Chemistry: Chapter 15 (Energy)

Entropy

A measure if the number of possible ways that the energy of a system can be distributed; related to the freedom of the system's particles to move and the number of ways they can be arranged

Calorimeter

An insulated device that is used to measure the amount of heat released or absorbed during a physical or chemical process

Surroundings

In thermochemistry, includes everything in the universe except the system

Universe

In thermochemistry, it is the system plus the surroundings

System

In thermochemistry, the specific part of the universe containing the reaction or process being studied

Law of Conservation of Energy

States that in any chemical reaction or physical process, energy may be converted from one form to another, but is neither created nor destroyed.

Joule

The SI unit of heat and energy

Specific heat

The amount of energy required to heat one gram of any given substance by one degree Celsius

Calorie

The amount of heat required to heat one gram of pure water by one degree Celsius

Enthalpy of reaction

The change of enthalpy in a reaction

Free energy

The energy available to do work-the difference between the change in enthalpy and the kelvin temperature :)

Enthalpy

The heat content of a system at constant pressure

2nd law of thermodynamics

The spontaneous processes always proceed in such a way that the entropy of the universe increases

thermochemical equation

a balanced chemical equation that includes the physical status of all the reactants and the energy change, usually expressed as the change in enthalpy

heat

a form of energy that flows from a warmer object to a cooler object

Spontaneous process

a physical or chemical change that occurs without outside intervention and mat require energy to be supplied to begin the process

Hess's law

states that if you add two or more thermochemical equations to produce a final equation for a reaction, then the sum of enthalpy changes for the individual reactions is the enthalpy change for the final reaction

Energy

the capacity to do work or produce heat, exist as potential energy, and kinetic energy

Standard enthalpy of formation

the change in enthalpy that accompanies the formation of one mole of the compound in its standard state from its elements in their standard state

Chemical potential energy

the energy stored in a substance because of its composition; most is released or absorbed as heat during chemical reactions or processes.

Enthalpy of combustion

the enthalpy change for the complete burning of one mole of the substance

mole enthalpy of fusion

the heat required to melt one mole of a solid solution

Mole enthalpy of vaporization

the heat required to vaporize one mole of a liquid

Thermochemistry

the study of heat changes that accompany chemical reactions and phase changes