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Chem 102 > FINAL study guides > Flashcards

FINAL study guides Flashcards

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1
Q

A spontaneous reaction implies…

A
  • ΔK > 1
  • ΔG < 0
  • ΔSuniverse > 0
  • E∅ > 0
  • NOT: ΔHrxn < 0
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2
Q

What does normal boiling pt / normal freezing pt signify?

A

Normal ⇒ 1 atm pressure

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3
Q

When does boiling occur (regarding the vapor pressure of the liquid)?

A

When vapor pressure (v. p.) of liquid equals external pressure
- for normal boiling point: Vpressure = 1 atm.
- ΔHvap = P

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4
Q

What are “standard conditions”?

A
  • 1 M aqueous species
  • P = 1 atm
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5
Q

dissolution (solubility/ionization) reaction

A

solid <–> aq + aq
- ex: AgI (s) <–> Ag+ (aq) + I- (aq)
- ex: Fe(OH)3 (s) <–> Fe3+ (aq) + 3(OH-) (aq)

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6
Q

dissolution (solubility/ionization) reactions can go in ___ direction(s)

A

forwards and backwards directions
<—–>

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7
Q

precipitation reaction

A

(aq) + (aq) –> solid
- Ag+ (aq) + I- (aq) –> AgI (s)
- Fe3+ (aq) + 3(OH-) (aq) –> Fe(OH)3 (s)

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8
Q

precipitation reactions go in __ direction(s)

A

ONLY forwards direction
—–>

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9
Q

water auto-ionization reaction (water dissociation reaction)

A

H2O (l) <—> H+ (aq) + OH- (aq)
- Kw = 1 x 10^14 @ 25C

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10
Q

will a buffer form?

A

CA/CB in comparable amounts
- if not comparable, do SICE table
SA/WB or WA/SB, SICE, CA/CB in comparable amounts?

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11
Q

is the aqueous solution (compound) acidic?

A

1) cancel out ions from SA/SB
2) are the remaining ions cations (+) or anions (-)?
- cations (+) = acidic
- anions (-) = basic

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12
Q

acid with smallest pKa corresponds to the _____ with largest ____ because pKa + pKb = 14 for conjugates.

A
  • conjugate base
  • pKb
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13
Q

The larger the pK value, the ___ that species is

A
  • weaker
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14
Q

pH at equivalence point of SA/SB

A

pH = 7

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15
Q

pH at equivalence point of a SB/ WA

A

pH > 7

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16
Q

pH at equivalence point of SA/WB

A

pH < 7

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17
Q

∆G = 0…

A
  • at phase transition
  • at equilibrium
  • Q = K
  • boiling
  • ∆H = T∆S
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18
Q

For an exothermic reaction…

A

reaction loses heat –> ∆Hrxn < 0
entropy of surrounding ↑ –> ∆Ssurr > 0

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19
Q

boiling point increases w/ increasing…

A
  • increasing molar mass
  • increasing polarity
  • increases greatly w/ hydrogen bonding
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20
Q

What are the general properties of a water-soluble molecule or ion?

A
  • monovalent charge (charge = ±1)
  • presence of polar bonds
  • if “long; several hydroxyl groups (OH) throughout
  • number of carbons ≤ 5 (linear chain)
  • heterocyclic rings ( nitrogen or oxygen as well as carbons at vertices of hexagon)
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21
Q

SO3 gas dissociation reaction:

A

2 SO3 (g) → 2 SO2 (g) + O2 (g)

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22
Q

if a question asks about a “shift in equilibrium”, you need…

A

K and Q and to compare

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23
Q

(multi-step reaction energy plot): the rate-limiting step usually…

A

involves the larger activation energy “barrier”
- largest Ea / largest “hump”

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24
Q

(multi-step reaction energy plot): How many transition states are involved?

A

how many humps on the graph

25
Q

(multi-step reaction energy plot): Which step has the largest forward rate constant?

A
  • largest forward rate constant = smallest activation energy (smallest Ea)
26
Q

breaking bonds…

A
  • requires energy
  • endothermic
  • ΔH > 0
27
Q

making bonds…

A
  • releases energy
  • exothermic
  • ΔH < 0
28
Q

Which species are likely soluble in water? is another way of asking

A

Which pairs of species could, in principle, hydrogen bond with each other in a solution

29
Q

Which of these gases could be liquefied (by pressure alone) at 25C…?

A

any gas w/ Critical Temp. (Tc) > 25C

29
Q

Which of these gases could be liquefied (by pressure alone) at 25C…?

A

any gas w/ Critical Temp. (Tc) > 25C

30
Q

ALL equilibrium constant questions require…

A

ICE TABLE

31
Q

nuclear reactions (ex: beta-plus decay) are ___ order

A

1st order

32
Q

any natural or molecular compound (glucose, sucrose, alcohol, NH3), “I” (number of ions) always =…

A

1

33
Q

cathode =

A

reduction = oxidizing agent

34
Q

anode =

A

oxidation = reducing agent

35
Q

the strongest base has…

A

the largest Kb, the smallest Ka

36
Q

electrolyte

A

a compound that conducts an electric current when it is in an aqueous solution or melted
- covalent, molecular

37
Q

electrolytic (i) = ?

A

(i) = 2

38
Q

non-electrolytic (i) = ?

A

1

39
Q

as Ksp increases, molar solubility…

A

increases

40
Q

as Ksp decreases, molar solubility…

A

decreases

41
Q

(reaction profile): slow =

A

tall

42
Q

(reaction profile): fast =

A

small

43
Q

condensation and deposition = ΔS =

A

ΔS < 0

44
Q

ΔS = ? for:
solid –> liquid, liquid –> gas, solid –> gas

A

ΔS = (+)

45
Q

How could the buffering capacity be improved?

A

increase mols of acid and base

46
Q

E = () = spontaneous

A

E = (+)

47
Q

E = () = non spontaneous

A

E = (-)

48
Q

the second law of thermodynamics states…

A

entropy (ΔS) of the universe = (+)
- ΔS(surroundings) = -ΔS(system)

49
Q

T/F: for the reversible process, ΔS(surroundings) = -ΔS(system)

A

TRUE

50
Q

T/F: for any spontaneous process, ΔS(universe) > 0

A

TRUE

51
Q

T/F: the entropy of the universe is conserved in any process

A

FALSE

52
Q

if a solution decreases in temp…ΔH = ?

A
  • endothermic = ΔH = (+)
53
Q

if a solution dissolves….ΔS = ?

A
  • dissolve = disorder = ΔS = (+)
54
Q

the oxidation state of a pure element is ALWAYS..

A

zero (0)

55
Q

the substance that is oxidized or reduced are ALWAYS

A

reactants

56
Q

if something is being oxidized or reduced it pertains to….

A

the element/ion

57
Q

if something is an oxidizing agent or reducing agent it pertains to…

A

the whole compound

Chem 102 (6 decks)

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