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Chem 195n Physical Chemistry C3 > Gases > Flashcards

Gases Flashcards

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1
Q

What is the major difference between the states of matter?

A

The arrangement of particles

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2
Q

Solid have

A

Definite volume
Definite Shape

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3
Q

Liquid have

A

Definite volume
Indefinite shape

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4
Q

Gas have

A

Indefinite volume
Indefinite shape

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4
Q

What is the physical significance of having the gas’ arrangement of particles?

A

It is compressible

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5
Q

The volume of a gas changes significantly with:

A

Pressure, temperature, gases flow freely, gases generally

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6
Q

Characteristics of gases

A

Gases flow freely, gases generally mix in all proportions

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7
Q

Major Characteristics of gases

A

Expansibility
Compressibility
Pressure
Effect on heat
Diffusibility

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8
Q

The collision of gases particles on the walls of the container gives rise to

A

Pressure

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9
Q

SI unit of pressure

A

Pascal

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10
Q

Formula for pressure

A

Force/ area

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11
Q

This may either be in terms of grams or moles

A

Amount

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12
Q

SI unit of amount

A

Moles

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13
Q

Formula for amount of substance

A

Grams/ molar mass

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14
Q

The amount of space that is to be occupied by gaseous state

A

Volume

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15
Q

SI unite of volume

A

Cubic meter

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16
Q

Relates to the average kinetic energy of gaseous particles

A

Temperature

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17
Q

SI unit of temperature

A

Kelvin

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18
Q

Celsius to Fahrenheit

A

(9/5 x C) + 32

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19
Q

Fahrenheit to Celsius

A

(5/9 x F) - 32

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20
Q

A parameter that describes gases, which have an SI unit of Joule

A

Energy

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21
Q

equivalent of 1 cal to joule?

A

4.184 J

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22
Q

What is the values for Universal Gas Constant in correct units?

A

8.314 J/ mol K
0.08205 L atm/ mol K
1.986 cal/ mol K

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23
Q

Pressure in STP

A

1 atm/ 101.3 kPa

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24
Q

Temperature in STP

A

0 C/ 273.15 K

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25
Q

Molar volume in STP

A

22.4 L/ atm

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26
Q

No. of moles in STP

A

1 mol

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27
Q

Enumerate the 5 kinetic molecular theory of gases

A
  1. Gases travel in straight lines and random directions
  2. Small particle sizes to be negligible
  3. Atomic collision are perfectly elastic, KE is conserved
    4.Gas particles do not repel or attract
  4. KE of gas is directly proportional to Kelvin Temperature
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28
Q

What are the parameters that describes gases

A

Pressure, temperature, amount, volume

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29
Q

Describe charles law and formula

A

States that there is a direct relationship between the gas volume and temperature
V1/T1 = V2/T2

30
Q

Describe boyles law and formula

A

States that there is an indirect relationship between the gas volume and pressure
V1P1 = V2P2

31
Q

Describe Gay-lussac law and formula

A

States that there is a direct relationship between the gas pressure and temperature
P1/T1 = P2/T2

32
Q

Describe avogadros law and formula

A

States that there is a direct relationship between the gas volume and number of moles
V1/N1 = V2/n2

33
Q

The total pressure of a mixture of gases is equal to the sum of the pressures of all the gases present.

A

Daltons Law of Partial Pressure

34
Q

Give formula of Partial Pressure

A

P total = (n1 + n2 + n3 …) (RT/V)

35
Q

Phenomena which results in the net
movement of particles from a region
of high concentration to a region of
low concentration in response to a
concentration gradient

A

Graham’s law of diffusion

36
Q

Under same conditions of constant temperature and pressure, the rates of diffusion of different gases are ____________ to the square roots of
their molecular masses.

