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Review > Review 6 > Flashcards

Review 6 Flashcards

1
Q

Relate standard ∆G˙ with ∆Grxn

A

∆G˙ = ∆Grxn + RTlnQ

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2
Q

Negative enthalpy is exothermic or endothermic?

A

Exothermic

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3
Q

Positive enthalpy is exothermic or endothermic?

A

Endothermic

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4
Q

What phase has the highest entropy?

What has the lowest?

A

Gas = highest entropy, solid = lowest

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5
Q

Under what conditions are gases real and not ideal?

A

Low pressure

High temperature

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6
Q

Ideal gases

A

No attractive forces b/w them

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7
Q

Graham’s Law of effusion

A

Higher molar mass => leaks more slowly through hole

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8
Q

How do you calculate pressure of gas?

A

Subtract vapor pressure of water from its measured pressure

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9
Q

Average kinetic energy is directly proportional to _____

A

Temperature of gas in kelvin

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10
Q

Another equation for n (moles)

A

n = m/M

  • m = mass of gas
  • M = molar mass
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11
Q

How many cm^3 in a liter?

A

1000

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12
Q

Coordinate covalent bond

A

Bond where one molecules acts as Lewis acid (accepts electrons) and the other acts as Lewis base (donates e-)

  • Play role in complex ions
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13
Q

Common ion effect on solubility

A

Decreases solubility

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14
Q

Raoult’s Law (effect of solutes on boiling point and vapor pressure)

A

Solutes => decrease vapor pressure => increase boiling point

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15
Q

Effect of solutes on freezing point

A

Depresses freezing point by disrupting crystal lattice => more energy must be taken out

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16
Q

Solubility of gases in liquids is directly proportional to ______

A

Atmospheric pressure

17
Q

What molecules would have positive deviation from Raoult’s Law?

Negative deviation?

A

Unlike molecules => want to get out of solution => higher vapor pressure than expected = positive deviation

Like molecules = negative deviation

18
Q

Formation of complex ions => what?

A

More molecules of solid will dissociate (ions are being removed from solution due to complexing)

19
Q

Solution

A

Mixture of uniform appearance (homogenous)

  • Can be solid-solid, gas-solid, gas-gas, etc.
20
Q

Molality

A

Moles of solute/kg of solvent

21
Q

Boiling point/freezing point change

A

∆T = iKm

  • i = # of ions it dissociates into
  • K = initial boiling/freezing point
  • m = molality
22
Q

How many liters of 2 M Ba(OH)2 are needed to titrate a 4 L solution of 6 M H3PO4?

A

18 L

  • NaVa = NbVb
  • N (normality) = molarity * number of OH or H+
  • Na of Ba(OH2) = 2*2 = 4
  • Nb of H3PO4 = 3*6 = 18
23
Q

3.4 x 10^-6 Ka correlates to what pH?

A
  1. 66

- 6 - 0.34 = 5.66 pH

24
Q

Gram equivalent weight of phosphoric acid

A

33g

  • H3PO4
  • Molar mass = 98g
  • 3 protons => divide molar mass by 3 for weight of one acid/base
25
Q

log(1/10)

A

-1

26
Q

Acids ending in -ic are derivatives of anions ending in _____

A
  • ate => -ic

- Attic

27
Q

Acids ending in -ous are derivatives of anions ending in _____

A
  • ite => -ous

- Iteous

28
Q

What has more O: -ate or -ite?

A

-ate

29
Q

Chlorate chemical formula

Chlorite chemical formula

A

ClO3-

ClO2-

30
Q

Oxidation = ____ (more/less) bonds to O or ____ bonds to H

A

More bonds to O

Less bonds to H

31
Q

Disproportionation reaction

A

Element appears with different oxidation states in two different products

32
Q

Concentration cell

A

Type of galvanic cell where both electrodes are made of same material

33
Q

E˙cell = ____ - _____

A

E°cell = E°red,cathode − E°red,anode

34
Q

Electrolytic cell process

A

Break compound into constituent ions

  • Cations => cathode
  • Anions => anode
35
Q

Relate ∆G and E

A

∆G = -nFE

  • n = moles of electrons (from half reactions)
  • F = Faraday’s constant
36
Q

In a galvanic cell, species with higher reduction potential is _____

A

Reduced

37
Q

Relate ∆G and Keq

A

∆G = -RTln(Keq)

38
Q

If Keq

A

Negative lnKeq => positive ∆G

39
Q

Lead-acid batteries have ____ energy density

Ni-CD batteries have ____ energy density

NiMH batteries have _____ energy density

A

Low energy density

Ni-Cd = higher energy density

NiMH = highest energy density

Review (13 decks)

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