equilibrium

Question 1

rate

Answer 1

measure of the speed of any change that occurs within an interval of time

Question 2

how are rates of chemical reactions measured

Answer 2

change in the number of moles during an interval of time

Question 3

collision theory

Answer 3

atoms, ions, and
molecules can react to form products when they
collide with one another, provided that the
colliding particles have enough kinetic energy.

Question 4

activation energy.

Answer 4

The minimum energy that colliding particles

must have in order to react

Question 5

activated complex

Answer 5

an unstable
arrangement of atoms that forms momentarily at
the peak of the activation-energy barrier.

Question 6

transition state.

Answer 6

another name for activated complex

Question 7

The rate of a chemical reaction depends

upon

Answer 7

temperature, concentration,

particle size, and the use of a catalyst.

Question 8

inhibitor

Answer 8

a substance that interferes

with the action of a catalyst.

Question 9

reversible reaction

Answer 9

one in which the
conversion of reactants to products and

the conversion of products to reactants occur
simultaneously.

Question 10

At chemical equilibrium,

Answer 10

no net change occurs in

the actual amounts of the

components of the system.

Question 11

chemical equilibrium.

Answer 11

When the rates of the forward and

reverse reactions are equal,

the reaction has reached a state

of balance called

Question 12

equilibrium position

Answer 12

The relative concentrations of the reactants and

products at equilibrium

Question 13

equilibrium constant (Keq)

Answer 13

the ratio of product

concentrations to reactant

concentrations at equilibrium,

Question 14

For all Keq,

Answer 14

·Units are omitted

·Regardless of initial [ ] the reaction

will establish equilibrium.

·Equilibrium can be obtained from either direction
of the reversible reaction

·Each set, or trial of equilibrium [ ] is called an
equilibrium position.

Question 15

Homogeneous equilibria

Answer 15

all reactants and

products are in the same state

Question 16

Heterogeneous equilibria

Answer 16

substances

are in more than one state

Question 17

what forms can be used?

Answer 17

Only use those in gaseous
(g) and aqueous (aq) forms;
ignore those in solid (s) or
liquid (l) forms

Question 18

·At equilibrium, the

Answer 18

forward and reverse
reactions are
proceeding at the same
rate.

Question 19

Once
equilibrium is
achieved,

Answer 19

the
amount of each
reactant and
product
remains
constant.

Question 20

·If K»1,

Answer 20

the reaction
is product-favored;
product
predominates

Question 21

·If K

Answer 21

the
reaction is
reactant-favored; reactant
predominates

Question 22

a Reaction Quotient

Answer 22

If the system is not at
equilibrium the ratio is known
as

Question 23

If Q > Keq

Answer 23

the product side
is too high and the equilibrium
will shift to the left to restore
equilibrium

Question 24

If Q

Answer 24

the product side
is too low and the equilibrium
will shift to the right to
restore equilibrium

Question 25

Le Châtelier’s principle:

Answer 25

If a stress is applied to a system

in dynamic equilibrium, the system

changes in a way that relieves the stress.

Question 26

when you decrease pressure, the system shifts to the

Answer 26

direction the

produces more moles of gas.

Question 27

solubility product constant (ksp)

Answer 27

the product of the concentrations of the ions, each raised o a power equal to the coefficient of the ion in the dissociation equation

Question 28

common ion

Answer 28

ion found in both salts in a solution

Question 29

common ion effect

Answer 29

if the product of the concentrations of two ions in the moixture is greater than the ksp of the compound formed from the ions, a precipitate will form