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Chem 106 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

equilibrium constant

A

K

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2
Q

what does the equilibrium constant change with?

A

temp

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3
Q

what does a large K value mean?

A

reaction is product-favored

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4
Q

what does a small K value mean?

A

reaction is reactant-favored

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5
Q

what does chemical equilibrium mean?

A

forward rate=reverse rate

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6
Q

reaction quotient

A

Q

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7
Q

what causes system stress?

A
  • addition/subtraction of a reactant/product
  • altering partial pressures
  • change in the volume while keeping a constant temp
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8
Q

what does an increase in temp in exothermic reactions mean?

A

a lower K value (they produce less)

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9
Q

what happens when Q>K?

A

the reaction occurs in the reverse direction

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10
Q

what affects equilibrium?

A
  • change in the amount of product/reactant
  • change in temp
  • change in the volume of gas
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11
Q

which way does the reaction move when you add more reactant?

A

towards the products

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12
Q

what happens to a reaction when you change the volume of a gas?

A

change to the partial pressure

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13
Q

how does a decrease of 2 of the volume affect the partial pressure?

A

increases the partial pressure by 2

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14
Q

what does a decrease in the volume/increase in pressure move the reaction towards?

A

side with the lower number of moles

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15
Q

what does an increase in the volume/decrease in pressure move the reaction towards?

A

side with more moles

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16
Q

what does an exothermic reaction move the reaction direction towards?

A

reactants

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17
Q

what does an endothermic reaction move the reaction towards?

A

products

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18
Q

what does an increase in temperature do to the direction of a reaction?

A

forwards

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19
Q

what does a decrease in temperature do to the direction of a reaction?

A

reverse

20
Q

RICE

A

reaction, initial concentration, changes, equilibrium concentration

21
Q

if a reaction quotient has a smaller value than the equilibrium constant

A

the reaction will continue to make more products

22
Q

increasing the temp in an exothermic reaction results in

A

more reactants and fewer products

23
Q

Bronsted-Lowery acid definition

A

H ion donor

24
Q

Bronsted-Lowery base definition

A

H ion acceptor

25
Q

strong acid

A
  • completely ionized
  • K value is to large to calculate
  • goes only in forward direction
26
Q

weak acid

A
  • partially ionized
  • K is small enough to be calculated and used
  • can go in reverse direction
27
Q

conjugate base-acid pairs

A

differ by only a proton

28
Q

the stronger the acid

A

the higher the K value

29
Q

what does charge delocalization do?

A

stabilizes

30
Q

autoionization

A

produces small equal concentrations of H30 and OH ions in pure water

31
Q

what does a small K value mean

A

reaction doesn’t happen in the forward direction

32
Q

strongest acid that can exist in water?

A

H3O

33
Q

are strong acids all the same in water?

A

yea

34
Q

what are strong acids converted into in water?

A

H3O

35
Q

why are stable things weak?

A

not reactive

36
Q

oxidation number

A

the greater the number of oxygen atoms the stronger the acid

37
Q

the lower the pH…

A

the more acidic

38
Q

pH neutral

A

7

39
Q

pH>7

A

basic

40
Q

pH<7

A

acidic

41
Q

how does the oxidation number affect the K value?

A

makes it rise

42
Q

pH+pOH=?

A

14

43
Q

what does water auto ionize into?

A

OH and H3O

44
Q

if [H3O] > [OH] is it acidic or basic?

A

acidic

45
Q

if [H30] < [OH] is it acidic or basic?

A

basic

46
Q

the weaker the acid…

A

the stronger the conjugate base

Chem 106 (13 decks)

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