Unit 10

Front 1

system

Back 1

the substances materials or objects under evaluation in a thermodynamic process

Front 2

surroundings

Back 2

everthing outside the system in a thermodynamic process

Front 3

universe

Back 3

the system and the surroundings

Front 4

state function

Back 4

a function whose changed value depends only upon its initial and final states-it is independent of the path taken in going from the initial state to the final state

Front 5

Entropy

Back 5

a thermodynamic state function that is the measure of disorder of a system

Front 6

what are two fundamental laws of nature that are important in thermodynamics?

Back 6

1. systems tend to attain a state of minimum energy
2. systems tend toward a state of maximum disorder

Front 7

zeroth law of thermodynamics

Back 7

if two bodies are each in thermal equilibrium with a third body,then they are in equilibrium with each other

Front 8

first law of thermodynamics

Back 8

the internal energy of a system increases when energy is transferred from the surroundings to the system or when the surroundings perform work on the system

Front 9

second law of thermodynamics

Back 9

the total entropy of the Universe always increases for a spontaneously occurring process

Front 10

third law of thermodynamics

Back 10

the entropy of a perfectly pure crystalline structure at absolute zero is zero

Front 11

spontaneous chemical reaction

Back 11

a reaction that proceeds from left to right (reactants to products) to achieve equilibrium

Front 12

Non-spontaneous chemical reaction

Back 12

a reaction that proceeds from right to left (products to reactants) to achieve equilibrium

Front 13

Gibbs free energy

Back 13

a thermodynamic state
function that can be used to determine
whether or not a given reaction is
spontaneous at a particular set of conditions

Front 14

The standard molar Gibbs Free Energy of Formation

Back 14

The change in free energy accompanying the
formation of one mole of a compound from its
elements in their standard states at standard
conditions

Front 15

Oxidation-Reduction Reaction

Back 15

A reaction in which changes in oxidation number occur

Front 16

oxidation number

Back 16

The apparent charge on an atom in a molecule or ion at the “ionic limit.”

Front 17

Ionic Limit

Back 17

A limiting case where all the bonds are assumed to be ionic, even though we know they aren’t.

Front 18

oxidation

Back 18

the increase in oxidation number

Hint 18

oxidation can be conveniently viewed as the loss of electrons

Front 19

reduction

Back 19

the decrease in oxidation number.

Hint 19

reduction can be conveniently viewed as the gain of electrons

Front 20

oxidizing agent

Back 20

reactant that causes
another substance to become oxidized.

Hint 20

The oxidizing agent is the reactant that is
being reduced.

Front 21

reducing agent

Back 21

the reactant that causes
another substance to become reduced

Hint 21

The reducing agent is the reactant that is
being oxidized.

Front 22

Combustion reaction

Back 22

A reaction between a substance and molecular
oxygen (O2) in which most (if not all) of the
products have oxygen as part of their
formulas.

Front 23

Electrochemical reaction

Back 23

A chemical reaction that produces electricity

Front 24

voltaic cell

Back 24

an electrochemical cell that uses a chemical reaction to produce electricity

Front 25

electrolysis cell

Back 25

an electrochemical cell that uses electricity to drive a chemical reaction.

Front 26

anode(anode compartment)

Back 26

the site where oxidation takes place (electrons are released)

Front 27

cathode(cathode compartment)

Back 27

the site where reduction takes place (electrons are consumed).

Front 28

external electrical circuit

Back 28

allows for the electrons generated at the anode to flow to the cathode.

Front 29

salt bridge

Back 29

needed to maintain the balance of charges in the anode and cathode compartments.
–(Anions flow from cathode compartment to anode compartment; cations flow from anode compartment to cathode compartment).