TOPIC 9- CHEMICAL EQUILIBRIUM

Question 1

applies to the extent of a reaction, the
concentration of product that has appeared after an unlimited
time, or once no further change occurs.

Answer 1

Equilibrium

Question 2

is the state where the concentrations
of all reactants and products remain constant with time.

Answer 2

Chemical Equilibrium

Question 3

At equilibrium,

Answer 3

rate forward = rate reverse

Question 4

is the ratio of reactants and products
calculated the same way as Keq.

Answer 4

Reaction quotient

Question 5

If Q = K, the reaction is in

Answer 5

equilibrium

Question 6

If Q < K, the reaction will proceed from

Answer 6

reactants to products

Question 7

If Q > K, the reaction will proceed from

Answer 7

product to reactants

Question 8

applies to reactions in which all reacting species are in the same phase.

Answer 8

Homogeneous Equilibrium

Question 9

Only _________________ are accounted for in calculating the
reaction quotient and the equilibrium constant.

Answer 9

Gaseous species

Question 10

three ways to change the pressure of a reaction system
involving gaseous components.

Answer 10

1. Add or remove a gaseous reactant or product.
2. Add an inert gas (one not involved in the reaction).
3. Change the volume of the container.

Question 11

Adding a gaseous reactant increases the volume of the reactant
side. For the system to reach equilibrium again, the volume is
decreased by

Answer 11

increasing pressure

Question 12

Increasing the pressure (decreasing the volume) shifts the
equilibrium to form

Answer 12

fewer molecules and moles of gas

Question 13

Decreasing the pressure (increasing the volume) shifts the
equilibrium to form

Answer 13

more molecules and moles of gas

Question 14

If a gaseous reactant/product is added/removed, check the
changes in Q to determine where the

Answer 14

equilibrium shifts

Question 15

The addition of an inert gas increases the ________________ but
has no effect on the concentrations

Answer 15

total pressure

Question 16

When the volume of the container is changed,

Answer 16

concentrations (and thus the partial pressures) of both
reactants and products are changed.

Question 17

Reducing the volume of the container shifts the equilibrium to the
side with ____________________ in the balanced equation.

Answer 17

fewer gas molecules

Question 18

Increasing the volume of the container shifts the equilibrium to the
side with ______________ in the balanced equation.

Answer 18

more gas molecules

Question 19

ndicates there are relatively large
concentrations of product gases as compared with the
concentrations of reactant gases at equilibrium.

Answer 19

large value for Keq (Keq > 1)

Question 20

A reaction with
a large Keq value is a

Answer 20

good source of products

Question 21

Keq and Kp are equilibrium constants as determined by the

Answer 21

law of mass action

Question 22

Q is called the

Answer 22

reaction quotient

Question 23

Q has the same
form as Keq or Kp, but instead of equilibrium concentration, ___________ are used to calculate the Q value.

Answer 23

initial concentrations

Question 24

When a chemical system at equilibrium is subjected to stress,
the system will return to equilibrium by shifting to reduce the
stress.

Answer 24

Le Chatelier’s Principle

Question 25

If the reactant concentration increases, the system reacts to

Answer 25

consume some of it

Question 26

if the concentration decreases, the system
reacts to

Answer 26

produce some of it

Question 27

If the concentration of the product decreases, the system
reacts to

Answer 27

produce some of it

Question 28

The reaction will start from which side concentrations were

Answer 28

increased

Question 29

Only _________changes can alter K.

Answer 29

temperature

Question 30

is considered as a product or reactant

Answer 30

heat

Question 31

In exothermic reactin, heat is a

Answer 31

product

Question 32

in endothermic reaction, heat is a

Answer 32

reactant

Question 33

applies to reactions in which reactants and products are in different phases.

Answer 33

Heterogeneous equilibrium