Chem Lesson 3: 13.1 - 13.4

Question 1

Equilibrium

(Dynamic Equilibrium)

Answer 1

The forward and reverse reaction rates are equal and when the concentrations of reactants and products aren’t changing anymore but it doesn’t necessarily mean that they are equal.
-The reversible reaction is still happening.

Question 2

Reversible Reaction (Half forward arrow over half reverse arrow)

Answer 2

The reactants combine to form products and at the same time products convert into reactants.
-Forward reaction is happening at the same time as reverse reaction.

Question 3

Reaction Rate

Answer 3

Speed at which a reaction takes place

Question 4

Rate constant

Answer 4

Constant in the rate law that depends on the specific reactants on hand and is related to the activation energy and temperature.

Question 5

Equilibrium Constant - Uppercase (K) (Definition)

Answer 5

The ratio of units (pressure or concentration) of the products over the reactants.
-Used to figure out whether we have more products or reactants.

Question 6

Activity

Answer 6

How many particles appear to be present in a solution.
-Solids and Liquids have an activity of 1 and aren’t used in the equilibrium constants.

Question 7

K,c Equilibrium Concentration Constant

Answer 7

Ratio of unit concentration of products over reactants.
-Let’s us see if we have more reactants or products in reversible reaction at equilibrium.

Question 8

K,p Equilibrium Constant

Answer 8

Ratio of unit pressure of products over reactants.
-Let’s us see if we have more reactants or products.
-Ratio surrounded by brackets and starts with p
-K,p = (PCO)^2/(PO,2)

Question 9

Pressure

Answer 9

Force exerted by gaseous molecules as they collide with the walls of their container.

Question 10

K,eq

Answer 10

Another meaning for equilibrium constant. May or may not specify p or c.

Question 11

K (equilibrium constant)»1

Answer 11

More products than reactants if the number is a lot bigger than one.

Question 12

K (equilibrium constant)«1

Answer 12

A lot more reactants than products at equilibrium if the number is way less than one.

Question 13

K (equilibrium constant) is close to 1

Answer 13

Similar ratio of reactants and products at equilibrium if the equilibrium constant is close to one.

Question 14

Reaction Quotient (Q,c or Q,p)

Answer 14

Ratio of units (concentration or pressure) of products over reactants at any given time. (Equilibrium Constant is only at equilibrium).
-Used to determine whether we have more products or reactants in reversible reaction.

Question 15

K,p Gasses or Aqueous Species?

Answer 15

Only Gasses

Question 16

K,c Gasses or Aqueous Species?

Answer 16

Both

Question 17

Homogenous Equilibria

Answer 17

All reactants and products in a reverse equilibrium reaction have the same phase. (Gas, Aqueous, etc)

Question 18

Q > K (Which direction does reaction proceed)

Answer 18

Left

Question 19

Q < K (Which direction does reaction proceed)

Answer 19

Right

Question 20

Q = K (Which direction does reaction proceed)

Answer 20

Rxn at Equilibrium

Question 21

Total Pressure

Answer 21

The sum of the partial pressures

Question 22

Total Pressure (Units)

Answer 22

Pa, Kpa, atm, or torrents (look at the question)

Question 23

Partial Pressure

Answer 23

Pressure of one type of gas in the total pressure.

Question 24

Ideal Gas Law (Equation)
& what does n and R stand for.

Answer 24

PV = nRT
n= amount of Moles
R = Energy Constant (0.08206 L atm/m*K)

Question 25

Partial Pressure - Mole Fraction (equation)

Answer 25

(mol of individual pressure)/Total Moles

Question 26

Partial Pressure (Def)

Answer 26

Pressure of one specific gas molecule that's apart of total pressure

Question 27

Partial Pressure (Final step after mole fraction step)

Answer 27

Mole fraction * total pressure (usually given)

Question 28

How to calculate partial pressure? (Two Steps) (Given Moles)

Answer 28

1. Find mole fraction 2. Multiple mole fraction by total pressure (not the total moles)

Question 29

How to calculate partial Pressure (not given moles)

Answer 29

Ideal Gas Law:PV =nRT

Question 30

R (Gas Law value)

Answer 30

0.0821 L*atm/mol * k

Question 31

K,p K,c Relationship Equation

Answer 31

K,p = K,c(RT)^delta n

Question 32

Delta^n (k,p k,c conversion equation

Answer 32

Sum[coefficients of products] - Sum[Coefficients of reactants] -Must balance equation first

Question 33

Le Chartilier's Principle

Answer 33

When a chemical system at equilibrium is disturbed it returns to equilibrium by counteracting the disturbance.

Question 34

Q < K (Le Charts - need to create more what?)

Answer 34

Products

Question 35

Q > K (Le Charts - need to create more what?)

Answer 35

Reactants

Question 36

Stress

Answer 36

Anything that takes the system out of equilibrium.

Question 37

Increase in Pressure (Le Chart - What direction does the reaction move?)

Answer 37

Side with the less moles.

Question 38

Decrease in Pressure (Le Chart - What direction does the reaction move?)

Answer 38

Move to the side with more moles.

Question 39

Le Chart - Does temp affect Q (Concentrations) or Kc (equilibrium constant)?

Answer 39

Both

Question 40

Le-Chart - Increasing heat in an endothermic reaction causes what shift?

Answer 40

To the right

Question 41

Le-Chart - Increasing heat in an exothermic reaction at equilibrium causes what shift?

Answer 41

Shift to the left.

Question 42

Endothermic Reaction

Answer 42

Energy is taken in. (Causes the temperature of the reaction mixture (system) to decrease).

Question 43

Exothermic Reaction

Answer 43

Energy is given off. (Causes the temperature of the system (reaction mixture) to increase).

Question 44

Does equilibrium happen in open or closed environments?

Answer 44

Closed

Question 45

Shift to the left (What do reactants and products do?)

Answer 45

Reactants increase and products decrease

Question 46

Shift to the right (What do reactants and products do?)

Answer 46

Reactants decrease and the products increase.

Question 47

Heat

Answer 47

Energy transferred to the motion of atoms or molecules.

Question 48

Enthalpy (def)

Answer 48

State function that shows heat loss or gain in a system.