Exam 2

Question 1

see last deck for colligative properties

Answer 1

okayt

Question 2

isotonic

Answer 2

concentration inside equals outside

Question 3

hypotonic

Answer 3

high concentrations of solute inside cell so water flows in

Question 4

hypertonic

Answer 4

concentration of solute is greater outside cell so it leaves

Question 5

suspension

Answer 5

particles settle out

Question 6

colloids

Answer 6

particles don’t settle out

Question 7

surfactant

Answer 7

hydrophilic head with a hydrophobic tail

Question 8

monolayer

Answer 8

one layer of surfactant

Question 9

micelles

Answer 9

nonpolar tails surround with polar heads sticking out. helps dissolve stuff AKA soap

Question 10

vesicles

Answer 10

polar inside, non polar facing each other and then polar heads facing outside again

Question 11

cell membrane

Answer 11

phospholipid bilayer. polar phospholipid head with 2 lipid tails that are hydrophobic

Question 12

supersaturated solutions

Answer 12

more than can dissolve, very unstable

Question 13

reaction mechanisms

Answer 13

the pathway that the materials follow while becoming products. can be unimolec, with one reactant, bi with two tri with three

Question 14

elementary reaction

Answer 14

one step of a mechanism

Question 15

mechanism

Answer 15

has multiple elementary reactions

Question 16

intermediate

Answer 16

appears between steps and not in products

Question 17

reaction rate

Answer 17

number of molecules reacting per second.

Question 18

rate determining step

Answer 18

slowest elementary reaction

Question 19

rate units

Answer 19

molarity per second

Question 20

as you go on with reactions, rate

Answer 20

decreases as there are fewer reactant molecules present. fewer collisions occur. the rate per collision is constant

Question 21

High conc, hi molecules, hi collisions

Answer 21

hi rate

Question 22

Twice as many NO moles

Answer 22

number of collisions doubles compared to just NO one mol

Question 23

overall order

Answer 23

sum of exponents

Question 24

Rate laws mirror the reactions stoichiometry for

Answer 24

rate- limiting steps

Question 25

first order reaction

Answer 25

Ln(A0/A)= kt ln of A vs t is straight

Question 26

second order reactiona

Answer 26

1/A-1/A0 = kt graph of 1/a vs t gives a line with slope k

Question 27

zero order reactions

Answer 27

A= -kt+ A0 graph of A vs t gives a line

Question 28

slopes are equal to

Answer 28

k

Question 29

half life of first order reaction

Answer 29

ln2/K

Question 30

half life is independent of A0 in

Answer 30

first order reactions

Question 31

energy profile for unimolecular reactions

Answer 31

fragmentation is when the products is higher than reactants rearrangement is when the energy rises but still releases

Question 32

energy profile for bimolecular reactions

Answer 32

energy rises then falls, still releases

Question 33

activated complex

Answer 33

AKA THE TRANSITION STATE. TOP O FTHE GRAPH

Question 34

RATE increases with

Answer 34

temperatrue

Question 35

Arrhenius equation

Answer 35

Ln (K2/K1) = - Ea/ R(1/t2 - 1/T1) T in kelvin R is 8.314 j since it is about activation energy!!

Question 36

catalysts

Answer 36

INCREASE RATES OF REACTION

Question 37

homo and hetero catalyst

Answer 37

same vs different phase of reactant

Question 38

in equilibrium

Answer 38

rates of forward and reverse reactions are equal NOT CONCENTRATIONS

Question 39

can be Keq or Kp

Answer 39

okay

Question 40

Keq

Answer 40

describes concenreatrions of reactants and products when the NET rate of reaction is zero

Question 41

Q

Answer 41

products over reactants. tells you which way equilibrium shifts

Question 42

when the reaction is reversed

Answer 42

K IS INVERSE NOT -VE

Question 43

converting between Kp and Kc

Answer 43

Kp= Kc (RT)^ delta N of gas R is 0.0821 T in K Delta n is # of moles of gas in products- number of moles of gas. can be -ve

Question 44

what is not in equilibrium

Answer 44

pure liquids and solids

Question 45

if K is huge

Answer 45

then reaction is basically completion

Question 46

if K is small

Answer 46

it basically doesn't occur

Question 47

increase in pressure

Answer 47

shifts to side with less gas moles

Question 48

K varies only with

Answer 48

temperature.

Question 49

what happens to k with for endothermic reaction when you add heat

Answer 49

K eq increases, shifts to produce less heat

Question 50

what happens to k with for exothermic reaction when you add heat

Answer 50

K eq decreases, shifts to side with less heat

Question 51

to prove X is negligble

Answer 51

put initial concentration over K and if its over 1000 , its negligble

Question 52

if K is very large

Answer 52

reaction goes to nearly completion so X is ALL final concentration

Question 53

strong acids

Answer 53

Her, HI, HCLO4, Hal, HNO3, N2SO4

Question 54

strong bases

Answer 54

group ! and 2 OH and CaOH, Sr OH and BaOh

Question 55

strong acids and bases K

Answer 55

dissociate. very large K have Ka and Kb make Oh or H3O

Question 56

solubility equilibrium

Answer 56

ksp usually makes solid

Question 57

complexation equilibrium

Answer 57

Kf

Question 58

weak acids

Answer 58

Ka