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15 Cards in this Set

  • Front
  • Back
the branch of chemistry that is the study of the energy changes that accompany chemical reactions and changes of state.
a device used to measure the energy as heat absorbed or released in a chemical or physical change.
a measure of how hot or cold something is; a measure of the average kinetic energy of the particles in an object.
the unit used to express energy; equivalent to the amount of work done by a foce of 1N acting through a distance of 1m in the direction of the force
the energy transferred between objects that are at different temperatures; energy is always transferred from higher-temperature objects to lower-temperature objects until thermal equilibrium is reached.
the quantity of heat required to raise one unit mass of homogeneous material 1K or 1C in a specified way given constant pressure and volume.
specific heat
the amount of energy released or absorbed as heat by a system during a process at constant pressure.
enthalpy of change
the amount of energy released or absorbed as heat during a chemical reaction.
enthalpy of reaction
an equation that includes the quantity of energy as heat released or absorbed during the reaction as written.
thermochemical equation
the amount of energy as heat resulting from the formation of 1 mol of a substance at constant pressure.
molar enthalpy of formation
the energy released as heat by the complete combustion of a specific amount of a substance at constant pressure of constant volume.
enthalpy of combustion
the overall enthalpy change in a reaction is equal to the sum of the enthalpy changes for the individual steps in the process.
Hess's law
a measure of the randomness or disorder of a system.
the energy in a system that is available for work; a system's capacity to do useful work.
free energy
the difference between the change in enthalpy, ^H, and the product of the Kelvin temperature and the entropy change, which is defined as T^S, at a constant pressure and temperature.
free-energy change