Studied by 3 peopleLe Châteliers principle
states that when a stress is applied to a system at equilibrium, the equilibrium shifts to relieve the stress.
→Gases
________ have more disorder and therefore higher entropy than liquids because particles in the gas move around more freely than particles in the liquid.
non spontaneous reaction condition
A(n) positive value for ∆G means that free energy must be added and the process is nonspontaneous.
∆S
Conversely, ________ has a negative value if the disorder of a system decreases.
catalyst
A(n) ________ does not affect the energy level of either reactants or products.
chemical compounds
In ________, the attractive forces between ions or atoms are a form of potential energy.
spontaneous reaction conditio
A(n) negative for ∆G means that free energy is released and the reaction or process is spontaneous.
endothermic
A(n) chemical change that absorbs heat, like the breaking of bonds, is endothermic.
exothermic processes
For ________, heat is released (lost) and is indicated with a negative sign.
nonspontaneous process
A(n) ________ requires continuous external influence and is endergonic; that is, free energy is added and it has a positive value of ∆G.
external assistance
A spontaneous process, once begun, proceeds without any ________ and is exergonic; that is, free energy is released and it has a negative value of ∆G.
reverse reactions
When a reaction reaches equilibrium, the rates of the forward and ________ are equal, and the concentrations of reactants and products remain constant.
external influence
A spontaneous process is one that, once started, proceeds on its own without any ________.
There are two fundamental kinds of energy
potential and kinetic
Two factors determine the spontaneity of a chemical or physical change
the release or absorption of heat, ∆H, and the increase or decrease in entropy, ∆S
K much smaller than 0.001
Only reactants are present at equilibrium; essentially no reaction occurs
K between 0.001 and 1
More reactants than products are present at equilibrium
K between 1 and 1000
More products than reactants are present at equilibrium
K much larger than 1000
Only products are present at equilibrium; reaction goes essentially to completion
potential energy
it is stored energy
kinetic energy
it is the energy of the motion
bond dissociation energy
amount of energy that must be absorbed to break the bond and separate the atoms in an isolated gaseous molecule.
heat of reaction
The difference between the heat energy absorbed in breaking bonds and the heat energy released in forming bonds
entropy
The amount of disorder in a system
activation energy
The amount of energy the colliding particles must have for productive collisions to occur
Note 
Flashcard (55)