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General Chemistry > Chem Lesson 3: 13.1 - 13.4 > Flashcards

Chem Lesson 3: 13.1 - 13.4 Flashcards

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1
Q

Equilibrium

(Dynamic Equilibrium)

A

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.

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2
Q

Reversible Reaction (Half forward arrow over half reverse arrow)

A

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.

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3
Q

Reaction Rate

A

Speed at which a reaction takes place

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4
Q

Rate constant

A

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

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5
Q

Equilibrium Constant - Uppercase (K) (Definition)

A

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

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6
Q

Activity

A

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.

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7
Q

K,c Equilibrium Concentration Constant

A

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

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8
Q

K,p Equilibrium Constant

A

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)

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9
Q

Pressure

A

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

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10
Q

K,eq

A

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

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11
Q

K (equilibrium constant)»1

A

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

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12
Q

K (equilibrium constant)«1

A

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

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13
Q

K (equilibrium constant) is close to 1

A

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

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14
Q

Reaction Quotient (Q,c or Q,p)

A

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.

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15
Q

K,p Gasses or Aqueous Species?

A

Only Gasses

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16
Q

K,c Gasses or Aqueous Species?

A

Both

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17
Q

Homogenous Equilibria

A

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

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18
Q

Q > K (Which direction does reaction proceed)

A

Left

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19
Q

Q < K (Which direction does reaction proceed)

A

Right

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20
Q

Q = K (Which direction does reaction proceed)

A

Rxn at Equilibrium

21
Q

Total Pressure

A

The sum of the partial pressures

22
Q

Total Pressure (Units)

A

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

23
Q

Partial Pressure

A

Pressure of one type of gas in the total pressure.

24
Q

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

A

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

25
Q

Partial Pressure - Mole Fraction (equation)

A

(mol of individual pressure)/Total Moles

26
Q

Partial Pressure (Def)

A

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

27
Q

Partial Pressure (Final step after mole fraction step)

A

Mole fraction * total pressure (usually given)

28
Q

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

A
  1. Find mole fraction
  2. Multiple mole fraction by total pressure (not the total moles)
29
Q

How to calculate partial Pressure (not given moles)

A

Ideal Gas Law:PV =nRT

30
Q

R (Gas Law value)

A

0.0821 L*atm/mol * k

31
Q

K,p K,c Relationship Equation

A

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

32
Q

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

A

Sum[coefficients of products] - Sum[Coefficients of reactants]

-Must balance equation first

33
Q

Le Chartilier’s Principle

A

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

34
Q

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

A

Products

35
Q

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

A

Reactants

36
Q

Stress

A

Anything that takes the system out of equilibrium.

37
Q

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

A

Side with the less moles.

38
Q

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

A

Move to the side with more moles.

39
Q

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

A

Both

40
Q

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

A

To the right

41
Q

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

A

Shift to the left.

42
Q

Endothermic Reaction

A

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

43
Q

Exothermic Reaction

A

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

44
Q

Does equilibrium happen in open or closed environments?

A

Closed

45
Q

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

A

Reactants increase and products decrease

46
Q

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

A

Reactants decrease and the products increase.

47
Q

Heat

A

Energy transferred to the motion of atoms or molecules.

48
Q

Enthalpy (def)

A

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

General Chemistry (15 decks)

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