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Chemistry > Chapter 19 - Equilibrium > Flashcards

Chapter 19 - Equilibrium Flashcards

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1
Q

What does a larger Kc value mean ?

A

The further the position of equilibrium is towards the products

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2
Q

What does a smaller Kc value mean ?

A

The further the position of equilibrium is towards the reactants

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3
Q

What do the units of Kc depend upon ?

A

They depend upon the number of concentration terms that are in the equilibrium constant term

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4
Q

How do you work out the units of Kc ?

A
  • Substitute units into the expression for Kc
  • Cancel common units and show the final units on a single line
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5
Q

What are the two main types of equilibria ?

A

Homogenous and heterogenous

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6
Q

What does a homogenous equilibrium contain ?

A

It contains equilibrium species that all have the same state or phase

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7
Q

What does a heterogenous equilibrium contain ?

A

A heterogenous equilibrium contains equilibrium species that have different states or phases

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8
Q

What concentrations does a homogenous equilibria contain ?

A

It contains concentrations of all species

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9
Q

What concentrations does a heterogenous equilibria contain ?

A
  • Any species that are in solid and liquid state are omitted from the Kc expression
  • They are automatically incorporated within the overall equilibrium constant
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10
Q

What states do the species have to be for them to be in the Kc expression ?

A

g or aq

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11
Q

What is a mole fraction ?

A

The proportion of the volume of a gas to the total volume of gases in the mixture

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12
Q

How do you work out the mole fraction ?

A

Mole fraction χ(A) = number of moles of A / total number of moles in the gas mixture

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13
Q

What does the sum of the mole fractions equal to ?

A

Should equal to 1

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14
Q

What does p stand for ?

A

The partial pressure of a gas

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15
Q

What does P stand for ?

A

The total pressure

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16
Q

What is the partial pressure ?

A

The contribution that the gas makes towards the total pressure

17
Q

How do you work out the partial pressure ?

A
  • p(A) = Mole fraction of A x total pressure P
  • p(A) = x(A) x P
18
Q

What does the sum of the partial pressures equal ?

A

It equals the total pressure

19
Q

What state does Kp only include ?

A

Only includes gases because only gases have partial pressures

20
Q

With the equilibrium H(2) + I(2) -> 2HI, what is the expression for Kp?

A

Kp = p(HI)^2 / p(H(2)) x p(I(2))

21
Q

What does the magnitude of an equilibrium constant represent?

A

The extent of an equilibrium

22
Q

Where does the equilibrium position shift if the concentration of a species increases ?

A

Shifts in the direction that decreases the concentration

23
Q

Where does the equilibrium position shift if the pressure is increased ?

A

Shifts towards the side with fewer gaseous moles

24
Q

Where does the equilibrium position shift if the temperature increases ?

A

Position shifts in the endothermic direction

25
Q

What does K = 1 indicate ?

A

Equilibrium halfway between reactants and products

26
Q

What does K = 100 indicate ?

A

Equilibrium well in favour of the products

27
Q

What does K = 1x10^-2 indicate ?

A

Equilibrium well in favour of the reactants

28
Q

What is K at a set temperature ?

A

Constant and does not change despite any modifications in conc, pressure or the presence of a catalyst

29
Q

What is the only condition that will cause K to change ?

A

Temperature

30
Q

What is the effect on K when the temperature is increased and the forward reaction is exothermic?

A
  • Equilibrium constant decreases
  • Equilibrium shifts to the left
31
Q

What is the effect on K when the temperature is increased and the forward reaction is endothermic?

A
  • Equilibrium constant increases
  • Equilibrium shifts to the right
32
Q

What effect does increasing pressure have on a reaction with fewer moles of gaseous products than reactants?

A
  • Products increase
  • Reactants decrease
  • Equilibrium shifts to the right
33
Q

What effect does increasing pressure have on a reaction with more moles of gaseous products than reactants?

A
  • Products decrease
  • Reactants increase
  • Equilibrium shifts to the left
34
Q

What effect does increasing pressure have on a reaction with the same number of moles of gaseous products and reactants?

A
  • No change
  • Equilibrium stays the same
35
Q

What is the effect of a catalyst on the equilibrium constant?

A
  • Catalyst affects the rate but not the equilibrium
  • Equilibrium is reached faster but position does not change

Chemistry (29 decks)

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