Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
47 Cards in this Set
- Front
- Back
Kinetic energy |
The energy an object has because of its motion |
|
Kinetic theory |
States that the tiny particles in all forms of matter are in constant motion |
|
Gas pressure |
Defined as the force exerted by a gas per unit surface area of an object |
|
Vacuum |
Empty space, with no particles, and no pressure |
|
Atmospheric pressure |
Results from the collisions of air molecules with objects |
|
Barometers |
Devices commonly used to measure atmospheric pressure |
|
Pascal (Pa) |
The SI unit of pressure |
|
Standard atmosphere (atm) |
One atm is the pressure required to support 760 mm of mercury in a mercury barometer at 25 degrees Cel just
1atm = 760 mm Hg = 101.3 kPa |
|
Vaporization |
The conversion of a liquid to a gas or vapor |
|
Evaporation |
Conversion occurs at the surface of a liquid that is not boiling |
|
Vapor pressure |
Particles collide with the walls of the sealed container to produce vapor pressure |
|
Boiling point |
(bp) is the temperature at which the vapor pressure of the liquid is just equal to the external pressure |
|
Normal boiling point |
Defined as the boiling point of a liquid at a pressure of 101.3 kPa |
|
Melting point |
(Mp) is the temperature at which a solid turns into a liquid |
|
Crystal |
Most solid substance. The atoms, ions, or molecules that make up the solid substance are arranged in an orderly, repeating, 3-dimensional pattern called the crystal lattice |
|
Unit cell |
The smallest group of particles within a crystal that retains the geometric shape of the crystal is known as a unit cell |
|
Allotropes |
Two or more different molecular forms of the same element in the same physical state |
|
Amorphous solids |
Lack an ordered internal structure (rubber, plastics, asphalts) |
|
Glasses |
Amorphous solids Transparent fusion products of inorganic substances that have cooled to a rigid state without crystallizing |
|
Phase diagram |
Gives the conditions of temperature and pressure at which a substance in a sealed container are best represented in a single graph |
|
Triple point |
Meeting point where all three phases can exist in equilibrium with eachother |
|
Sunlimation |
The change of a substance from a solid to a vapor without passing through the liquid state |
|
Thermochemistry |
Concerned with the Heat changes that occur during chemical reactions |
|
Energy |
The capacity for doing work or supplying heat |
|
Chemical potential energy |
Energy stored within the structural units of chemical substances |
|
Heat |
Represented by: q Energy that transfers from one object to another because of a temperature difference between them |
|
System |
Part of the universe on which you focus your attention |
|
Surroundings |
Everything else in the universe |
|
Universe |
Together the system and its surroundings constitute the universe |
|
Law of conservation of energy |
States that in any chemical or physical process, energy is neither created nor destroyed |
|
Endothermic process |
Process that absorbs heat |
|
Exothermic processs |
Process that released heat to its surroundings |
|
Calorie |
Defined as the quantity of heat needed to raise the temperature of 1 g of pure water 1 degree Celsius |
|
Joule |
The SI unit of heat and energy named after the English physicist 1 J = 0.2390 cal |
|
Heat capacity |
The amount of heat needed to increase the temp of an object exactly 1 degree Celsius of that object |
|
Specific heat capacity |
Or specific heat, of a substance is the amount of heat it takes to raise the temp of 1 gram of a substance 1 degree Celsius |
|
Calorimetry |
The accurate and precise measurement of heat change for chemical and physical processes |
|
Calorimeter |
The insulated device used to measure the absorption or release of heat in chemical or physical processes |
|
Enthalpy (H) |
For systems at constant pressure, the heat content is the same as a property (H) of the system |
|
Thermochemical equation |
An equation that includes the heat change |
|
Heat of reaction |
The heat change for the equation exactly as it is written |
|
Heat of combustion |
The heat of reaction for the completed burning of one mile of a substance |
|
Molar heat of fusion |
(🔼Hfus) The heat absorbed by one mile of a substance in melting from a solid to a liquid at a constant temperature |
|
Molar heat of solidification |
(🔼Hsolid) The heat lost when one mole of a liquid solidifies at a constant temp |
|
Molar heat of vaporization |
The amount of heat necessary to vaporize one mole of a given liquid |
|
Molar heat of condensation |
Amount of heat released when 1 mole of vapor condenses (🔼Hcond) |
|
Molar heat of solution |
The heat change caused by dissolution of one mole substance (🔼Hsolo) |