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DAT Chemistry > Ch 5: Solutions + Ch 6: Gases + Ch. 7 Liquids and Solids > Flashcards

Ch 5: Solutions + Ch 6: Gases + Ch. 7 Liquids and Solids Flashcards

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1
Q

Units for pressure = ?

A

1 atm = 760 torr = 760 mmHg

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2
Q

Gases behave more ideally under ___ pressure and ____ temperature

A

low pressure
high temperature
(this is stated by the ideal gas theory an kinetic molecular theory)
- at higher temperature collisions are more elastic and there will be no attraction among molecules

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3
Q

What does the kinetic molecular theory state?

A
  1. gas molecule do not have volume
  2. there are no attraction forces between molecules
  3. collisions are elastic = no intermolecular forces = no loss of energy
  4. average kinetic energy depends on temperature
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4
Q

What is the R gas constant?

A

8.3145 J/mol K

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5
Q

What is avogadro’s law?

A

volume is proportional to moles

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6
Q

Boyle’s law?

A

pressure is inversely proportional to volume

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7
Q

Charles’ law?

A

volume is proportional to temperature

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8
Q

Dalton’s law of partial pressure?

A

mix of gases, total pressure of mixture = summation of partial pressure of individual gases (molar fraction of gas times total pressure)

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9
Q

Graham’s Law of Effusion

A

rate of effusion of a gas inversely proportional to square root of it’s molar mass

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10
Q

___ bond are between tightly packed metal ions and a pool of electrons

A

metallic

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11
Q

What forces hold liquids together?

A

intermolecular forces:

  • van der waals
  • dipole-dipole/polar
  • hydrogen bonding
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12
Q

A substance at very high temperature and pressure is at it’s

A

critical point.

= supercritical fluid with gaseous and liquid properties

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13
Q

What is the freezing point depression formula?

A

dT freezing = i Kfreezing M

M = mol solute / mass of solvent

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14
Q

If a type of solute is not important bt the van’t Hoff factor is important, what type of property is this?

A

colligative

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15
Q

When two substances with different vapor pressures are combined, vapor pressure of mixture changes is according to who’s law?

A

Raoult’s law

P total = Pa + Pb

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16
Q

Lower vapor pressure when adding salt in comparison to water.
Lower vapor pressure means fewer liquid particles vaporized.
This yields…

A

boiling point elevation

dt = iKboilingM

17
Q

What is sensible heat?

A

energy required to increase the temperature of a substance

18
Q

Rate of dissolution = rate of precipitation at…

A

molar solubility

solid form precipitated and dissolved form are at equilibrium

19
Q

For solids in liquids:

incr temperature means _____ solubility

A

increase solubility

20
Q

For gases in liquids:

incr temperature means ______ solubility

A

decrease solubility

21
Q

For gases in liquids:

increase pressure means ____

A

increase solubility

22
Q

Soluble or insoluble: CsOH

A

soluble

group 2 salts are always soluble

23
Q

Soluble or insoluble:

NH3NO2

A

soluble

nitrate, perchlorate, acetate are always soluble (think nitrate dissolving in nitrogen cycle

24
Q

Soluble or insoluble:

AgClO4

A

soluble

silver, lead, mercury is insoluble except with nitrates, perchlorates, acetates

25
Q

High vapor pressure means ____ intermolecular forces

A

weaker
therefore, substances will more easily evaporate
= more volatile

26
Q

What are the four properties of colligative properties?

A
  1. Vapour pressure depression
  2. Boiling Point elevation
  3. Freezing point depression
  4. Osmotic Pressure
27
Q

What is the difference between dissolution and solvation?

A

dissolution: solvent-solvent and solute-solute intermolecular attractions that need to be broken
solvation: solvent-solute intermolecular attractions that need to be formed to form a soluution

28
Q

What is stronger hydrogen bond or ion-dipole?

A

ion-dipole

-note hydrogen bond is a very strong type of dipole-dipole

29
Q

Intermolecular forces play a role in boiling points how so?

A

stronger intermolecular forces that hold molecules together, more energy required to separate i.e. boiling point is higher

30
Q

How do intermolecular forces play a role in determining solubility?

A

solute must be surrounded by solvent (solvated)

solute-solvent bonds stronger than > solute-solute or solvent-solvent bonds

31
Q

Boiling point: True or false

weaker intermolecular forces will have higher boiling point

A

False
stronger force = higher bp
need more energy to break strong force

32
Q

Boiling point: True or false

between nonpolar molecules the one with more extended molecule will have higher boiling point

A

True

as length of hydrocarbonds increase, boiling point and melting point increases

33
Q

Boiling point:

Do smaller or larger molecules have higher boiling points?

A

larger = higher bp

DAT Chemistry (9 decks)

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