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Chemistry R120 > Chapter 10 > Flashcards

Chapter 10 Flashcards

1
Q

What are the 6 characteristics of gases?

A

nonmetals | simple molecular formulas | low masses | expand spontaneously to fill the volume of a container | highly compressible | form homogenous mixtures

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2
Q

What allows for the existence of the characteristics that gases have?

A

because the gas molecules are far apart

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3
Q

What are vapors?

A

substances that exists as solids and liquids under ordinary conditions and can exist in the gaseous state

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4
Q

What is pressure?

A

the force gas molecules exert on the walls of the container (outward push against walls)

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5
Q

What is the equation for pressure?

A

P = Force / Area of container

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6
Q

What is atmospheric pressure?

A

force atmosphere exerts on a given surface area

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7
Q

What is the equation for force?

A

F = ma

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8
Q

What is the value of acceleration?

A

9.8 m/s^2

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9
Q

Who is Blaise Pascal?

A

French scientist who studied pressure

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10
Q

What is the unit of 1 Pascal (Pa)?

A

N/m^2

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11
Q

How many Pascals is 1 bar?

A

10^5 Pa

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12
Q

What is a barometer?

A

a 760 mm long tube filled with mercury = the height of Hg is a measure of atmospheric pressure and changes as the atmospheric pressure changes

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13
Q

Who invented the barometer?

A

Evangelista Torricelli

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14
Q

What is standard atmospheric pressure?

A

corresponds to the typical pressure at sea level

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15
Q

What is the unit for atmospheric pressure?

A

1 atm

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16
Q

How many mmHg = torr = Pa = kPa = bar is 1 atm?

A

1 atm = 760 mmHg = 760 torr = 1.01325*10^5 Pa = 101.325 kPa = 1.01325 bar

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17
Q

What are the 4 variables needed to define the state of a gas?

A

temperature (T) | pressure (P) | volume (V) | amount of gas in moles (n)

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18
Q

What does Boyle’s Volume-Pressure relationship state?

A

volume (V) inversely proportional to pressure (P) @ constant T and n

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19
Q

What does Jacques Charles’ Volume-Temperature relationship state?

A

volume(V) directly proportional to temperature(T)

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20
Q

who is William Thomson?

A

aka: Lord Kelvin = Kelvin scale

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21
Q

What was Guy-Lussac’s law of combining volumes?

A

pressure(P) and temperature(T) are directly proportional

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22
Q

What does Avogadro’s Law state?

A

volume(V) of a gas is directly proportional to the number of moles (n) of the gas at constant T and P

23
Q

What was Avogadro’s hypothesis?

A

equal volumes of gases at the same temperature contain equal numbers of molecules

24
Q

What is an ideal gas?

A

hypothetical gas whose pressure, volume, and temperature relationships are described completely by the ideal-gas equation

25
Q

What is the ideal gas law?

A

PV = nRT

26
Q

What is the gas constant and its value?

A

R = 0.08206 L.atm/mol.K

27
Q

What are 2 assumptions made when deriving the ideal-gas equation?

A

ideal gas molecules don’t interact with one another | combined volume of the molecules is smaller than the container volume

28
Q

What does STP stand for?

A

standard temperature and standard pressure

29
Q

What are the conditions for STP?

A

P = 1 atm | T = 273 K (0 degC)

30
Q

What is molar volume?

A

volume occupied by 1 mol of ideal gas at STP

31
Q

What is the value of the molar volume?

A

22.41

32
Q

What is Dalton’s law of partial pressures?

A

total pressure of a gas mixture = the sum of the pressures that each would exert alone

33
Q

What is partial pressure?

A

pressure exerted by a gas in a gas mixture

34
Q

What is mole fractions?

A

dimensionless number | expresses the ratio of the #moles of a gas in a gas mixture to the total #moles of the mixture

35
Q

What is the kinetic molecular theory of gases?

A

model that depicts what happens to gas particles when conditions (temp, pressure, or volume) change

36
Q

Who developed the kinetic molecular theory of gases?

A

Rudolf Clausius

37
Q

What are the 5 things that summarize the theory of moving molecules?

A

random motion | negligible molecular volume | negligible forces | constant average kinetic energy | average kinetic energy proportional to temp(T)

38
Q

What is random motion?

A

gases consist of large numbers of particles that are in continuous random motion

39
Q

What is negligible molecular volume?

A

combined volume of all gas particles is negligible relative to the container that holds these gases

40
Q

Why are forces negligible in the theory of moving molecules?

A

attractive and repulsive forces between particles are negligible

41
Q

What is constant average kinetic energy?

A

energy can be transferred between particles during collisions as long as temp(T) is constant

42
Q

What is the average kinetic energy proportional to temperature?

A

avg KE of the particles is proportional to the absolute temp = @given T = particles of all gases have the same avg KE

43
Q

What is most probable speed µ(mp)?

A

molecular speed measured by the largest total of particles

44
Q

What is root-mean-squared speed µ(rms)?

A

speed of a particle whose KE is equal to the avg. (mean) KE of all gas particles

45
Q

What is average (mean) speed µ(av)?

A

the average (mean) speed of all particles

46
Q

What are the 2 applications of the kinetic molecular theory to the Gas Laws?

A

Boyle’s Law (V and P are inverse) at constant T = constant KE = constant µ(rms) | Guy-Lussac’s Law (T and P are direct) at constant V = increase KE = increase µ(rms)

47
Q

What is effusion of gas particles?

A

escape of gas particles through a tiny hole

48
Q

What is diffusion of gas particles?

A

spread of gas A throughout gas B or space

49
Q

What is Graham’s Law of Effusion?

A

effusion rate of a gas is inversely proportional to the sqrt of its molar masses

50
Q

Who developed Graham’s Law?

A

Thomas Graham

51
Q

What is mean free path?

A

average distance traveled by a molecule in between collisions

52
Q

What is a short mean free path?

A

high pressure = crowded space

53
Q

What is a long mean free path?

A

low pressure = empty space

54
Q

What does van der Waals equation state?

A

takes into account the attraction of gas particles to each other and the finite volume

Chemistry R120 (18 decks)

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