Reading...
Play button
Play button
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;
22 Cards in this Set
- Front
- Back
|
Activated Complex
|
The short-lived particle formed as the result of a collision of particles in a chemical reaction. In this complex, the electrons have the opportunity to shift positions and produce new combinations of atoms.
|
|
|
Activation Energy
|
The amount of energy required to initiate a chemical action.
|
|
|
Catalyst
|
A substance that changes the speed of a chemical reaction without being permanently altered itself.
|
|
|
Heat of Reaction
|
The quantity of heat liberated or absorbed during a chemical change
|
|
|
Heterogeneous Reaction
|
A reaction that involves reactants in more than one phase.
|
|
|
Homogenous Reaction
|
A reaction in which all the reactants are in the same phase.
|
|
|
Kinetics
|
The study of chemical reactions.
|
|
|
Potential Energy
|
The energy an object has because of its positions.
|
|
|
Rate-Determining Step
|
The slowest step of a reaction mechanism.
|
|
|
Reaction Mechanism
|
The series of steps by which reacting particles rearrange themselves to form the products of a chemical reaction.
|
|
|
Endothermic Reaction
|
A reaction that absorbs heat energy.
|
|
|
Enthalpy
|
A measure of the internal energy of a system.
|
|
|
Entropy
|
The degree of randomness or a measure of the probability of existence of a system.
|
|
|
Exothermic Reaction
|
A reaction that releases energy.
|
|
|
Free Energy
|
A measure of the tendency of a change to occur spontaneously.
|
|
|
Free Energy of Formation
|
The change in free energy when one mole of a compound is formed from its constituent elements.
|
|
|
Gibbs Equation
|
∆G = ∆H - T∆S, where ∆H equals the change in enthalpy, T equals the Kelvin temperature, and ∆S equals the change in entropy.
|
|
|
Heat of Formation
|
The heat absorbed or given off when a mole of a compound is formed from its elements.
|
|
|
Heat of Reaction
|
The quantity of heat liberated or absorbed during a chemical change.
|
|
|
Hess's Law
|
When a reaction can be expressed as the algebraic sum of two or more other reactions, then the heat of the reaction is the algebraic sum of the heats of these other reactions.
|
|
|
Kelvin Temperature
|
The temperature scale on which zero (0 K) is the lowest temperature that is theoretically attainable. It is called absolute zero.
|
|
|
Standard Heat of Formation
|
The reaction when 1 mole of a compound is formed from its elements at standard conditions (25 degrees C and 101.3 kPa)
|
