Chemistry Chapter 10 And 11

Front 1

Gas-->Solid

Back 1

deposition

Front 2

Gas-->Liquid

Back 2

condensation

Front 3

Liquid-->Solid

Back 3

freezing

Front 4

Liquid-->Gas

Back 4

evaporation

Front 5

Solid-->Liquid

Back 5

melting

Front 6

Solid-->Gas

Back 6

sublimation

Front 7

Melting Point

Back 7

the temperature and pressure at which a solid becomes a liquid

Front 8

Boiling Point

Back 8

the temperature and pressure at which liquid and gas molecules are in equilibrium

Front 9

fusion

Back 9

transition between solid and liquid

Front 10

enthalpy (both formulas)

Back 10

q=mCpT

Q=nCT

Front 11

gibbs energy formula

Back 11

determines spontinaeity of the reaction

G=H-TS

Front 12

catalyst

Back 12

speeds up reaction

moves curve down on the graph that shows exothermicness

Front 13

heat
vs
temp

Back 13

heat: the energy transferred between objects that are at different temperatures

temp: the measure of the avg kinetic energy of the particles in an object

Temp=intensive property (temperature does not depend on the amount of the sample)

heat=extensive property(amount of energy transferred depends on amount of heat in the sample)

Front 14

Enthalpy

Back 14

the sum of the internal energy of a system

H

Front 15

molar heat capacity

Back 15

the energy as heat needed to increase the temperature of 1 mol of the substance by 1 K

Front 16

Molar Enthalpy Change

Back 16

the enthalpy change for one mole of a pure substance

molar enthalpy change=CT
molar enthalpy change=(moalr heat capacity)(temperature change)

Front 17

H=q when...

Back 17

you are heating or cooling of substances

Front 18

endothermic reactions have _____ enthalpy changes

exothermic reactions have ______ enthalpy changes

Back 18

positive

negative

Front 19

Standard thermodynamic Temperature

Back 19

25.00 degrees Celcius

used to standardize the enthalpies of reactions, both reactants and products have it

Front 20

Calorimetry

Back 20

measures enthalpy change (H)

Front 21

Hess's Law

Back 21

adding up the equations

the law that states that the amount of heat released or absorbed in a chemical reaction does not depend on the number of steps in the reaction

Front 22

entropy

Back 22

the measure of the randomness or disorder of a system

thermodynamic property

J/k

S

Front 23

a process is more likely to occur if it is accompanied by a _______ in entropy, that is S is ________

Back 23

an increase

positive

Front 24

Gibbs energy/free energy

Back 24

the energy in a system that is available for work

G=H-TS

Front 25

FILL IN A GIBBS TABLE

RIGHT NOW

Back 25

H | S | G | Spontaneous?
-----------------------------
- | + | - | yes
- | - | +/- | only if T<H/S
+ | + | +/- | only if T>H/S
+ | - | + | never

Front 26

H=CT

Back 26

change in molar enthalpy when ONLY temperature changes

Front 27

surface tension

Back 27

the force that acts on the surface of a liquid and that tends to minimize the area of the surface

Front 28

intermolecular forces

Back 28

the forces of attraction between molecules

Front 29

enthalpy of fusion

Back 29

the energy added during melting or removed during freezing

Front 30

entropy of fusion

Back 30

as a solid melts, particle motion increases as it transitions into the liquid state (or other way around)

Front 31

triple point

Back 31

the temperature and pressure conditions at which the solid, liquid and gaseous phases of a substance coexist at equilibrium

Front 32

order on a phase diagram (from left)

Back 32

solid, liquid, vapor

Front 33

critical point

Back 33

the temperature and pressure at which the gas and liquid states of a substance become identical and form one phase

Front 34

what are the units for Energy

Back 34

Joules

Front 35

under what conditions is heat (q) the same as enthalpy (H)

Back 35

at constant pressure

Front 36

in an endothermic reaction, do the products or reactants have lower energy

Back 36

reactants

Front 37

are products or reactants more stable in an endothermic reaciton?

Back 37

reactants, because you have to give it energy for it to do anything

Front 38

what does entropy tell you about a reaction?

Back 38

entropy determines the randomness of the particles of a substance

Front 39

what does it mean if the sighn for S for a reaction is
A.negative
B.positive

Back 39

A.if it is negative it will be less likely to happen

B. If S is positive a process is more likely to occur


(see gibbs table)

Front 40

What does Gibb's energy tell you about a reaction

Back 40

it tells you the spontaneity of a reaction aka whether or not it will happen

Front 41

If a reaction has a negative H and a positive S, what will the sign of G be? Is this reaction spontaneous?

Back 41

negative

yes it will be spontaneous

Front 42

is condensing an endothermic or exothermic process?`

Back 42

exothermic process

Front 43

hydrogen bond

Back 43

bonds with forces of high electronegativity (right corner)

Front 44

dipole-dipole

Back 44

interactions between polar molecules

Front 45

london dispersion force

Back 45

the intermolecular attraction resulting from uneven distribution of electrons and the creation of temporary dipoles

Front 46

vapor pressure

Back 46

the partial pressure exerted by a vapor that is in equilibrium with its liquid state at a given temperature