Module 3 - Thermochemistry Flashcards
The study of heat change in chemical reactions.
Thermochemistry
The transfer of thermal energy between two bodies that are at different temperatures.
Heat
The specific part of the universe (substances or conditions) that are of specific interest to us
Systems
The rest of the universe outside the system.
Surroundings
A type of system that can exchange mass and energy.
Open system
A type of system that allows the transfer of energy (heat) but not mass.
Closed system
A type of system that which does not allow the transfer of either mass or energy.
Isolated system
Any process that gives off heat or transfers thermal energy to the surroundings.
Exothermic process
Any reaction in which heat has to be supplied to the system by the surroundings.
Endothermic process
The scientific study of the interconversion of heat and other kinds of energy.
Thermodynamics
Defined by the values of all relevant macroscopic properties (i.e. composition, energy, temperature, pressure, and volume).
State of a system
Properties that are determined by the state of a system, regardless of how the condition was achieved.
State functions
States that energy can be converted from one form to another; but cannot be created nor destroyed.
First Law of Thermodynamics
Thermodynamic Processes
- Pressure remains constant.
- System either expands or contracts.
Isobaric Process
Thermodynamic Processes
- Volume remains constant.
- The system cannot expand or contract.
Isochoric Process
Thermodynamic Processes
- Temperature remains constant.
Isothermal Process
Thermodynamic Processes
- No heat exchanged with the surroundings.
- The system doesn’t absorb or release any heart energy.
Adiabatic Process
Difference between the enthalpies of the products and the enthalpies of the reactants.
Enthalpy of reactions
Shows the enthalpy changes as well as the mass relationships.
Thermochemical equations
The science of measuring the amount of heat.
Calorimetry
“Calor” meaning
Heat
“Metry” meaning
To measure
Amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius.
Specific heat (s)
Amount of heat required to raise the temperature of a given quantity of the substance by 1 degree Celsius.
Heat capacity (C)
The heat changes that results when a mole of a compound is formed from its elements in the standard states.
Standard enthalpy of formation
The enthalpy change when the reaction is carried out under standard-state conditions.
Standard enthalpy of reaction
