Test 3 Equilibrium

Question 1

Collision theory

Answer 1

A reaction will occur if the reactants reactants collide with enough energy

Question 2

Activation energy

Answer 2

Minimum amount of energy needed for a reaction

Question 3

Anything that enhances collisions will __________ the rate of reaction

Answer 3

Increase

Question 4

Many gasses in a closed container are

Answer 4

Reversible

Question 5

Increasing concentration __________ rate of reaction

Answer 5

Increases

Question 6

Lowering temperature ___________ rate of reaction

Answer 6

Decreases

Question 7

Decreasing particle size __________ rate of reaction

Answer 7

Increases

Question 8

Catalysts __________ rate of reaction

Answer 8

Increase

Question 9

Anything that _____ __________ will increase rate of reaction

Answer 9

Enhances collisions

Question 10

Chemical equilibrium

Answer 10

Is reached when the rates of the foward and reverse reaction are equal

Question 11

Lechatelier’s principal

Answer 11

If a stress is applied to a system at equilibrium, the system changes to relieve the stress and return to equilibrium

Question 12

Stresses include a change in

Answer 12

Concentration
Temperature
Pressure

Question 13

Increasing the pressure of an equation would shift the equilibrium towards the side with the _______ moles

Answer 13

Least

Question 14

Increasing pressure has no effect on an

Answer 14

Aqueous solution

Question 15

Equilibrium position of a reaction

Answer 15

Is given by the relative concentrations of reactants and products at equilibrium

Question 16

Instead of using % for equilibrium position, equilibrium contracts are used (_____)

Answer 16

K eq

Question 17

Equilibrium constant equation

Answer 17

K eq = [C]^c [D]^d
___________
[A]^a [B]^b

[ ] = mol/liter or M

Question 18

K eq > 1

Answer 18

Products are favored at equilibrium

Question 19

K eq

Answer 19

Reactants are favored at equilibrium

Question 20

Solubility product constant

Answer 20

K sp

Question 21

Soluable

Answer 21

Describes ionic compounds (salts) that dissolve in water

Question 22

Insoluable

Answer 22

Describes ionic compounds (salts) that don’t dissolve in water

Question 23

The solubility product constant (K sp) quantifies

Answer 23

The extent to which salt dissolves

Question 24

Don’t include _____ in equilibrium expression

Answer 24

Solids

Question 25

Smaller k sp =

Answer 25

Lower solubility (less ions dissolved in solution)

Question 26

Common ion

Answer 26

Ion present in both salts

Question 27

Precipitate

Answer 27

A solid product that “comes out” of solution when two aqeous reactants are mixed

Question 28

Q ( reaction quotient )

Answer 28

Used in place of k sp at non equilibrium conditions

Question 29

Q > K sp

Answer 29

Precipitate will form

Question 30

Q

Answer 30

No precipitate will form

Question 31

Q = K sp

Answer 31

System is at equilibrium

Question 32

Rate of chemical change

Answer 32

Amount of reactant changing per unit time (how fast reactants become products)

Question 33

Equilibrium which processes occur continuously with no net charge

Answer 33

Dynamic equilibrium

Question 34

Chemical equilibrium

Answer 34

Dynamic with foward and reverse reactions occurring at the same rate

Question 35

Equilibria involving species in more than one phase

Answer 35

Heterogenous equilibrium