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MCAT Chem > Chem #8 > Flashcards

Chem #8 Flashcards

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1
Q

gases and liquids are ____

A

fluids

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2
Q

sphygmomanometer

A

medical devices that measure blood pressure (mmHg)

 Normal BP: 120 systolic and 90 diastolic

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3
Q

understand how a barometer works

A

 Many medical devices use the same conceptual design of a barometer.
• Atmospheric pressure creates a downward force on the pool of mercury at the base of the barometer while the mercury in the column exerts an opposite force (its weight) based on its density.
• When the external air exerts a higher force than the weight of the mercury in the column, the column rises, and vice versa.

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4
Q

ideal gas

A

hypothetical gas with molecules that have no intermolecular forces and occupy no volume

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5
Q

ideal gas law

A

shows relationship between Pressure, Volume, moles, and temperature for an ideal gas.
o Used to analyze the relationships between variables when certain ones are held constant.

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6
Q

combined gas law

A

: changes in temperature, volume, and pressure of a gas

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7
Q

what are the requirements of an ideal gas?

A

no intermolecular forces and occupy no volume

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8
Q

real gas

A

: deviate from ideal behavior at high pressures (low volumes) and low temperatures because of intermolecular forces or volume effects.

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9
Q

when do real gases deviate from ideal behavior?

A

high pressure (low volume) and low temperature

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10
Q

the gas laws show that ____

A

that all gases show similar physical characteristics and behavior irrespective of their particular chemical identity.

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11
Q

the ideal gas constant for the ideal gas law can be rounded to ____

A

0.8

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12
Q

the ideal gas constant for the ideal gas law can be rounded to ____

A

0.08

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13
Q

how to solve for molar mass at STP given density

A

o Molar mass equals the density at STP x 22.4 L/mol

 Holding mass constant for calculations using combined gas law.

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14
Q

avogadro’s principle

A

all gases at a constant temperature and pressure occupy volumes that are directly proportional to the number of moles of a gas present.
 As the number of moles of gas increases, the volume increases in direct proportion.

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15
Q

boyle’s law

A

for a given gaseous sample held at constant temperature (isothermal conditions) and constant moles, the volume of the gas is inversely proportional to pressure.
 As pressure increases, volume decreases.

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16
Q

charle’s law

A

at constant pressure, the volume of a gas is proportional to its absolute temperature, expressed in K. n and P are constant
 As temperature increases, volume increases.

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17
Q

gay lussac’s law

A

at constant volume, the pressure of a gas is proportional to its absolute temperature in kelvins. n and V are constant
 As temperature increases, pressure increases.

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18
Q

dalton’s law of partial pressures

A

o When two or more gases that do not chemically interact are found in one vessel, each gas will behave independently of the others.
 Each gas will exert pressure independently of the other gases, as if it were the only gas present: partial pressure of the gas.

the total pressure of a gaseous mixture is equal to the sum of the partial pressures of the individual components.
 Partial pressure of a gas is related to its mole fraction

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19
Q

partial pressure of a gas is related to its ____

A

mole fraction

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20
Q

henry’s law

A

 The solubility of a gas will increase with increasing partial pressure of a gas.

21
Q

vapor pressure

A

: the pressure exerted by evaporated particles above the surface of a liquid
 Vapor pressure from the evaporated molecules forces some of the gas back into the liquid phase, and equilibrium is reached between evaporation and condensation.

22
Q

what are the assumptions of the kinetic molecular theory

A

o 1. Gases are made up of particles with volumes that are negligible compared to the container volume.
o 2. Gas atoms or molecules exhibit no intermolecular attractions or repulsions.
o 3. Gas particles are in continuous, random motion, undergoing collisions with other particles and the container walls.
o 4. Collisions between any two gas particles (or between particles and the container walls) are elastic, meaning that there is conservation of both momentum and kinetic energy.
o 5. The average kinetic energy of gas particles is proportional to the absolute temperature of the gas (in kelvins), and it is the same for all gases at a given temperature, irrespective of chemical identity or atomic mass.

