Assignment 6

Question 1

properties of a gas

Answer 1

volume

density

mass/amount/moles

pressure

Question 2

IMFs (what do they determine)

Answer 2

determine physical properties

Question 3

Particle Theory/Kinetic Molecular Theory

Answer 3

particles…

are meaured in moles (6.02 x 10²³)

have mass

are the smallest representative unit of a substance that contain the properties of the larger substance

travel randomly in a straight line

speed indicate its heat

have no IMFs (ideal gas assumption)

collide with each other and the walls of the container (measured by vol and pressure)

Question 4

particles

Answer 4

the smallest representative unit of a substance that contains the properties of the larger substance

Question 5

ideal gas assumption

Answer 5

no IMFs

PV = nRT

theoretical

no freezing/boiling point

no energy (heat) lost

Question 6

Relationship of Pressure to Volume

Answer 6

Inverse

same # particles + more volume/space = less bumping of particles = less pressure

same # particles + less volume/space = more bumping = more pressure

Question 7

Relationship of Pressure to Temperature

Answer 7

Direct (if you start at absolute zero)

more temp = more movement of particles = more bumping = more pressure

less temp = less movement of particles = less bumping = less pressure

Question 8

Relationship of Temperature to Volume

Answer 8

Direct (if you start at absolute zero)

more temp = more motion = more collision = more push on conainer = more volume

less temp = less motion = less collision = less push on conainer = less volume

Question 9

Relationship of Number of Moles (n) to Pressure/Temperature/Volume

Answer 9

Direct

more moles = more mass = more vol

more moles = more particles in same space = more bumping = more pressure

more moles = more particles bumping = more KE/heat = more temp

Question 10

Proportionality Constant R =

Answer 10

0. 0821 (for atm)
1. 314 (for kPa)
2. 396 (for mmHg/torr)

Question 11

what happens as a system is cooled

Answer 11

density increases

kinetic energy (temp) decreases

pressure decreases

volume decreases

particles squish together (IMFs became important, no ideal gas assumptions no equations)

Question 12

solid

Answer 12

low KE

IMFs > KE of particles

incompressable

maintains shape and vol

Question 13

liquid

Answer 13

medium KE

IMFs ≈ KE of particles

incompressable

constant vol, variable shape

Question 14

gas

Answer 14

high KE

IMFs (essentially zero) < KE

compressable

no set vol or shape

Question 15

boyle’s law

Answer 15

P₁V₁ = P₂V₂

Question 16

charles’ law

Answer 16

V₁/T₁ = V₂/T₂

Question 17

Gay-Lussac’s Law

Answer 17

P₁/T₁ = P₂/T₂

Question 18

gas law equation for descriptive and changing moles

Answer 18

PV = nRT

Question 19

gas law equation for changing conditions, constant moles

Answer 19

P₁V₁ P₂V₂

———— = nR = ———-

T₁ T₂

Question 20

mole fraction equation

Answer 20

P_x n_x

—————— = —————–

P_TOTAL n_TOTAL

Question 21

PV = nRT

Answer 21

gas law equation for descriptive and changing moles

Question 22

P₁V₁ P₂V₂

———— = nR = ———-

T₁ T₂

Answer 22

gas law equation for changing conditions, constant moles

Question 23

density (at STP) =

Answer 23

gfm

22.4

Question 24

density (not at STP) =

Answer 24

P(gfm)

RT

Question 25

Dalton’s Law of Partial Pressures

Answer 25

sum of the pressures in a vessel for a mixture of gases depend only on the pressures of the individual gases

P_TOTAL = P₁ + P₂ + … + P_n

Question 26

Graham’s Law (of Diffusion and Effusion)

Answer 26

smaller things diffuse faster

Question 27

diffusion

Answer 27

particles move from high concentration to low concentrations until they are equal

Question 28

effusion

Answer 28

particles will move from a pressurized space to a non-pressurized space (vaccum)

Question 29

temperature

Answer 29

measure of avg kinetic energy

Question 30

STP

Answer 30

standard temp (0ºC/273K) and pressure (1atm/101.3kPa/760mmHg/760torr)

Question 31

vapor

Answer 31

small airborne particles of liquid (not molecules like gas)

intermediary between gas and liquid

gas where liquid phase is present

Question 32

dynamic equilibrium

Answer 32

evaporation rate = condensation rate

Question 33

evaporation

Answer 33

no external energy added

automatically occurs with any liquid

Question 34

vapor pressure

Answer 34

partial pressure of vapor above any liquid

temp dependent: higher temp = higher avg KE = more particles have ability to leave = higher vapor pressure

Question 35

boiling

Answer 35

P_TOTAL = P_VAPOR

atmospheric pressure = vapor pressure

Question 36

freezing

Answer 36

phase change from liquid to solid

Question 37

melting

Answer 37

phase change from solid to liquid

Question 38

condensation

Answer 38

phase change from gas to liquid

Question 39

vaporization

Answer 39

phase change from liquid to gas

Question 40

sublimation

Answer 40

phase change from solid to gas without passing through liquid

Question 41

desposition

Answer 41

phase change from gas to solid without passing through liquid

Question 42

triple point

Answer 42

temp and pressure where all phases (solid, liquid, gas) occur simultaneously

Question 43

equilibrium

Answer 43

the temp and pressure where two phases exist simultaneously

Question 44

critical point

Answer 44

temp above which the substance is always a gas

Question 45

when do ideal gases behave like actual gases

Answer 45

at high temp/volume or low pressure

Question 46

1 atm =

Answer 46

101.3 kPa = 760 mmHg = 760 torr

Question 47

2 bonds + electron pairs

Answer 47

linear

sp

Question 48

3 bonds + electron pairs

Answer 48

trigonal planar

sp²

Question 49

4 bonds + electron pairs

Answer 49

tetrahedral

sp³

Question 50

5 bonds + electron pairs

Answer 50

bipyramidal

sp³d

Question 51

6 bonds + electron pairs

Answer 51

octahedral symmtery

sp³d²