reaction
is the quantity of energy transferred as heat during a chemical reaction
an equation that includes the quantity of energy released of absorbed as heat during the reaction as written
Morlar Enthalpy of Formation
is the enthalpy change that occurs when one mole of a compound is formed from its elements in their standard state at 25C and one atom
Enthalpy of Combustion
the enthalpy change that occurs during the complete combustion of one mole of a substance
the overall enthalpy change in a reaction is equal to the sum of enthalpy changes for the individual steps in the process
a measure of the degree of randomness of the particles such as molecules in a system
this combined enthalpy-entropy function
of a system is defined as the difference between the change in enthalp, and the product of the Kelvin temperature and the entropy chnage which is defind as TtriangleS
the change of state in which a solid becomes a liquid by adding energy as heat or changing pressure
the change of state in which a liquid becomes asolid as energy as heat is removed
the process by which a liquid or solid changes to a gas
the change of state from a gas to a lizuid
the temperature and pressure conditions at which a solid, liquid, and gaseous phases of a substance coexist at equilibrium
the process in which a solid changes directly into a gas
the change of state from a gas directly to a solid
the temperature and pressure at which the gas and liquid states of a substance become identical and form one phase
the lowest pressure at which a substance can exist as a liquid at the critical temperature
the temperature above which a substnace cannot exist in a liquid state
the change of state from a liquid to a gas
the boundary between solid and liquid for any given substance plotted on the phase
a graph of th evapor pressure of a solid as a function of temperature, goes directly from a solid to a gas
Substance at a temperature and pressure above its critical point
barely visible or cloudy difused matter mist fums of smoke supended in the air
process by which particles escape from the surface of a nonboiling liquid and enter the gas state
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