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MCAT > General Chemistry Ch 8. Gas Phase > Flashcards

General Chemistry Ch 8. Gas Phase Flashcards

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MCAT flashcards
1
Q

Gas phase

A

Least dense phase of matter, fluids, conform to the shape of their container, easily compressible

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2
Q

Pressure equivalencies

A

1 atm = 760 mmHg = 760 torr = 101.325 kPa

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3
Q

Simple mercury barometer

A

Measures incident (usually atmospheric) pressure, as pressure increases, more mercury is forced into the column increasing its height, as pressure decreases, mercury flows out of the column under its own weight, decreasing its height

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4
Q

Standard temperature and pressure

A

273 K and 1 atm

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5
Q

Ideal gases

A

Assume negligee mass and volume of gas molecules, equimolar amounts of two gases will occupy the same volume at the same temp and pressure, at STP, one mole of ideal gas occupies 22.4 L

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6
Q

Avogadros principle

A

A special case of the ideal gas law for which the pressure and temperature are held constant, it shows a direct relationship between the number of moles of gas and volume

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7
Q

Boyles law

A

Special case of the ideal gas law for which temperature and number of moles is held constant, shows an inverse relationship between pressure and volume

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8
Q

Charles law

A

Special case of the ideal gas law for which pressure and number of moles is held constant, shows a direct relationship between temperature and volume

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9
Q

Gay-Lussacs Law

A

Spacial case of the ideal gas law for which volume and number of moles are held constant, shows a direct relationship between temperature and pressure

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10
Q

Combined gas law

A

Combination of Boyles, Charles, and gay-lussacs laws, shown and inverse relationship between pressure and volume along with direct relationship between pressure and volume with temperature

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11
Q

Daltons laws of partial pressures

A

States that individual gas components of mixture of gases will exert individual pressures in proportion to their mole fractions, the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases

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12
Q

Mole fractions

A

-

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13
Q

Henrys laws

A

States that the amount of gas dissolved in solution is directly proportional to the partial pressure of that gas at the surface of a solution

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14
Q

Kinetic molecular theory

A

Attempts to explain the behavior of gas particles, makes the following assumptions:

Gas particles have negligible mass, gas particles do not have intermolecular attractions or repulsions, gas particles undergo random collisions with each other and the walls of the container, collisions between gas particles and the walls of the container are elastic, the average kinetic energy of the gas particles is directly proportional to temperature

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15
Q

Grahams law

A

Describes the behavior of gas diffusion or effusion, stating that gases with lower molar masses will diffuse oe effuse faster than gases with higher molar masses at the same temperature

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16
Q

Diffusion

A

The spreading out of particles from high to low concetrations

17
Q

Effusion

A

Movement of gas from one compartment to another through a small opening under pressure

18
Q

Real gases

A

Deviate from ideal behavior under high pressure, low volume, or low temperature conditions

19
Q

Moderately high pressure, low volume, low temperature real gases

A

Will occupy less volume than predicted but the ideal gas law because the particles have intermolecular attractions

20
Q

Extremely high pressure, low volume, low temperature real gases

A

Will occupy more volume than predicted by the ideal gas law because the particles occupy physical space

21
Q

van der Waals equation of state

A

Used to correct the ideal gas law for intermolecular attractions and molecular volume

22
Q

Ideal gas law equation

A

PV = nRT

23
Q

Density of a gas equation

A

rho = m/V=PM/RT

24
Q

Combined gas law equation

A

P1V1/T1 = P2V2/T2

25
Q

Avogadros principle equation

A

n/V = k or n1/V1 = n2/V2

26
Q

Boyles law equation

A

PV= k or P1V1=P2V2

27
Q

Charles law equation

A

V/T=k or V1/T1=V2/T2

28
Q

Gay Lussacs law equation

A

P/T=k or P1/T1=P2/T2

29
Q

Daltons law total pressure from partial pressures equation

A

PT = PA+PB+PC…

30
Q

Daltons law partial pressure from total pressure equation

A

PA=XA*PT

31
Q

Henrys law equation

A

[A] = k_H*P_A or [A1]/P1=[A2]/P2 = k_H

32
Q

Average kinetic energy of a gas equation

A

KE = 1/2mv^2=3/2K_b*T

33
Q

Root mean square speed equation

A

u_RMS = sqrt(3RT/M)

34
Q

Grahams law equation

A

r1/r2 = sqrt(M2/M1)

35
Q

van der Waals equation of state

A

(P+n^2*a/V^2)(V-nb) = nRT

MCAT (67 decks)

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