A

inversely proportional

37
Q

Formula for Grahams law of diffusion

A

rate2/rate1 = Square root M1/M2

38
Q

net movement of particles through
an opening smaller than the mean
free path of the gas (no collisions)

A

Effusion

39
Q

net movement of particles from a
region of high to low concentration
as influenced by collisions

A

Diffusion

40
Q

Formula for Graham law of effusion

A

Effusionrate2/ Effusionrate1 = Square root M1/M2

41
Q

Formula for average KE of a gas molecule

A

e = 3RT/ 2N0

42
Q

In deriving the kinetic gas equation, what
was the assumption made regarding the
velocities of the gaseous molecules?

A

Constant velocity for all molecules.

43
Q

The velocity place in the utmost peak in of molecular velocity graph

A

Most probable velocity

44
Q

Located after the most probable velocity

A

average velocity

45
Q

The farthest velocity from the most probable velocity

A

Root mean square velocity

46
Q

Distance travelled by a molecule between two successive collisions

A

THE MEAN FREE PATH

47
Q

Relationship of mean free path to
pressure;
volume; and
temperature

A

Indirectly Proportional
Indirectly Proportional
Directly Proportional

48
Q

If collision diameter is large, mean free path will _____

A

Smaller

49
Q

Relationship of collision diameter to the mean free path

A

If collision
diameter is large, mean free path will be smaller!

50
Q

amount of heat required to raise the temperature of one gram of a substance by 1°C
may be measured at constant volume or constant pressure

A

Specific Heat Ratio of Gases

51
Q

The Vibrational and rotational degrees of freedom in monoatomic gases

A

Zero

52
Q

volume kept constant while allowing pressure to increase

A

Specific Heat at Constant Volume

53
Q

pressure kept constant while allowing volume to increase

A

Specific Heat at Constant Pressure

54
Q

Two applications of heat in Specific Heat at Constant Pressure

A
  1. Increase KE of molecules
  2. Performing expansion work
55
Q

What specific conditions do ideal gases work in?

A

High temperature
Low pressure

56
Q

The deviation of the compression factor from unity is a measure of

A

Nonideality of gas

57
Q

At very low pressures, Z will be
approximately ____ for all the gases

A

1

58
Q

Deviation from ideality becomes
much _____ at high temperatures

A

lesser

59
Q

At low pressures and high temperatures, real gases approach _____ and so obey the ideal gas equation

A

ideality

60
Q

At low temperatures and sufficiently high pressures, the gas behaves as

A

Real gas

61
Q

Larger deviations are primarily observed when the gas is closer to its

A

liquefaction point

62
Q

Ideality satisfied at ____
temperatures and ____ pressures

A

high, low

63
Q

Because of the existence of attractive forces, pressure is ______ for a real gas

A

lesser

64
Q

Since the non-volume postulate is no longer valid, volume is _____ for a real gas

A

Larger

65
Q

Related to
the effective /excluded volume

A

van der Waal’s Constants, b

66
Q

Related to the strength of the
interactions between your molecules

A

van der Waal’s Constants, a

67
Q

When gases are compressed, it

A

Liquefies

68
Q

Temperature above which it cannot be liquefied no matter how much pressure is applied

A

CRITICAL TEMPERATURE, Tc

69
Q

Minimum pressure required to liquefy the gas at its critical temperature

A

CRITICAL PRESSURE, Pc

70
Q

Volume occupied by a mole of the gas at the critical temperature and critical pressure.

A

CRITICAL VOLUME, Vc

71
Q

When a gas is at its critical temperature and critical pressure the gaseous and liquid phase lose their discernible boundary
(known as the critical phenomenon) and the gas is in its

A

critical state

72
Q

What are the 5 Kinetic Molecular Theory of Gases

A
  1. Gases travel in straight lines and in random directions
  2. Gases particles are so small that their size is negligible
  3. Atomic or molecular collisions are perfectly elastic and so kinetic energy is conserved
  4. The gas particles are assumed not to attract or repel each other.
  5. The average kinetic energy of the gas particles is directly proportional to the Kelvin temperature.
73
Q

In deriving the kinetic gas equation, what was the assumption made regarding the velocities of the gaseous molecules?
.

A

Constant velocity for all molecules

Chem 195n Physical Chemistry C3 (3 decks)

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