Unit 3 Equilibrium Review Flashcards

1
Q

Le Chateliers principle

A

when a stress is applied to a system in dynamic equilibrium, the equilibrium will shift to relieve the stress

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2
Q

exothermic

A

energy is a product

ΔH is negative because you lose energy

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3
Q

endothermic

A

energy is a reactant

ΔH is positive because you gain energy

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4
Q

dynamic equilibrium

A

a state of balance in a CLOSED system at constant temperature and there are no changes at the visible level but there is a constant change at the molecular level

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5
Q

Closed system

A

a reaction system in which no matter can enter or exit. Only a closed system can reach an equilibrium.

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6
Q

Steady State

A

is an open system that has no properties that are directly observable; however, this is because any materials that leave the system are immediately replaced

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7
Q

three stresses that can be applied to an equilibrium system

A

concentration
temperature
volume/pressure

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8
Q

concentration [ ]

A

NO SOLIDS
shifts away from increase
shifts toward decrease
(arrow goes towards increase. ex:

↓ → ↑

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9
Q

temperature

A

shifts away from increase
shifts toward decrease
(arrow goes towards increase. ex:
↓ → ↑)

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10
Q

volume/pressure

A

GASES ONLY
increase pressure favours side with less moles
increase volume favours side with more moles

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11
Q

catalysts

A

catalyst is a substance that speeds
up the rate of reaction without being used up in the reaction.

*Catalysts will NOT have any effèct on an equilibrium position because they speed up the reaction equally in both directions.

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12
Q

concentration graph

A

vertical line and a hill

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13
Q

temperature graph

A

all hills

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14
Q

pressure graph

A

all vertical lines

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15
Q

keq

A

[products]/[reactants]

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16
Q

keq is only

A

gases and aqueous
no solids or liquids

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17
Q

if keq is larger than 1

A

A value for Keq significantly.
larger than one means that products are favored over reactants.

18
Q

if keq is less than one

A

A value of Keq significantly less than one it means that reactants are favoured over products

19
Q

if keq is very close to 1

A

A value of Keq very close to 1 means that the (reactant] ~ [product)

20
Q

spontaneous

A

products are favoured

large equilibrium constant (keq)

> > > > > 1

21
Q

non spontaneous

A

reactants are favoured

small equilibrium constant

««1

22
Q

ICE charts

A

Initial: if not known, put 0

Change: + or - ___x (one side will be +, one side will be -) (__x will be the # in front of chemical)

Equilibrium: if not given is I + C

23
Q

dissociation

A

is reversible physical change

24
Q

net ionic

A

the non reversible chemical change where an insoluble ppt is formed

25
solubility
the mass of a given substance that can be dissolved by a specific solvent at a given temp
26
saturated solution
the solvent has the maximum amount of solute dissolved in it can hold at that specific temp ON the line
27
unsaturated solution
the solvent can still dissolve more solute at that temperature UNDER the line
28
supersaturated solution
a solvent can hold more than the maximum amount of solute at a given temp ABOVE the line
29
equilibrium
balanced state of a reversible reaction in which there is NO observable change the rate of the forward reactor equals that of the reverse reaction
30
Le Chateliers principle pt 2
if a system at equilibrium is subjected to an external stress, the equilibrium will shift so as to minimize that stress
31
in heat, equilibrium will shift…
in the case of heat, the equilibrium will shift in the direction which the added heat is used up
32
what happens to the solubility of solids when you increase temperature
when you increase the temperature of a solid, the solubility increases solids are endothermic
33
what happens to the solubility of gases when you increase temperature
the solubility decreases upon heating exothermic
34
common ion effect
the solubility of an ionic substance in water is decreased when another substance containing ONE of the ions in the solution (the common ion) is added
35
predicting precipitate’s: if Qsp is larger than Ksp
a precipitate WILL form
36
predicting precipitate’s: if Qsp is smaller than Ksp
a precipitate will NOT form the solution is unsaturated
37
predicting precipitate’s: if Qsp is equal to Ksp
the solution is saturated and no change will occur
38
when it gives you solubility
calculate ksp
39
when it gives you ksp
find solubility by substituting x for the chemicals
40
ksp
only products