Gases are miscible.

What does this mean?

What are the four units of pressure?

And how are they all related?

atmospheres; torr; mmHg; Pascals

1 atm=760 torr=760 mmHg=1.01E5 Pa

What is included in the ideal gas equation

PV=nRT

pressure (atm)

volume (L)

number of moles

R (constant) .08206 atm-L/mol-K

R for pressure (atm/torr) .08206 atm-L/mol-K

R for energy (heat/energy) 8.314

V1P1=V2P2

volume and pressure are indirectly proportional

What does STP stand for?

what what are the values?

standard temperature and pressure

T= 0 degrees celsius

273.15 K

P= 1 atm

standard molar volume: 22.4 L

one mole of any gas will occupy 22.4 L at STP.

(depends on number of moles... it may double or triple)

at a given temperature, the energy and the speed of a molecule is inversely proportion to what?

(rate of effusion equation)

IDEAL GASES:

-work best as ____ pressure and ____ temperatures

-assumes no ________ ______

-assumes no ______ ______

low/high

intermolecular interaction

molecular volume

REAL GASES:

-molecules have _______ size and occupy ______

-molecules have _______ forces that become significant when they are in close proximity

-at ______ pressures attractive forces lead to the appearance of fewer ______

-at very _____ pressure the finite volume of molecules causes repulsion and leads to the appearance of more ____

finite/space

attractive

high/moles

high/moles

in the real gas equation:

pressure values are adjusted to account for...?

what is the constant?

attractive interactions of intermolecular forces

a

in the real gas equation:

volume is adjusted to account for the...?

what is the constant?

finite volume, molecular shape and the increased frequency of collisions

b

what two components make up a majority of the earth's atmosphere?

in what proportions (%volume and mole fraction)

nitrogen N2

78.084%

.78084

oxygen O2

20.948%

.20948

at a lower altitude the pressure is greater.

why?

ozone:

- ___ resonance forms

- ____ stable than O2

-_____ bond length than O2

-Bent angle at ____degrees

-what color?

2

less

longer

117

light blue gas

how many reactions are needed to form ozone?

how many reactions are needed to destroy ozone?

2

1

carbon dioxide

water

Solid state:

-_________ force between the particles is far _____ than the ________ _____ of the particles.

solid state:

-particles remain in _______

-solid has a ______ shape

-no _______

-no _____ ___ _____

stronger IF's mean...

-position

-specific

-compressibility

-ability to flow

higher melting point

Liquid state:

________ _____ of the particles is ______ than those in a solid but still weaker than the ______ ____

kinetic energy

stronger

attractive force

liquid state:

___ = ____

liquid state:

-kinetic energy allows for particles to ____ ____, but remain in virtual _____

-very low ______

-moderate ____ __ ____

tumble randomly/contact

compressibility

ability to flow

Gas State:

the _____ ____ of the particles is stronger than _____ _____

-occupy the shape of the _____

-high _______

-high _____ __ ____

kinetic energy

attractive forces

container

compressibility

ability to flow

solid ---> liquid

endo or exo?

melting/fusion

endo

liquid ----> gas

endo or exo?

vaporization

endo

solid ---> gas

endo or exo?lo

sublimation

endo

** at low pressure

gas ---> liquid

endo or exo?

condensation

exo

liquid ---> solid

endo or exo?

freezing

exo

gas ----> solid

endo or exo?

deposition

exo

what are the delta H symbols?

liquid and solid...

liquid and gas...

solid and gas...

fus

vap

sub

definition:

the amount of heat needed to change the temperature of 1 gram of a substance by 1 Kelvin

Phase change:

during a phase shift, the ______ remains constant and all heat energy changes result from either _______ or ____ the _____ between the molecules within the substance

temperature

forming/breaking

bonds

energy changes are calculated using:

delta H: fusion

delta H: vaporization

bomb calorimeters

coffee cup calorimeters

temperature:

-raising the temperature increases the _____ ____ of the molecules, making it easier for them to escape from the ______, and harder for them to _______.

-in general, the higher the temperature, the higher the ______ _______

kinetic energy/surface/return

vapor pressure

intermolecular forces:

-these are the _____ ____ that keep particles ______. Weake intermolecular forces allow the particles to _______ more easily.

-in general, the weaker the intermolecular forces, the higher the ______ _____.

attractive forces/together/vaporize

vapor pressure

for normal compounds, an increase in pressure will result in the phase change of liquid to solid, like CO2.

Why is this?

the maximum amount that can be dissolved into a fixed amount of a specific solvent at a given temperature.

what is this?

1. ion-dipole (ion-polar)

2. dipole-dipole (two polar molecules)

3. hydrogen bonding (H-NOF)

4. ion-induced dipole (ion-nonpolar)

5. dipole-induced dipole (polar-nonpolar)

6. dispersion (London) (nonpolar-nonpolar)

common solution:

_____ solvents

______ or ______ solutes

liquid

liquid/solid

solubility:

-ions and polar molecules will readily dissolve into ______ solvents

-nonpolar molecules will readily dissolve into ______ solvents

polar

 nonpolar

when a solution is formed, energy is either ______ or ______.

which is measures by a change in ______.

released/absorbed

enthalpy

enthalpy

solute particles separate

solvent particles separate

solute and solvent mix

endo

endo

exo

what is it called when solvent particles surround a solute particle?

what is this called in water?

solvation

hydration

what if it has less than the maximum amount of dissolved solute particles?

what if it has more?

unsaturated

supersaturated

temperature and solubility:

for solids, increasing temperature ______ solubility.

for gases dissolved in water, increasing temperature ______ solubility.

increases

decreases

pressure and solubility

-as pressure increases, the solubility of a gas _______

M

moles of solute/Liters of solution

1. molarity (M)

2. molality (m)

3. parts by mass

4. parts by volume

5. mole fraction (x)

not all electrolyates are ionic compounds...

true or false

1. vapor pressure lowering

2. osmotic pressure changes

3. boiling point elevation

4. freezing point depression

lowering vapor pressure

-the vapor pressure of a solution is always ______ than that of the pure solvent

-what law proves this?

lower

Raoult's Law

boiling point increase

a solution has a _______ boiling point than the pure solvent

freezing point decrease

-a solution freezes at a ______ temperature than a pure solvent

Van"t Hoff Factor, i

-refers to how the amount of ______ _____ can increase if the solute itself i able to ______ into its constituent ions.

-______ that are capable of _______ in solution are often called ________

solute particles/dissociate

solutes/dissociating/electrolytes

osmotic pressure

-known also as ______ pressure

-it is produced by a solution with a ________ in the concentration of solute

-- Van't Hoff factor refers to how the mount of solute particles ______ by a ________ factor if the solute is an ionic compound and _______ into its _________ ions.

hydrostatic

differential

increases/specific/dissociates/constituent