Chemical Equilibrium

Question 1

Define rate.

Answer 1

the speed at which a process occurs

Question 2

Define chemical equilibrium.

Answer 2

when the forward and reverse reactions reach a state of balance in which the concentrations of the reactants and products remain the same

Question 3

Define complex ion.

Answer 3

any metal atom or ion that is bonded to more than 1 atom or molecule

Question 4

Define ligands.

Answer 4

molecules or anions that readily bond to metal ions

Question 5

Define solubility product constants.

Answer 5

equilibrium constants for the dissolution of slightly soluble salts

Question 6

What do reversible reactions do?

Answer 6

They reach equilibrium when the concentration of the reactants and the product is constant

Question 7

Define Keq.

Answer 7

a constant which shows the ratio of product concentrations to reactant concentrations, with each concentration raised to the power equal to its coefficient at equilibrium

Question 8

What is a favorable reaction?

Answer 8

A reaction that will have a higher concentration of products than reactants, resulting in a large Keq at equilibrium

Question 9

Define stress.

Answer 9

something that causes a change in a system at equilibrium

Question 10

Define Le Chatelierś Principle.

Answer 10

States that when a system at equilibrium is disrupted, the system adjusts in a way to reduce the change

Question 11

The equilibrium constant is

Answer 11

concentrations of products vs reactants at equilibrium

Question 12

which of the following can change an equilibrium constant: concentration, rate, temperature, or pressure

Answer 12

temperature

Question 13

reactions tend to run to completion if

Answer 13

a gaseous product escapes or a precipitate forms

Question 14

Keq > 1 (large equilibrium constant)

Answer 14

products are favored at equilibrium

Question 15

Keq < 1 (small equilibrium constant)

Answer 15

reactants are favored at equilibrium

Question 16

what happens at equilibrium?

Answer 16

both the forward reaction and backward reaction have the same rate

Question 17

a ligand is a molecule or ion that can

Answer 17

make a bond with a transition metal ion

Question 18

what must a ligand have?

Answer 18

a lone pair of electrons

Question 19

at equilibrium…

Answer 19

the concentration of reactants and products must be constant

Question 20

increasing temperature in an exothermic reaction will shift the equilibrium towards the

Answer 20

products (the right)

Question 21

Any change in temperature, concentration, or pressure on the system at equilibrium is called a

Answer 21

stress

Question 22

Which change would shift the equilibrium to the right? N2(g) + 3H2(g) –> 2NH3 (g) + heat: increase the pressure, increase the temperature, decrease the H2, decrease the N2

Answer 22

increase the pressure

Question 23

If the reactant is added (adding a reactant or removing a product)

Answer 23

the equilibrium shifts to the right

Question 24

if the product is added (adding a product or removing a reactant)

Answer 24

equilibrium shifts to the left

Question 25

The Common Ion Effect is used to explain what?

Answer 25

Shift in equilibrium position due to a concentration of an ion

Question 26

The smaller the value of the solubility product constant:

Answer 26

the lower the solubility of the compound

Question 27

what can Ksp be applied to?

Answer 27

slightly soluble solutions

Question 28

Define the Haber process.

Answer 28

The manufacturing of ammonia from nitrogen and hydrogen

Question 29

Define the common ion effect.

Answer 29

the lowering of solubility of a substance by the presence of a common ion

Question 30

When do you see a reversible reaction?

Answer 30

when the reaction goes forward and backwards w/o extra energy being used

Question 31

What happens when you increase pressure at equilibrium?

Answer 31

there is more stress on the high volume than the low volume (pressure will shift to the lower side)

Question 32

What happens when you decrease pressure at equilibrium?

Answer 32

the reaction proceeds in the direction that raises pressure to where it was (most gas molecules)

Question 33

What happens when heat is added?

Answer 33

endothermic reaction is favored (shifting to the left, favoring reverse reaction)

Question 34

What happens when you raise the temperature?

Answer 34

the reaction goes to the right

Question 35

What happens when you lower the temperature?

Answer 35

reaction goes to the left