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AH Chemistry > 2.1 Introducting the equilibrium constant > Flashcards

2.1 Introducting the equilibrium constant Flashcards

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1
Q

what is Kc

A

the equilibrium values are expressed as concentrations of mole l-1

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2
Q

the equilibrium values are expressed as concentrations of mole l-1

A

Kc

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3
Q

Kp

A

the equilibrium values are expressed as partial pressures

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4
Q

the equilibrium values are expressed as partial pressures

A

partial pressure

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5
Q

does K have units

A

never

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6
Q

what is the equilibrium constant

A

the ratio of the concentration of products divided by the concentration of reactants

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7
Q

the ratio of the concentration of products divided by the concentration of reactants

A

the equilibrium constant

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8
Q

what gives an indication of the extent a reaction has progressed / the position of the equilibrium

A

the equilibrium constant

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9
Q

what does the equilibrium constant show

A

gives an indication of the extent a reaction has progressed / the position of the equilibrium

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10
Q

the greater the value of K, …

A

the greater the concentration of products compared to reactants

thus, the further a reaction has gone to the products

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11
Q

the greater ______, the greater the concentration of products compared to reactants

thus, the further a reaction has gone to the products

A

the value of K

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12
Q

what is K equation

A

K = C^c x D^d / A^a x B^b

where… aA + bB —> cC + dD

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13
Q

K = C^c x D^d / A^a x B^b

where… aA + bB —> cC + dD

A

equation for K

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14
Q

what does the equilibrium constant give no indication on

A

the rate at which equilibrium is achieved

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15
Q

what does it mean if the value of K (equilibrium value) is < 10^-3

A

effectively no reaction, it is too slow

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16
Q

what does it mean when K = 1

A

products = reactants

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17
Q

what does it mean if the value of K (equilibrium value) is from 10^-3 to 10^3

A

significant quantities of reactions and products at equilibrium

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18
Q

when is there significant quantities of reactions and products at equilibrium

A

K is between 10^-3 to 10^3

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19
Q

what is K when there is effectively no reaction, it is too slow

A

value of K (equilibrium value) is < 10^-3

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20
Q

in the equilibrium constant equation, what is []

A

the equilibrium concentration in mol l^-1

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21
Q

concentrations of pure solids and liquids are constant or not constant

A

constant

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22
Q

what dont appear in the equilibrium constant equation and why

A

pure solids and liquids as they are given the value 1

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23
Q

what happens to K when concentration or pressure are changed?

A

nothing

24
Q

changes in pressure only affect what reactions

A

reactions involving gases

25
Q

what doesnt effect K

A

concentration or pressure

26
Q

what affects K

A

temperature

27
Q

is K temperature dependant

A

yes

28
Q

endothermic reactions: increasing the temperature

A

favours the products

the equilibrium shifts right

29
Q

when are the products favoured and

the equilibrium shifts right when changing temperature

A

increasing the temperature in endothermic reactions

30
Q

what happens to K when product concentration increases

A

increases

31
Q

increasing temperature in exothermic reactions

A

favours the reactants

equilibrium shifts to the left

32
Q

favours the reactants

equilibrium shifts to the left in what reactions when changing temperature

A

increasing temp in exothermic reactions

33
Q

value of K when increasing temp in exothermic reactions

A

the value of K decreases

34
Q

value of K when increasing temp in endothermic reactions

A

K increases

35
Q

what must be done to maintain the equilibrium in constant

A

the composition of the equilibrium changes

36
Q

what happens if you increase the concentration of a substance

A

the value of Kc will be affected

37
Q

increasing conc. of a reactant…

A

moves equilibrium to the right

38
Q

increasing conc. of a product…

A

moves equilibrium to the left

39
Q

decreasing conc. of a product…

A

equilibrium moves to the right

40
Q

decreasing conc. of a reactant…

A

moves equilibrium to the left

41
Q

particles in a volume and pressure relationship

A

as the number of particles in a volume increases, the greater the pressure they exert

42
Q

increasing pressure…

A

equilibrium moves to the side with fewer gaseous molecules

43
Q

equilibrium moves to the side with fewer gaseous molecules

A

increasing pressure

44
Q

decreasing pressure

A

equilibrium moves to the side with greater number of gaseous molecules

45
Q

equilibrium moves to the side with greater number of gaseous molecules

A

decreasing pressure

46
Q

enthalpy change of exothermic reaction

A

-

47
Q

enthalpy change of endothermic reaction

A

+

48
Q

exothermic affect on equilibrium summary

A

negative enthalpy change

increase temp: to the left
decrease temp: to the right

49
Q

negative enthalpy change

increase temp: to the left
decrease temp: to the right

A

exothermic

50
Q

endothermic reaction and equilibrium

A

enthalpy change: +

increase temp: to the right
decrease temp: to the left

51
Q

enthalpy change: +

increase temp: to the right
decrease temp: to the left

A

endothermic

52
Q

endothermic reactions with increase in temp and K

A

K increases

53
Q

exothermic reactions with increase in temp and K

A

K decreases

54
Q

heterogeneous equilibrium

A

pure solids or pure liquids are taken as being constant and given the value of 1

55
Q

pure solids or pure liquids are taken as being constant and given the value of 1

A

heterogeneous equilibrium

AH Chemistry (7 decks)

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