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Organic Chem > equilibrium > Flashcards

equilibrium Flashcards

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1
Q

chemical equilibrium

A

when the forward and backward rates of a reaction at equal

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2
Q

what happens to the concentration of products and reactants at chemical equilibrium

A

they remain constant

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3
Q

physical equilibrium

A

the same chemical with physical processes in equilibrium

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4
Q

what is the general form to describe equilibrium

A

K=Prod/Reactants

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5
Q

if the K value is greater than one, what will the reaction favor

A

it will favor products

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6
Q

if the K value is less than one, what will the reaction favor

A

the reactants

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7
Q

Heterogenous equilbrium reactions

A

species are not in the same phase

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8
Q

Homogenous equilibrium reactions

A

species are in the same phase

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9
Q

what is the equation to convert Kc into Kp

A

Kp = Kc(0.0821 T)^delta n Kc = concentration equilibrium T = temp in kelvin delta n = change in the number of gas moles

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10
Q

What equation is used for Kc

A

Kc = [prod]^n/[react]^n

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11
Q

what equation is used for Kp

A

Kp = Pprod^n/Preact^n

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12
Q

how to find delta n

A

gaseous moles product - gaseous moles reactants

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13
Q

what is the first step in solving an equilibrium probelm

A

making sure the equation is balanced

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14
Q

how are pure solids and liquids represented in equilibrium equations

A

both are 1

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15
Q

what is the K formula if there are multiple elementary steps

A

A + B C + D EF/AB, CD cancels out

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16
Q

what must be quoted when stating a K value

A

temperature and the balanced equation

17
Q

why must temperature be specified for a K value

A

increasing T increases the frequency factor, more collisions means more energy, which means a different equilibrium

18
Q

what are equilibrium equations used for

A
  • determining the extent of a reaction - determining the concentration of species
19
Q

when is the Q value used

A

when you are given a K value and you need to compare that value to experimental data

20
Q

Q>K

A

there is too much product and some of it will be broken down back into reactants (equilibrium shifts to reactants)

21
Q

Q=K

A

equilibrium

22
Q

Q

A

there are too many reactants, the amount of product will increase (equilibrium shifts to the product)

23
Q

what does ICE stand for

A

Initial, Change, Equilibrium

24
Q

when should an ICE table be used

A

to determine the concentration of species at equilibrium

25
Q

steps to solve ICE problems

A

1) Balance the reaction 2) write the expression 3) fill given values into the ICE table 4) set unknowns as an expression of x 5) solve

26
Q

factors that impact chemical equilibrium

A
  • temp - pressure - volume - concentration
27
Q

Le Chatelier’s principle

A

if an external stress is applied to a system at equilibrium, the system adjusts in such a way that the stress is reduced and the system reaches a new equilibrium

28
Q

according to Le Chatelier’s principle, if concentration is increased what will happen to equilibrium

A

it will shift away from which ever side of the equation had the increase

29
Q

according to Le Chatelier’s principle, if pressure or volume are increased, what will happen to equilibrium

A

it will shift toward whatever side of the reaction produces the fewest number of moles

30
Q

what is the effect of an inert gas on equilibrium

A

no effect

31
Q

what will an increase in temperature do to equilbrium

A

it will shift to favor the direction that is endothermic (+H)

32
Q

what will a decrease in temperature do to equilibrium

A

it will shift to favor the direction that is exothermic (-H)

33
Q

how can heat be thought of as a concentration in relation to equilibrium

A

if you add “heat” to one side of the reaction, the equilibrium will shift away from the added energy

34
Q

what is the effect of a catalyst on equilibrium

A

no effect, it helps both sides of the reaction

Organic Chem (8 decks)

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