Final new material Flashcards
entropy
measure of the matter and/or energy dispersal within a system,
often described as a measure of the disorder of the system
Gibbs free energy
energy available to do work
G<0 exergonic/spontaneous
G>0 endergonic/ not spontaneous
G = 0 equilibrium
non spontaneous process
process that requires continual input of energy from an external source
reversible process
can go in both directions under same conditions
First law of thermodynamics
energy cannot be created or destroyed; it can only be converted from one form to another.
second Law of thermodynamics
all spontaneous process involve an increase in the entropy of the universe
Third law of thermodynamics
entropy of a perfect crystal at absolute zero is zero
spontaneous change
process that takes place without a continuous input of energy from an external source
standard entropy (S*)
entropy for one mole of a substance at 1 bar pressure
tabulated values are usually determined at 25C/298K
Standard entropy change
change in entropy for a reaction calculated using the standard entropies
standard free energy of formation (G*f)
change in free energy accompanying the formation of one mole of substance from its elements in their standard states
standard free energy change (G*)
change in free energy for a process occurring under standard conditions (1 bar pressure for gases, 1 M concentration for solutions)
anode
electrode at which oxidation occurs
cathode
electrode at which reduction occurs
cell potential (Ecell)
difference in potential of the cathode and anode half cells
electrolysis
process using electrical energy to cause a nonspontaneous process to occur
Faraday’s constant
charge on 1 mol of electrons
F = 96,485 C/mol e-
galvanic/voltaic cell
electrochemical cell in which a spontaneous redox reaction takes place
standard cell potential (E*cell)
the cell potential when all reactants and products are in their standard states (1 bar or 1 atm for gases, 1 M for solutions), usually at 298.15 K
standard electrode potential (E*x)
electrode potential measured under standard conditions (1 bar or 1 atm for gases, 1 M for solutions), usually at 298.15 K
spontaneous reactions are ____ exothermic
often
(but not always)