Chem 102 Lab Final

Front 1

Arrhenius Equation

Back 1

k = Ae^(-Ea/RT)

Front 2

K usually _______ with Temperature

Back 2

Increased

Front 3

What is the slope in lnk=-Ea/RT + lnA in lnk vs. 1/T

Back 3

slope = -Ea/R

Front 4

concentration equation

Back 4

c = n/v

Front 5

Calculate order of reaction

Back 5

Rate1/Rate2=(K1A1^nB1^m)/(K2A2^nB2^m)

Front 6

Iodine clock

Back 6

2 S2O3 2- + I2 —> 2I- + S4O6 2-

Front 7

What reaction occurs after all the thiosulfate in the iodine clock reaction has been reacted?

Back 7

I2 + I- —> I3 -

Front 8

What does the linear triiodide molecule reaction with and what colour does it turn?

Back 8

Reacts with starch and turns blue

Front 9

What does the delta t of colourless —> indicate ?

Back 9

the time that it takes to react all of the S2O3 2-

Front 10

T= infinity

Back 10

K = A

Front 11

rate = k’[dye]^q

q=0?

q=1?

q=2?

Back 11

0, half life and zero order reaction vary linearly with [dye]

1, half life and first order reaction are independent of [dye]

2, second order reaction and half lives are inversely proportional to [dye]

Front 12

Zero order

Back 12

Back (Definition)

Front 13

First order

Back 13

Back (Definition)

Front 14

Second Order

Back 14

Back (Definition)

Front 15

Half life, zero order

Back 15

t1/2 = [A]o/2K

Front 16

Half life, first order

Back 16

t1/2 = ln2/k

Front 17

Half life, second order

Back 17

t1/2 = 1/k[A]o

Front 18

What layer is the I2 in ?

Back 18

Mineral Oil layer

Front 19

What layer is the I2 in ?

Back 19

Mineral Oil layer

Front 20

Is the mineral oil layer above or below the aqueous layer?

Back 20

Above

Front 21

Distribution coefficient

Back 21

equilibrium of one species in between two phases

Front 22

pH = ?

Back 22

-log[H3O+]

Front 23

pOH = ?

Back 23

-log[OH-]

Front 24

[H3O+] = ?

Back 24

10^-pH

Front 25

[OH-] = ?

Back 25

10^-pOH

Front 26

HA + H2O —> ?

Back 26

H3O+ + A-

Front 27

pH = pKa at ?

Back 27

1/2 equivalence volume

Front 28

[A-(at equivalence point)] = ?

Back 28

n HA initial / V HA initial + V NaOH added

Front 29

Equivalence Point

Back 29

moles of tire ant equals moles of reactant initially in the sample

Front 30

pH at equivalence point = ?

Back 30

pH of A- in solution at same concentration

Front 31

%Dissociation = ?

Back 31

[H3O+]eq/[HA]initial x 100%

Front 32

Buffer capacity

Back 32

the amount of acid or bae that can be added with only a minimal change in the pH of the solution

Front 33

pH = ?

Back 33

pKa + log ([Base]/[Acid])

Front 34

n acid neutralized by antacid = ?

Back 34

n H added to antacid - n NaOH used in back titration

Front 35

pKa = ?

Back 35

-log Ka

Front 36

Ka = ?

Back 36

10^-pKa

Front 37

Oxidation number

Back 37

electrons lost

Front 38

coordination number

Back 38

how many ligands are bonded

Front 39

monodentate ligand

Back 39

H2O

Front 40

cheating agent

Back 40

EDTA

Front 41

C heat capacity ?

Back 41

the amount of energy or “heat” needed to change the temperature of a substance per degree

Front 42

c

Back 42

specific heat capacity

Front 43

Cm

Back 43

molar heat capacity

Front 44

delta H

Back 44

enthalpy

Front 45

Exothermic

Back 45

Enthalpy leaving the system

Front 46

Endothermic

Back 46

Enthalpy entering the system

Front 47

delta Go = ?

Back 47

-RTlnK

Front 48

delta Go = ?

Back 48

delta Ho - T delta So

Front 49

delta H neutralization = ?

Back 49

-C water x (Tf - Ti) water

Front 50

Reducing agent

Back 50

species that is oxidized by losing electrons

Front 51

Oxidizing agent

Back 51

species that gains electrons and is reduced

Front 52

What appears in the reactants of a spontaneous reaction?

Back 52

The better reducing agent and better oxidizing agent appear in the reactants

Front 53

E = ?

Back 53

Eo - 0.0592/n logQ

Front 54

Ecell = ?

Back 54

E cathode - E anode

Front 55

E cell = ?

Back 55

E red - E ox

Front 56

Eo cell = ?

Back 56

(Eoc - 0.0592/nc logQcathode) - (Eoa - 0.0593/na logQanode)