Chem Sat- Chemical Equilibrium

Front 1

equilibrium

Back 1

when the forward RXN rate is equal to the reverse RXN rate

Front 2

calculating forward RXN rate

for A+B--> AB

Back 2

R= k[A]^n[B]^n

these describe the REACTANTS

Front 3

calculating reverse RXN rate

for A+B--> AB

Back 3

R=k2 [AB]^n

these describe the PRODUCTS

Front 4

calculating equilibrium constants

Keq

for A+B--> AB

Back 4

k= [AB]^n / [A]^n[B]^n


put PRODUCTS over REACTANTS

Front 5

Large Keq

Back 5

Keq=equilibrium constant

takes longer to reach equilibrium

Front 6

Small Keq

Back 6

takes shorter amount of time to reach equilibrium

Front 7

what happens when the pressure is changed on a system at equilibrium

Back 7

it only changes the equilibrium if the system has GASES in it

Front 8

when writing equilibrium equations

Back 8

DON"T INCLUDE SOLIDS

since they have a fixed concentration

Front 9

Calculating Ka

Acid ionization constants

Back 9

Ka= [A]^n [B]^n / [C]^n [D]^n

concentrations of products/concentrations of reactants



when a weak acid doesn't ionize completely it reaches an equilibrium (acid dissociation constant)

Front 10

Small Ka

Back 10

concentration of unionized acid is large

Front 11

large Ka

Back 11

concentration of unionized acid is small

Front 12

the smaller the Ka

Back 12

the weaker the acid

Front 13

Ionization constant of water

Back 13

1e-14

Front 14

PH=

Back 14

-log[H3O +]

Front 15

1-->6

Back 15

ACID

Front 16

8--->14

Back 16

BASE

Front 17

%dissociation

Back 17

mol/L that dissociate / original concentration

x100

Front 18

Ksp

calculating Ksp


Solute---> it's ions

example AgCl---> Ag+ + Cl-

Back 18

Ksp= [A]^n [B]^n


take the solute's ions (not the solute b/c it's a solid) and use the concentrations to find the ksp

Front 19

Common Ion effect

Back 19

when more ions are added the reverse reaction increases

ex. NaCl---> Na+ + Cl-

when HCL is added the reverse reaction increases b/c it adds Cl- ions

Front 20

delta S

Back 20

entropy

when there are more moles of gas on the products side the entropy has INCREASED

when there are more moles of gas on the reactants side the entropy has DECREASED

Front 21

Entropy equation

Back 21

delta S universe= delta S system + delta S surroundings

Front 22

entropy (delta S) is positive (very entropic)

Back 22

when a gas is formed from a solid

when a gas is evolved from a solution

when the #mols of a gaseous product is bigger than the # mols of a gaseous reactant

when crystals dissolve in water

Front 23

Gibbs equation

Back 23

delta G= delta H - T(delta S)

T=temperature in Kelvin

Front 24

delta G

Back 24

spontaneity

a negative delta G means it's spontaneous

Front 25

delta H

Back 25

enthalpy

positive delta H means it's endothermic

Front 26

delta S

Back 26

entropy

positive delta S means it's more chaotic