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Chem > chapter 7; Changes of State and the gas Laws > Flashcards

chapter 7; Changes of State and the gas Laws Flashcards

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1
Q

kinetic molecular view

A

describes behavior of gases at the molecular level

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2
Q

gaseous atoms and molecules are in constant motion, moving at […] speeds

A

high

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3
Q

greater speeds =

A

greater kinetic energy

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4
Q

gaseous atoms or molecules move in […] lines in […] directions, […] with walls of their container, and fill entire container

A

straight
random
collide

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5
Q

greater speeds = greater kinetic energy =

A

higher temperatures

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6
Q

gaseous atoms or molecules are […] apart from one another and have […] intermolecular forces of attraction

A

far
negligible

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7
Q

gases are […] giving them unique properties that are different from […] and […]

A

compressible
gases
liquids

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8
Q

gas particles collide with the walls of the container, creating […]

A

pressure

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9
Q

Pressure (P) =

A

force / area

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10
Q

1 atmosphere (atm) =

A

760 millimeters of mercury (mmHg) used in medicine
760 torr
14.70 pounds per square inch (psi) English unit for pressure
101,325 pascals (Pa)

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11
Q

at sea level, atmospheric pressure is how many atm

A

1 atm

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12
Q

higher altitudes =

A

Lower atmospheric pressure
- fewer molecules pressing down
- less oxygen per breath

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13
Q

why do people who climb mount Everest usually carry cylinders of oxygen with them

A

the decreased atmospheric pressure at high altitude means that less oxygen is inhaled with every breath. Cylinders of oxygen provide supplemental oxygen and at a higher pressure

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14
Q

what are the four variables that describe the macroscopic properties of a gas

A

pressure (P)
volume (V)
temperature (T) and
moles (n)

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15
Q

what is the pressure volume relationship (Boyle’s law)

A

pressure and volume are inversely proportional when n and T are constant

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16
Q

what is the volume temperature relationship (Charles’s law)

A

volume and temperature are directly proportional when n and P are constant

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17
Q

what is the pressure temperature relationship (Gay Lussac’s law)

A

pressure and temperature are directly proportional when n and V are constant, and T is given in kelvins

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18
Q

in a graph how is the Boyle’s law shown

A

(constant temperature)
- as volume increases pressure decreases
pressure vs 1/V
if inversely it is straight line with pressure increasing as 1/V

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19
Q

in a graph how is Charles’s law shown

A

(constant pressure)
- increase temperature so does the volume
proportional

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20
Q

in a graph how is Gay-Lussac’s law

A

(constant volume)
- as temperature increases there is increase in pressure

21
Q

what is the equation of Boyle’s law

A

PiVi = PfVf

22
Q

what is the equation of Charles’s Law

A

Vi/Ti = Vf/Tf
volume and temperature are directly proportional
tmp is given in kelvins

23
Q

convert celcius to kelvin

A

kelvin = celcius + 273

24
Q

what is the equation of gay-lussac’s law

A

Pi/Ti = Pf/Tf
pressure and temperature are directly proportional
T is in kelvins

25
Q

what is the combined gas law: pressure, volume, and temperature

A

PiVi/Ti = PfVf/Tf

26
Q

when is the combined gas law used

A

when there is a fixed amount of gas, n, and the variables P, V, and T are changing

27
Q

what is the volume mole relationship (Avogadro’s law)

A

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

28
Q

what is the equation of the volume-mole relationship (avogrado’s law) equation

A

Vi/ni= Vf/nf
constant pressure and temperature

29
Q

what is standard temperature and pressure (STP)

A

0 degrees Celsius
(273.15 K)
and 1 atm of pressure

30
Q

what is molar volume of a gas at STP

A

22.4 L

31
Q

one mole of any gas at […] degrees celsius and […] atm occupies a volume of […] L, known as the molar volume of a gas

A

0
1
22.4

32
Q

what is 1 mole = in L at STP

A

22.4L
1 mole = 22.4 L

33
Q

what is the density of a gas at STP equation

A

density = molar mass / molar volume (22.4 L/mol)

34
Q

example of density of helium

A

density (helium) = (4.00 g/mol) / (22.4 L/mol) = 0.179 g/L less dense then air

35
Q

what is the molar mass of air

A

28.8 g/mol
if divided by STP
28.8 g/mol / 22.4 L/mol
= 1.29 g/L

36
Q

when something is less dense than air does it float or sink

A

sink

37
Q

how many gases do gas mixtures contain

A

two or more

38
Q

what is daltons law of partial pressures

A
  • each gas in a mixture exerts a pressure independent of other gases, behaving as if it alone occupied the total volume
  • Dalton’s law states that the total pressure of a gas mixture is equal to the sum of the partial pressure of each gas in the mixture
39
Q

what Daltons Law of partial pressure equation

A

Ptotal = P1 +P2 + P3 + … Pn
P1, P2, P3 …, Pn are partial pressures of the gases in the mixture

40
Q

what is the percentage oxygen in the atmosphere

A

20.95%

41
Q

e.g.
at sea level (760 mmHg), the partial pressure of oxygen is)
+
on Mount Everest (400 mmHg) the partial pressure of oxygen

A

0.2096 x 760 mmHg = 159 mmHg
0.2096 is 20.95% of oxygen in the atmosphere divided by 100
+
0.2095 x 400 mmHg) the partial pressure of oxygen is 84 mmHg

42
Q

what does Henry’s law state

A

that the number of moles of gas, n, dissolved in a liquid is directly proportional to the partial pressure, P, of the gas

43
Q

what dissolved gases does blood serum contain

A

oxygen nitrogen, and carbon dioxide

44
Q

what is Henry laws equation

A

P = K subscript H C P=KHC (t is constant)

45
Q

what do the letters stand for in Henrys Law equation P = K subscript H C

A

P = the partial pressure of the gas
K subscript H = Henry’s constant which is unique for each gas
C = the concentration of the dissolved gas (mol/L)

46
Q

how to solve for concentration of the dissolved gas from Henry’s law P = K subscript H C

A

P/K subscript H = C

47
Q

Henry’s law shows that the moles of gas dissolved in solution are […] to the partial […] of the gas

A

proportional
pressure

48
Q

Is volume and temperature proportional

A

Yes, as temperature increases volume.

Chem (10 decks)

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