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Chemistry 121 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

Define pressure, which all gases have

A

Force pushing against a surface, F/A

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2
Q

SI unit of pressure

A

Pascal = 1kg/ms^2 = 1n/m^2

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3
Q

Device used to measure the pressure of the atmosphere

A

Barometer, uses mercury

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4
Q

How many pascals in 1 atm

A

101,325 Pa

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5
Q

How many millimeters of mercury in 1 atm

A

760 mmHg

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6
Q

How many torrs in 1 atm

A

760 torr

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7
Q

How many pounds per square inch in 1 atm

A

14.7 lb/in^2

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8
Q

Pressure of a water barometer is proportional to

A

(column height)(density)

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9
Q

Two types of manometers, which is more convenient

A

Closed end, gas pressure is measured directly versus in a open end manometer where you need to know pressure of the atmosphere

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10
Q

What is Boyle’s law

A

Volume of a fixed volume of gas at a constant pressure is inversely proportional to the applied pressure

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11
Q

Volume of a gas is in proportion to (involving pressure)

A

1/P

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12
Q

What is Charles’s law

A

The volume of the gas increases linearly with temperature

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13
Q

Volume of a gas is in proportion to (involving temp)

A

T

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14
Q

-293.15 degrees C was deduced to be the coldest possible temp because why

A

A colder temp would yield a negative volume

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15
Q

What is Gay-Lussac’s law

A

Pressure of a gas increases linearly to the Kelvin temperature when volume & moles are constant

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16
Q

Pressure of a gas is in proportion to (involving temp)

A

T

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17
Q

What is Avagadro’s law

A

The volume of a gas increase linearly to the number of moles

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18
Q

Volume of a gas is in proportion to (involving moles)

A

n

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19
Q

What is the universal gas constant

A

PV/nT

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20
Q

What is the ideal gas equation

A

PV=nRT

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21
Q

Standard temp & pressure of a gas

A

273.15 K at 1 atm

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22
Q

1 mole of any gas at 0 degrees C & 1 atm occupies what volume

A

22.41 L

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23
Q

R involving L*atm

A

.08206 Latm/molK

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24
Q

R involving cal

A

1.987 cal/mol*K

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25
Q

R involving J

A

8.314 J/mol*K

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26
Q

R involving m^3*Pa

A

8.314 m^3Pa/molK

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27
Q

R involving L*torr

A

62.36 Ltorr/molK

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28
Q

How to find molar mass of a gas

A

dRT/P

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29
Q

Formula for finding mole fraction relating pressures of gases

A

Pa/Pt

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30
Q

Pressure of gas must take into account the pressure of what

A

Water

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31
Q

The average kinetic energy of molecules in a gas are directly proportional to what

A

Kelvin Temp

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32
Q

Average KE is in proportion to

A

T

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33
Q

SI unit for energy

A

1 J = 1kg*m^2/s^2=1Nm

34
Q

In the ideal gas equation, PV is equal to what

A

Average KE

35
Q

Distribution of molecular speeds (molecular kinetic energies) set forth by

A

Maxewell-Boltzmann

36
Q

How to find root-mean-square speed

A

sqrt of 3RT/M

37
Q

Rates of diffusion of gases are what to the square roots of their molar masses

A

Inversely proportional, r1/r2=sqrt(M2/M1)

38
Q

Equation that takes into account the adjustments of pressure and volume for real gases

A

Van der Waals

39
Q

Define energy

A

Ability to do work

40
Q

1 calorie is how many J

A

4.184 J

41
Q

First law of thermodynamics

A

Law of conservation of energy

42
Q

Open system

A

Allows for exchange of mass & energy with surroundings

43
Q

Closed system

A

Allows for the transfer of energy but not mass with the surroundings

44
Q

Isolated system

A

No transfer of mass or energy with surroundings

45
Q

Internal energy

A

Total energy of a system (ΔE)

46
Q

Can we measure the absolute internal energy

A

No, just changes

47
Q

What adds together to get internal energy of a system

A

q (heat) + w (work)

48
Q

If heat is added, q is

A

+

49
Q

If heat is removed, q is

A

-

50
Q

If work is done ON the system (system compressed), then w is

A

+

51
Q

If work is done BY the system (system expands), then w is

A

-

52
Q

Expansion of a gas against a constant pressure is referred to what

A

Mechanical work

53
Q

Work equation for compressing/expanding a gas

A

W=-PΔV

54
Q

In gas expansion, ΔV is

A

+

55
Q

In gas compression, ΔV is

A

-

56
Q

Process that gives off heat is called

A

Exothermic, system loses heat & surroundings gain heat

57
Q

Process where heat flows from surroundings to the system

A

Endothermic, system gain heat & surroundings lose heat

58
Q

Heat energy is called what when the system is at a constant pressure

A

Enthalpy (ΔH)

59
Q

In an endothermic reaction, ΔH is

A

+, heat flows into system

60
Q

In an exothermic reaction, ΔH is

A

-, heat flows out of system

61
Q

At constant volume, there is no work done so

A

ΔE=q

62
Q

At constant pressure, work can be done on or by the system (compression/expansion)

A

ΔE=q-PΔV

63
Q

Relationship between ΔH and ΔE at a constant pressure

A

ΔH=ΔE+PΔV

64
Q

Does enthalpy change depend on the physical states of substances

A

Yes

65
Q

Is enthalpy an extensive or intensive property

A

Extensive

66
Q

What is a calorimeter

A

Measures the amount of heat generated or consumed

67
Q

Heat capacity (extensive property)

A

Amount of heat required to raise the temp of matter 1 K (heat absorbed/ΔT)

68
Q

Molar heat capactiy (intensive property)

A

Amount of heat required to raise the temp of one mole of a substance 1 K (heat absorbed/mol*ΔT)

69
Q

Specific heat (intensive property)

A

Amount of heat required to raise the temp of one gram of a substance 1 K (q/m*ΔT)

70
Q

Constant pressure calorimeter

A

q=ΔH (~ΔE)

71
Q

Constant volume calorimeter

A

q=ΔE

72
Q

To calculate Δreaction using a calorimeter

A

q(p)=C*ΔT=ΔH

73
Q

If ΔH is negative, then do products or reactants have less energy content (PE)

A

Products have less

74
Q

Standard conditions for thermochemistry (ΔHdegree)

A

25 degrees C, 1 atm

75
Q

State functions

A

Depend only on conditions, not on the process to reach said conditions

76
Q

Examples of state functions

A

Pressure, temp, volume, chemical composition, internal energy, enthalpy

77
Q

Modifying chemical reactions to get ΔH uses what

A

Hess’s Law of heat summation

78
Q

Gases with standard enthalpy change of 0 (ΔHfdegrees)

A

C(graphite), beer (all g except I & Br), all metals (s) (except Hg), Hg(l)

79
Q

Define (ΔHfdegrees)

A

Standard enthalpy change for formation of a substance from the elements in their standard states

80
Q

How to find ΔHdegrees of a reaction

A

Add up the standard heat of formation of products and subtract the standard heat of formation of the reactants

81
Q

Compare ΔH and ΔE for reactions using the Δn

A

ΔE=ΔH-Δn(RT) or ΔE=ΔH-PΔV

Chemistry 121 (5 decks)

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