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Chemistry > Chapter 10 > Flashcards

Chapter 10 Flashcards

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1
Q

What are vapors?

A

gaseous state of any substance that normally exists as a liquid or solid

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2
Q

What does the volume of gas=?

A

volume of tis containter

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3
Q

How are gases highly compressible?

A

pressure is applied to a gas its volume readily decreases.

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4
Q

Are solids or liquids readily compressible?

A

no

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5
Q

What kind of a mixture does gases form?

A

forming homogeneous mixtures

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6
Q

Do all gases exert pressure on any surface if they are in contact?

A

yes

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7
Q

How do the molecules of gas move?

A

chaoticllay, colliding with each other and with the walls of their container

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8
Q

How do you find the pressure of gas?

A

P=F/A

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9
Q

What does A stand for on the equation to find pressure of gas?

A

area

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10
Q

What does the F in the equation for pressure of gas stand for?

A

force

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11
Q

What energy of gas overides its gravitational force?

A

thermal energies of motion(kinetic energies)

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12
Q

What is atmospheric pressure?

A

as the force exerted by the atmosphere on a given surface area

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13
Q

How do you find the magnitude of atmospheric pressure?

A

F=ma

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14
Q

What does a stand for in the magnitude eof atmospheric pressure equation?

A

acceleration

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15
Q

What is the equation to find gravitational force of the atmosphere?

A

F-=mg

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16
Q

What does g stand for in the graviational force equation?

A

9.8 m/s^2

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17
Q

What is the units for gravitoanl force?

A

N or 1kg-m/s^2

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18
Q

How do you go from kPa to bar?

A

100kPa= 1bar

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19
Q

How does height realte to atmospheric pressure?

A

the height will increase or decrease as atomspheric pressure increases or decreases

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20
Q

What is standard atmospheric pressure?

A

corresponds to the typical pressure at sea level 760 torr

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21
Q

What does gas volume do as pressure decreases?

A

increases

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22
Q

As altitude increases what does atmospheric pressure do?

A

decreases

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23
Q

What is boyle’s law?

A

the volume of a fixed quantiy of gas maintined at constant temperature is inversely proportional to the pressure

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24
Q

What is boyles law equation?

A

PV=constant

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25
Q

When the volume of gas increases what does the temperature do?

A

increases

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26
Q

What does charles law states?

A

the volume of a fixed amount of gas maintined at constant pressure is directly proportional to its absolute tempature

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27
Q

What is charles law equation?

A

V/T= constant

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28
Q

What is avogadro’s hyopthesis?

A

equal volumes of gases at the same temperature and pressure contain equal number of molecules

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29
Q

What is avagdro’s law?

A

the volume of a gas maintined at constant temperature and pressure is directly proptotional to the number of moles of the gas

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30
Q

What is avagdro’s equation?

A

V/n constant

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31
Q

What is the ideal gas equation?

A

PV=nRT

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32
Q

What is R in the ideal gas equation?

A

gas contant

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33
Q

What does R equal in the ideal gas law equation?

A

0.08206 L-atm/Mol x K

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34
Q

What are the standard temparute and pressure?(STP)

A

T=0˚c and P=1atm and V=22.41L

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35
Q

What is the equation to find pressure when n and t is a constant

A

P1V1=P2V2

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36
Q

What is the combined gas law equation?

A

P1V1/T1= P2V2/T2

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37
Q

What is the equation to find density?

A

d=PM(molar mass)/RT

38
Q

What happens to the density as molar mass increases?

A

density increases

39
Q

What happens to the denisty of the gas as temperature increases?

A

decreases become less dense

40
Q

How can you determine the molar mass of gas with density?

A

M(molar mass)= dRT/P

41
Q

What is partial pressure?

A

the pressure exerted by a particular gas in a mixture?

42
Q

What dalton’s law of partial pressure?

A

A law stating that the total pressure of a mixture of gases is the sum of the pressures that each gas would exert if it were present alone

43
Q

How do you find the total pressure of a mixture of gases?

A

Pt=P1 + P2 + P3+….

44
Q

How do you calculate the partial pressure of a gas when given the P and the mol precnet?

A

divide the mole percent by 100 and then times it by the pressure

45
Q

What is the kinetic molecular theory of gases?

A

a set of assumptions about the nature of gases

46
Q

What do large number of molecules in gas do?

A

are in continous random motion

47
Q

What is negligible molecular volume?

