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MCAT Gen Chem > Phases > Flashcards

Phases Flashcards

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1
Q

Ideal gases have what types of intermolecular forces?

A

No IMF’s

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2
Q

Decreasing order of IMF’s

A

Solids -> liquids -> gases

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3
Q

Condensation reaction

A

Gas to liquid

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4
Q

Fusion reaction

A

Solid -> liquid (melting)

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5
Q

Sublimination

A

Solid -> gas

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6
Q

Deposition

A

Gas -> solid

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7
Q

What happens when heat is absorbed?

A

Internal KE increases, entropy increases

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8
Q

What is the triple point?

A

The temperature and pressure where all three phases coexist

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9
Q

What is the critical point?

A

The temperature and pressure above which the difference between liquids and gases is no longer distinct

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10
Q

What happens to the freezing and melting point of ice as pressure increases?

A

The freezing and melting point decrease

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11
Q

Heart energy to change phase

A

q = n∇H

Units are in kJ

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12
Q

Heat for temperature change

A

q = mc∇ T

m = mass (Units are in J)

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13
Q

What effect does external pressure have on vapor pressure?

A

External pressure has no effect on vapor pressure

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14
Q

Boiling point is where

A

Vapor pressure = Atmospheric pressure

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15
Q

What is a solution?

A

A homogeneous mixture of two or more substances

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16
Q

What are the relative quantities of solutes and solvents?

A

Solutes are normally present in smaller quantities

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17
Q

How do strong/weak/non- electrolytes dissociate in water?

A

Strong electrolytes dissociate completely

Weak electrolytes partially dissociate

Non-electrolytes don’t dissociate

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18
Q

Vant Hoff factor (i)

A

The # of particles per mole of a substance

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19
Q

What is the Vant Hoff factor of sugar (C6H12O6), NaCl, Ca(NO3)2, and HF respectively

A

Sugar = 1, it won’t dissociate in water

NaCl = 2

Ca(NO3)2 = 3

HF = 1 < i < 2

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20
Q

Electrolyte process of dissociation

A

Agitation (endothermic) → Dissociation (endothermic) → Solvation (exothermic)

Dissociation is net exothermic

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21
Q

Polar non-electrolytes dissolving process

A

Agitation → solvation

22
Q

Nonpolar non-electrolytes

A

Agitation

23
Q

What is solubility?

A

The amount of substance that can dissolve in a solvent at a specific temperature

Changes in temperature alter solubility

24
Q

What are the relative concentrations of an unsaturated solution?

A

[solute] < solubility

Additional solute will dissolve

25
Q

What are the relative concentrations of a saturated solution?

A

[solute] = solubility

No additional solute will dissolve

26
Q

What are the relative concentrations of a supersaturated solution?

A

[solute] > solubility

Additional solute causes excess to precipitate

27
Q

What are the solubility rules of solids and liquids in water?

A

Solubility is proportional to temperature

Solubility is not affected by pressure

28
Q

What are the solubility rules of a gas in water?

A

Solubility is indirectly proportional to temperature

Solubility is proportional to temperature

29
Q

What electrolytes are always soluble in water? (6 items)

A

Alkali metals

Hydrogen

Ammonium (NH4+)

Nitrate (NO3-)

Acetate (CH3COO-)

Perchlorate (ClO4-)

30
Q

What electrolytes are usually insoluble in water? (6 items)

A

Silver

Lead

Mercury

Carbonate (CO32-)

Phosphate (PO43-)

Sulfur

31
Q

What happens when you pair an insoluble electrolyte with a soluble electrolyte?

A

The substance is soluble in water

32
Q

Where would dissolved gas be highest in a shallow body of water?

A

The bottom

33
Q

How would you increase the solubility of sugar in water?

A

The substance is a solid

Increase the temperature

34
Q

What are the components of the kinetic molecular theory of gases? (4 things)

A

An ideal gas has zero IMF’s

An ideal gas has particles of negligible mass (Helium)

An ideal gas has an average kinetic energy proportional to temperature

Ideal gas is favored at high temperature and low pressure because it minimizes the interactions of the particles

35
Q

What are the 4 pressure conversions?

A

1 atm = 101,000 Pa = 760 mmHg = 760 torr

36
Q

What are the volume equivalents?

A

1 L = .001 m3 = 1,000 mL = 1,000 cm3

37
Q

What are the conditions at STP?

A

0 degrees C (273 K) and 1 atm

38
Q

What are the standard state conditions?

A

25 degrees C ( 298 K), 1 atm

39
Q

What is the combined gas law?

A

P1V1 / T1 = P2V2 / T2

40
Q

How does pressure relate to volume?

A

Pressure is inversely proportional to volume

41
Q

How does Temperature relate to volume?

A

Temperature is proportional to volume

42
Q

How does temperature relate to pressure?

A

Temperature is proportional to pressure

43
Q

If the pressure and volume of a 2 mole sample of Helium is doubled, what is the new temperature if the initial temperature is 27 degrees C

A

*Plug in simple numbers

P1V1 / T1 = P2V2 / T2

1 atm 1 L / 300 K = 2 atm * 2 L / T

T = 1200 K

44
Q

What is Avogadro’s Law

A

Volume is proportional to the number of moles

45
Q

What is the volume of NH3 made from 3 L N and 3 L H at STP?

N2 + 3 H2 = 2N2H3

A

Take the number of moles of the limiting reagent and multiply if by the ratio of that reagent to the product

3 moles H2 x 2 mol NH3 / 3 mol H2 = 2 mols NH3

46
Q

What is the ideal gas law?

A

PV = nRT

R = 0.08 L

47
Q

If given the number of moles near STP, how would you most simply find the volume?

A

V = 22.4 L/mol near STP

22.4 x # moles

48
Q

How do pressure and volume of ideal gases compare to real gases?

A

Pideal > Preal

VIdeal > Vreal

49
Q

What is the Real Gas Law?

A

(P + n2/V2*a) (V - nb) = nRT

50
Q

Partial pressure equation and mole fraction equation

A

Pa = Xa*Ptotal

Xa= na/ntotal

51
Q

What is Graham’s law? (rate of diffusion)

A

The rate of diffusion (v) is inversely proportional to molecular weight

v1/v2 = Square root of (mw2/mw1)

MCAT Gen Chem (2 decks)

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