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AP Chemistry > Chapter 10: Gases > Flashcards

Chapter 10: Gases Flashcards

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1
Q

substances that a liquids or solids under ordinary conditions can also exist in the gaseous state, often referred to as _______

A

vapors

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2
Q

gases differ from liquids and solids by? (4)

A
  1. expands to fits its containers
  2. highly compressible
  3. homogeneous mixtures
  4. individual molecules are relatively far apart
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3
Q

conveys the idea of a force, a push that tends to move something

A

pressure

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4
Q

P = F/A

A

pressure equation

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5
Q

gravity works w/ gases to creates ________ _______

A

atmospheric pressure

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6
Q

you can calculate the magnitude of atmospheric pressure F exerted by any object is the product of its mass x acceleration

A

F = ma

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7
Q

the SI unit for kg-m/s^2 is a ________

A

Newton

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8
Q

SI unit of pressure is 1. _______ given the name 2. _______

A
  1. N/m^2

2. pascal (Pa)

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9
Q

a related unit to the Pascal is the _____ which one equals to 105 Pa

A

bar

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10
Q

atmospheric pressure @ sea level is ______ Pa or 1 bar

A

105

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11
Q

who created the barometer?

A

Evangelista Torricelli

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12
Q

dish experiences the full force of the Earth’s atmosphere and the column of Hg tries to match it as to why it increases —> barometer increased, height of Hg column, amount of atmo pressing down on surface decreases

A

Torricelli’s argument about pressure

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13
Q

corresponds to the typical pressure @ sea level

A

standard atmospheric pressure

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14
Q

1.01325 x 10^5 Pa =

A

standard atmospheric pressure

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15
Q

standard atmospheric pressure defines common non-SI units used to express gas such as 1. _________ and 2. _______

A
  1. atmosphere (atm)

2. millimeters of mercury (mm Hg) or torr

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16
Q

operates like a barometer; sometimes used to measure gas pressures near atmospheric pressure; P (gas) = P (atm) + P (height)

A

manometer

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17
Q

120 in 120/80 in blood pressure

A

systolic pressure

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18
Q

80 in 120/80

A

diastolic pressure

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19
Q

reading gauge

A

systolic pressure

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20
Q

pressure reduced until blood flows freely

A

diastolic pressure

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21
Q

presence of abnormally high blood pressure greater than 140/90

A

hypertension

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22
Q

what are the 4 variables for the physical conditions of gas?

A
  1. pressure
  2. volume
  3. moles of gas (amount of gas)
  4. temperature
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23
Q

the laws expressed the effect of 1. ____ variable on 2. ______ w/ the remaining two variables held at 3. ________

A
  1. one
  2. volume
  3. constant
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24
Q

the volume of a fixed quantity of gas maintained @ constant temp is inversely proportional to the pressure

A

Boyle’s Law

25
Q

one gets smaller as the other gets larger

A

inversely proportional

26
Q

PV = constant

A

Boyle’s Law

27
Q

______ was the first to experiment with a variable systematically changed to determine the effect of the other

A

Boyle

28
Q

hot air balloons 1. ______ as it’s heated, a balloon will shrink as the 2. _____ is cooled

A
  1. expand

2. gas

29
Q

Pressure-Temperature relationship

A

Robert Boyle

30
Q

Temperature-Volume relationship

A

Jacques Charles

31
Q

the volume of a fixed amount of gas maintained at constant pressure is directly proportional to it’s absolute temp

A

Charles’s Law

32
Q

proposed the absolute temp scale and for what?

A

William Thomson, for Charles’ Law

33
Q

experimented on the properties of gas to try and better control lighter-than-air balloons observed the law of combining volumes

A

Joseph Louis Gay-Lussac

34
Q

@ a given temp and pressure, the volumes of gases that rect w/ one another are in ratio of small whole numbers (like empirical formulas?)

A

law of combing gases

35
Q

based on Gay-Lussac’s observations, = volumes of gases @ the same temp + pressure contain the same # of molecules

A

Avogadro’s Hypothesis

36
Q

follow fr. hypothesis: the volume of a gas maintained at constant temperature and pressure is directly proportional to the # of moles of the gas

A

Avogadro’s Law

37
Q

PV = nRT

A

ideal-gas equation

38
Q

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

A

ideal gas

39
Q

what is absolute temperature?

A

the Kelvin scale

40
Q

the term “R” in the ideal-gas equation

A

gas constant

41
Q

the gas constant is _________ on units of pressure, volume, moles of gas, and temperature

A

dependent

42
Q

temp in the ideal-gas equation must _______ be expressed as absolute temp

A

ALWAYS

43
Q

in the ideal-gas equation:

  1. pressure = ______
  2. volume = _______
  3. quantity of gas in ______
  4. temp in ______
A
  1. atm
  2. L
  3. moles
  4. Kelvin
44
Q

Product PV has units of energy, so units of __ can contain joules or calories

A

R

45
Q

in problems of ideal-gas equations, units of P, V, n, and T must ______ w/ the gas constant

A

agree

46
Q

0.08206 L-atm/mol-K

A

value of R for units of atm in pressure

47
Q

8.314 J/mol-K

A

value of R for units of Pa in pressure

48
Q

conditions 0 degrees C and 1 atm are referred to _______ _______ ________

A

standard temperature pressure (STP)

49
Q

22.41L can be seen as the ______ mass of an ideal-gas @ STP

A

molar

50
Q

measure V might ____ from PV = nRT

A

differ

51
Q

nRT are all constants so must be the product of ___

A

PV

52
Q

P and V can change values independently but when together, their product must be a ________

A

constant

53
Q

P1V1 / T1 = P2V2 / T2

A

combined gas law

54
Q

nM/V = PM/RT

A

the relationship b/w gas densities and molar mass

55
Q

M in the relationship is. . .

A

molar mass; # of grams in one mole of substance

56
Q

d = PM/RT

A

density of gas

57
Q

density of gas depends on (3)

A
  1. pressure
  2. molar mass
  3. temperature
58
Q

though gas forms homogeneous mixtures, a 1. ______ dense gas will lie above a 2. _____ dense gas in the absence of 3. _______

A
  1. less
  2. more
  3. mixing
59
Q

M = dRT/P

A

molar mass of a gas

AP Chemistry (10 decks)

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