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Chemistry > Chapter 14: Principles of Chemical Equilibrium > Flashcards

Chapter 14: Principles of Chemical Equilibrium Flashcards

1
Q

Reversible reactions

A

Can proceed in both forward and reverse directions

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2
Q

What becomes constant when at equilibrium?

A

The concentrations

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3
Q

What becomes equal at equilibrium?

A

The rates

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4
Q

The equilibrium expression despribes the concentration of reactants and products when the net rate of the reaction is_____?

A

Zero

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5
Q

Rate Law

A

Describes how the rate of a reaction changes with concentration

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6
Q

What are the 5 rules of the equilibrium constant?

A
  1. Applies only at equilibrium
  2. Is related to the stoichiometry of the balanced net reaction
  3. Is independent of initial concentrations
  4. Is dimensionless and has no units
  5. Pure solids and liquids are not included because their activities are constant and equal to 1.
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7
Q

How are the forward and reverse Keq related?

A

Keq forward = 1/Keq reverse

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8
Q

What does a big Keq favour?

A

Products

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9
Q

What does a small Keq favour?

A

The reactants

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10
Q

For nonequilibrium conditions, Keq is replaced by?

A

Q

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11
Q

If Q<Keq?

A

The reaction shifts to the products

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12
Q

If Q>Keq?

A

The reactions shifts to the reactants

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13
Q

If Q = Keq?

A

The reaction is at equilibrium and there is no net change

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14
Q

What is Le Chatelier’s Principle?

A

When a change is imposed on a system at equilibrium, the system will react in the direction that reduces the change

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15
Q

What does Le Chateliers principle not apply to?

A

The addition of catalysts. Catalysts change the rate of the reaction, not the equilibrium conditions

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16
Q

Does adding a solid or liquid change the equilibrium concentrations?

A

No

17
Q

What is the only variable that can change Keq?

A

Temperature

18
Q

An increase in temperature always shifts the equilibrium position in the ______ direction.

A

Endothermic

19
Q

A decrease in temperature always shifts the equilibrium position in the __________ direction

A

Exothermic

20
Q

What does increasing pressure do to the system?

A

Shifts to the side of the reaction with fewer number of moles of gas

21
Q

What does decreasing the pressure do to the system?

A

Shifts the side of the reaction with the greater number of moles of gas

22
Q

If there are the same number of gas molecules on both sides of the equilibrium?

A

Increasing/decreasing the pressure has no effect on the position of the equilibrium

23
Q

If the equilibrium constant has a very small value, we can assume what?

A

That the change required to reach equilibrium (x) is very small and can be ignored

24
Q

What do you do with a very large equilibrium constant?

A

Work backwards. Start by acting as though the reaction went to completion, then work your way to equilibrium.

25
Q

What are the two categories for an aqueous solution?

A

Major species and minor species

26
Q

What is a major species?

A

High concentrations

27
Q

What is a minor species?

A

Low concentrations

28
Q

What is the dominant equilibrium?

A

The more important equilibrium. Always has major species as its reactants, but the products can be major or minor

29
Q

What species is always a major species in an aqueous solution?

A

H2O

30
Q

In aqueous salt solutions, major species are ______ molecules and _______ generated by the salt

A

Water molecules

Cations and anions

31
Q

What are the major species of a strong acid?

A

H2O and H3O+ by removing a proton from the acid

32
Q

What are the major species in an aqueous solution of a strong base?

A

H2O, OH-, and the cation generated by the base

33
Q

What are the three categories for aqueous equilibria?

A
  1. Proton Transfer (Acid/Base)
  2. Solubility (excess solid salt and a saturated solution indicate a solubility equilibrium
  3. Complexation (When metal cations in aqueous solutions form bonds to anions or neutral molecules that have lone pairs of electrons)
34
Q

The equilibrium constant for transfer of a proton from an acid to a water molecule is called ________?

A

The acid hydrolysis constant (Ka)

35
Q

The equilibrium constant for the transfer of a proton from water to a base is called________?

A

The base hydrolysis constant (Kb)

36
Q

The solubility of a solid compound in water is described by the _______?

A

Solubility product constant (Ksp)

37
Q

The equilibrium constant for the formation of a complex ion is called______?

A

The formation constant (Kf)

38
Q

Spectator ions

A

Ions that undergo no significant reactions

Chemistry (6 decks)

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