A

the combined volume of all the molecules of the gas is negligible relative to the toal volume in which teh gas is contained

48
Q

What negligible forces?

A

attractive and repulsive forces between gas molecules

49
Q

What does average kinetic energy do as temperature remains constant?

A

doesnt change with time

50
Q

What is the average kinetic energy of the molecules proportional to?

A

the absolute temperature

51
Q

What determines the magnitude of pressure?

A

how often and how forcefully the molecules strike the walls

52
Q

When two gases are at the same tempertature what is the average kinetic temperature?

A

the same

53
Q

What does molecular motion do as temerpature increases?

A

increases

54
Q

What does the range of molecular speed do as temeprature increases?

A

increases

55
Q

When there is an increase in volume at constant temperature and the pressure decreases what happens to teh average kinetic energy?

A

is unchanged

56
Q

When there is an increase in volume at constant temperature and the pressure decreases,
What happens to the distance between molecules?

A

move a longer distance between collisions

57
Q

AS temperature icnreases at constant volume casues pressure to increase,
What happens to the average kinetic energy?

A

increase in average kinetic energy

57
Q

When there is an increase in volume at constant temperature and the pressure decreases.
What happens to the amount of collisions?

A

fewer wall collisions

58
Q

ASs temperature icnreases at constant volume casues pressure to increase,
What happens to the number of collisions?

A

more collisions with walls

59
Q

ASs temperature icnreases at constant volume casues pressure to increase,
What happens to the momentum?

A

it increases causing more forceful collisions

60
Q

How do you find rms speed?

A

√3RT/M(molar mass)

61
Q

What does the rms speed do as molar mass decreases?

A

increases

62
Q

How do you find probable speed of a gas?

A

√2RT/M(molar mass)

63
Q

How do you find the average speed of a gas?

A

√8RT/πM(molar mass)

64
Q

What will speed do as temperature increases?

A

increase

65
Q

What is effusion?

A

the escape of a gas through an orfice or a hole

66
Q

What is diffusion

A

the spreading of one substance throughput a space or throughout a second substance

67
Q

What units does molar mass have to find the speed of gases?

A

kg/mol

68
Q

What does R equal in the speed equations?

A

8.314 J/mol-k or kg-m^2/s^2-mol-k

69
Q

What is the effusion rate inversely proportional to?

A

the square root of its molar mass

70
Q

How do you find effusion rate?

A

√M2/M1(molar mass)

71
Q

If a gas is lighter does it have a high or low effusion rate?

A

high

72
Q

What is effusion rate directly proportional to?

A

the rms speed of molecules

73
Q

What is another equation to find effusion rate?

A

rms1/rms 2 or √3RT/M1/ RT/M2

74
Q

How do you use the ideal gas law to solve for n(moles)

A

PV/RT=n

75
Q

What does temerpature cause ideal behavior to do?

A

the deviation from ideal behavior increases

76
Q

What is the van der waals equation?

A

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

77
Q

Why is there a pressure adjustment for the nonideal behavior?

A

molecules attract and repel each other

78
Q

Why is there a volume adjustment for the nonideal behavior?

A

molecules occupy some space on their own

79
Q

When using the rms speed equation what is the molar mass units?

A

kg/mol

80
Q

When using the rms speed equation what does the R constant equal?

A

8.314

81
Q

In the rms speed equation what does the Tempature units have to be?

A

Kelvins

82
Q

How to find the rate of effusion?

A

Divide the molar masses and then take the square root

√M2/M1

83
Q

Which of the following will lead to an increase in the mean free path of gas molecules in a closed container?

A

Increase V
without changing T
Open valve to release half the molecules without changing T
or V
.

84
Q

Is ionic compounds boiling points alwyas smaller or bigger?

A

bigger

85
Q

What is the first step in determing which boiling point is smaller or larger?

A

seeing if they are polar or not

86
Q

If a molecule is polar and the other molecule is nonpolar who has the bigger boiling point?

A

polar molecule

87
Q

What is the second step in determing which boling points is smaller or larger?

A

By the molecular weight if both are nonpolar which ever molecule has a larger weight

88
Q

What is the third step in determing which boiling point is smaller or larger? If they are both polar

A

if they are both polar looking at the other intermolecular forces

89
Q

If one molecule can do hydrogen bonding and is polar and another molecule is polar but can’t do hydrogen bonding which molecule has the largerst boiling point?

A

the molecule that can do hydrogen bonding

Chemistry (13 decks)

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