23
Q

kinetic molecular theory

A

explain the behavior of gases.

24
Q

The higher the temperature, the ____ molecules move. The larger the molecules, the ____ they move.

A

faster

slower

25
Q

The average kinetic energy of a gas particle is proportional to the ____ of the gas.

A

absolute temperature

26
Q

The average kinetic energy of a gas particle is proportional to the ____ of the gas.

A

absolute temperature

27
Q

Maxwell-Boltzmann Distribution Curve

A

shows the distribution of gas particle speeds at a given temperature.

28
Q

compare diffusion and effusion

A

Diffusion: when gases mix with one another
Effusion: when a gas moves through a small hole under pressure.
Both conditions are slower for larger molecules AND USE THE SAME EQUATION

29
Q

graham’s law

A

under isothermal and isobaric conditions, the rates at which two gases diffuse are inversely proportional to the square routes of their molar masses

30
Q

diffusion

A

the movement of molecules from high concentration to low concentration through a medium (such as air or water)

31
Q

effusion

A

: the flow of gas particles under pressure from one compartment to another through a small opening.
• For two gases at the same temperature, the rates of effusion are proportional to the average speeds.

32
Q

what are the deviations of real gases from the ideal gas law due to high pressure?

A

o Pressure of gas increases, condensation point is reached, gases condense
o At moderately high pressure, a gas’s volume is less than would be predicted by the ideal gas law due to intermolecular attraction.
o At extremely high pressure, the gases take up a larger volume than would be predicted by the ideal gas law.
o The ideal gas law assumes that a gas can be compressed to take up zero volume which is not physically possible.

33
Q

what are the deviations of real gases from the ideal gas law due to low temperature?

A

o Temperature of gas decreases, condensation point is reached, gases condense.
o Same as above:
 At moderately low temperature, the gas will have a smaller volume than what would be predicted. DUE TO IMF
 At extremely low temperature, gases will occupy more space than predicted by the ideal gas law. DUE TO particles can’t be compressed to 0 volume.

34
Q

van der waals equation of state: a term

A

corrects for the attractive forces between molecules (van der waals term for attractive forces)
 Small and less polarizable < larger and more polarizable < largest for polar molecules

35
Q

van der waals equation of state: b term

A

corrects for the volume of the molecules (van der waals term for big particles)
 larger molecules have larger values for b

36
Q

a term vs b term van der waals equation of state

A

a term is generally much larger than b
a term: attractive forces
b term: volume

37
Q

how are the characteristics of gases different than liquids?

A

gases have the ability to expand to any volume and can be easily compressible.
they are very distanced with weak intermolecular forces.

38
Q

what 4 variables define the state of a gas?

A

pressure, volume, moles, temperature

39
Q

In _____ law, pressure and volume are inversely related

A

Boyle’s

40
Q

Equal amounts of all gases at the same temperature and pressure will occupy _____ volume

A

equal

41
Q

in ___ law, volume and temperate are directly proportional

A

Charle’s

42
Q

adding up all of the partial pressures gives the ____

A

total pressure for the vessel

43
Q

the value of Henry’s constant depends on _____

A

the identity of the gas

44
Q

all of the ideal gas laws use what units for temperature?

A

Kelvin

45
Q

the gas laws demonstrate that all gases _____

A

show similar physical characteristics and behavior irrespective of their particular chemical identity

46
Q

the kinetic molecular theory of gases predicts that heavier gasses diffuse ______ than lighter ones because of their different average speeds

A

more slowly

47
Q

All gas particles have the same _____ at the same temperautre

A

average kinetic energy

48
Q

trends with increased pressure and decreased temperature regarding ideality

A

initially the gasses have lesser volume then would be predicted and then they would have greater volume than would be predicted.

49
Q

1000 cm^3 = ?

A

1 L

MCAT Chem (12 decks)

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