Chem 102 Unit 1

Front 1

1st order half life

Back 1

.693/k = .5T

ln([Ao/.5Ao]) = KT

Front 2

2nd order half life

Back 2

1/K[Ao]

Front 3

Zero order reaction

Back 3

A -> product
rate = k

Front 4

arrhenius equation

Back 4

K=Ae^-Ea/RT

A = pre exponential term (dependent constant)
Ea = energy of activation
R = 8.314 J/mol
T = temperature, K

Front 5

arrhenius equation slope intercept

Back 5

ln k = (-Ea/R)(1/T) + ln A

y = m x + b

Front 6

arrhenius plot

Back 6

ln (K1/K2) = -Ea/R (1/T1 - 1/T2)

Front 7

arrhenius equation measures....

Back 7

use energy of activation to predict how changes in temperature affect reaction

Front 8

determine first order rate law by

Back 8

taking ln of concentration vs time; need straight line

Front 9

determine second order rate law by

Back 9

1/[concentration] vs time

Front 10

collision frequency

Back 10

Z, number of molecular collisions per second

Front 11

activation complex

Back 11

peak of graph; site where reaction is occurring, extremely temporary and unstable

Front 12

3 types of catalysts

Back 12

homogenous - same state as reactants
heterogenous - different state
enzyme - large molecules that catalyze biological rxns

Front 13

molecularity

Back 13

number of species in a single elementary step
iA + iB = products

if total i is 1 unimolecular, first order rxn
if total i is 2 bimolecular, second order rxn
termolecular

Front 14

Equilibrium constants do not include

Back 14

solids or liquids (only gas, aqueous)

Front 15

Kc and Kp are

Back 15

unitless

Front 16

Kp =

Back 16

Kc (.0821xT)^ delta n

delta n = # of moles GAS products - # of moles GAS reactants

Front 17

homogeneous vs heterogeneous equilibria

Back 17

reversible reactions same phase/different phases

Front 18

if two reactions added, overall Kc is

Back 18

PRODUCT of individual reactions Kc's

Front 19

Qc > Kc

Back 19

rxn goes R to L forming more reactants

Front 20

Qc < Kc

Back 20

rxn goes L to R forming more producst

Front 21

Qc is Kc but

Back 21

using actual concentrations

Front 22

pressure up?

Back 22

favors side of rxn with less moles of GAS

Front 23

volume up

Back 23

favors side of rxn with more moles of gas

Front 24

le chateliers principle

Back 24

if external stress is applied to a system at equilibrium, the system adjusts to partially offset it (changes direction to stabilize)

Front 25

law of mass action

Back 25

aA+bB (back an forth yields) cC + dD

Front 26

equilibrium constant expression

Back 26

[C]^c[D]^d/[A]^a[B]^b = Keq

Front 27

temp up?

Back 27

endothermic - products
exothermic = reactants

Front 28

energy of activation increases, rate

Back 28

increases

Front 29

forward energy _____ reverse energy in reaction step = energy of step

Back 29

minus

Front 30

catalysts actually

Back 30

participate in the rxn

Front 31

catalysts _______ and ________

Back 31

lower Ea and create a new path