Chemistry Chapter 11 Thermochemistry
Heat Capacity
The amount of heat required to raise the temperature of a specified amount of a substance by 1°C or 1 K.
Thermochemical Equation
a chemical equation that includes the enthalpy change
Calorimeter
a measuring instrument that determines quantities of heat
Endothermic Process
a process that absorbs heat from the surroundings
Exothermic Process
a process that releases heat to its surroundings
System
a specific portion of matter in a given region of space that has been selected for study during an experiment or observation
Chemical Potential Energy
energy stored in chemical bonds
Surroundings
everything outside the system
Hess's Law of Heat Summation
if you add two or more thermochemical equations to give a final equation, then you also add the heats of reaction to give the final heat of reaction
Joule
the SI unit of energy, 4.184 Joules = 1 calorie
Heat of Fusion
the amount of heat absorbed by one mole of a solid substance as it melts to a liquid at a constant temperature
Specific Heat Capacity
the amount of heat energy required to raise the temperature of one gram of substance by one degree celcius
Molar Heat of Solidification
the amount of heat lost by one mole of a liquid as it solidifies at a constant temperature
Molar Heat of Vaporization
the amount of heat necessary to vaporize one mole of a given liquid
Molar Heat of Condensation
the amount of heat released by one mole of a vapor as it condenses to a liquid at a constant temperature
Energy
the capacity of a physical system to do work
Standard Heat of Formation
the change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states at 25 degrees celsius
Molar Heat of Solution
the enthalpy change caused by dissolution of one mole of substance in one liter of water.
Heat of Reaction
the enthalpy change for a chemical equation exactly as it is written
Law of Conservation of Energy
the fundamental principle of physics that the total energy of an isolated system is constant (is not created or destroyed) despite internal changes
Enthalpy (H)
the heat content of a system at constant pressure
Heat of Combustion
the heat of reaction for the complete burning of one mole of a substance
Specific Heat
the heat required to raise the temperature of one gram of a substance one degree centigrade
Heat
the movement of thermal energy from a substance at a higher temperature to one at a lower temperature
Calorimetry
the precise measurement of heat flow out of a system for chemical and physical processes
Thermochemistry
the study of the transfers of energy as heat that accompany chemical reactions and physical changes
Calorie
unit of heat defined as the quantity of heat required to raise the temperature of 1 gram of water by 1 degree centigrade at atmospheric pressure
