Chemistry 2 Test 2

Front 1

Chemical equilibrium

Back 1

A type of dynamic equilibrium that occurs when a reaction and its reverse reaction proceed at the same rates

Front 2

Approaches equilibrium

Back 2

Both the forward and reverse reactions are occurring but at different rates

Front 3

Equilibrium achieved

Back 3

Both the forward and reverse reactions are occurring at the same rate

Front 4

keq

Back 4

equilibrium constant

Front 5

Equilibrium expression

Back 5

kc = C^c x D^d / A^a x B^b

Front 6

kp

Back 6

Particle pressure

Front 7

Relationship between KC and KP

Back 7

Kp = Kc (RT)^ ∆n

Front 8

∆n

Back 8

Moles of gases product - moles of gases reactants

Front 9

products, reactants

Back 9

K>1 favor

K<1 favor

Front 10

Homogenious equilibrium

Back 10

When all substances and chemical equilibrium are in the same phase

Front 11

Heterogeneous equilibrium

Back 11

When all substances in a chemical reaction are not in the same phase

Front 12

Pure solid or liquid

Back 12

These concentrations do not matter in an equation

Front 13

For a system that is not yet at equilibrium

Back 13

Q is used when

Front 14

Too much product left
Too much reactants right

Back 14

Q > K too much _____ shifts _____
Q< K too much ______ shifts ______

Front 15

Le Chateliers Principle

Back 15

1. Adding or removing a reactant or product
2. Change in pressure or volume
3. Change in temperature

Front 16

expert a lower pressure

Back 16

Fewer gas molecules

Front 17

a change in volume or pressure will not shift in either direction

Back 17

If the number of gas molecules is the same on both side...

Front 18

Pressure and volume

Back 18

Inverse of each other

Front 19

Endothermic

Back 19

Increasing temperature a reactant results in more product so K is larger

Front 20

Exothermic

Back 20

Increasing temperature a product results and more reactant so K is smaller

Front 21

Catalyst

Back 21

Increase the rate of those for it and reverse reaction by same amount. The cooler brand is it cheaper faster but does not change the position of the equilibrium picture.

Front 22

Arrhenius

Back 22

Acid substance that dissolves in water increases concentration of protons.

Base of substance same

Front 23

Bronsted - Lowry

Back 23

Acid proton donor. base proton acceptor

Front 24

amphiprotic amphoteric

Back 24

Chemical species that can either donate or accept protons

Front 25

Hydronium

Back 25

H3O+

Front 26

The weaker its conjugate is

Back 26

The stronger an acid or a base...

Front 27

Moving the proton from the stronger acid to the stronger base

Back 27

Equilibrium will favor which type of reaction for acids and bases

Front 28

Autoionization

Back 28

In pure water a few molecules act as bases and if you act as acid to form hydroxide and hydronium ions

Front 29

KW

Back 29

1.0 x 10^-14

Front 30

- log of

Back 30

PH

Front 31

10^-ph

Back 31

H3O+

Front 32

14

Back 32

PH + Poh

Front 33

Basic

Back 33

Red paper blue

Front 34

acidic

Back 34

Blue paper red

Front 35

- log of M, if base subtract from 14

Back 35

For strong acids and bases if it gives you the molarity then...

Front 36

Ka

Back 36

Acid dissociation constant

Front 37

Percent ionization

Back 37

H+ equilibrium/ Ha initial x 100

Front 38

Ka Kb

Back 38

[H+]^2 / ACID
[OH-]^2 / BASE

Front 39

Presentaion ionization is less than 5%

Back 39

In an acid and base calculation for pH you do not need an ice table if

Front 40

Neutral

Back 40

Nacl
Na -> base Na(OH-) strong
Cl -> acid HCl strong

Front 41

Oxy acids

Back 41

Acid in which an OH- group is bonded to another atom Y

Front 42

Lewis base

Back 42

Electron pair donators

Front 43

Lewis acid

Back 43

Electron pair acceptor

Front 44

enzymes

Back 44

catalyst of biological systems