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Chemistry > Gases > Flashcards

Gases Flashcards

1
Q

two factors that determine the state of a substance

A
  • the forces holding the particles tother
  • the kinetic energy of the particles
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2
Q

ionic forces

A
  • intramolecuclar
  • usually solid state
  • NaCl
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3
Q

Polar (dipole-dipole) forces

A
  • intermolecular
  • can be anything, usually liquid or gas
  • HCL (g)
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4
Q

Dispersion force

A
  • intermolecular
  • liquid or gas
  • CO2 (g)
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5
Q

What is the kinetic molecular theory?

A

all substances contain entities that are in constant motion

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6
Q

3 types of entity motion

A
  1. vibrational
  2. rotational
  3. translational
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7
Q

what particles have a vibration motion?

A

all particles

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8
Q

what particles have a rotational motion?

A
  • liquids
  • solids
  • some solids
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9
Q

what particles have a translational motion?

A
  • only in liquids and gases
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10
Q

temperature definition

A

a measure of the average kinetic energy of the entities of a substance

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11
Q

What is the kinetic molecular theory?

A
  • the volume of an individual gas moecule is negligible
  • there are no attractive nor repulsive forces between gas molecules
  • gas molecules move randomly in all directions, in straight lines
  • when gas molecules collide, they don’t loose kinetic energy
  • ideal gases, do not condense into liquids when cooled
  • the average kinetic energy of a gas molecule is directly related to the temperature. The greater the temperature, the greater the average motion of the molecules and the greater their kinetic energy
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12
Q

KMT describes a hypothetical gas called an ideal gas

A

i deal particles take up hardly any space

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13
Q

Who came up with kinetic molecular theory?

A

Robet Brown

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14
Q

pressure definition

A

the force exerted on an object per unit of surface area (P = F/A)

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15
Q

common SI unit of measurement of pressure

A

the pascal Pa = 1N/m^2

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16
Q

how is the pressure of a gas determined

A

by the kinetic moition

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17
Q

what device is used to measure pressure

A

a barometer

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18
Q

Describe the mercury barometer

A
  • a closed tube is filled with mercury, then inverted into a pan
  • gravity pulls the mercury downwards, but pressure pushes on the mercury in the pan, keeping it inside the tube
  • the result is that we can measure the height of the Hg( mm) in the tube as a measure of pressure
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19
Q

mass of atmosphere

A

5.1 * 10^18 kg

= 1000 kg over an area of 1 m^2

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20
Q

Why is there lower pressure the higher up in the atmosphere you are?

A

there is lass atmosphere above, less atmosphere pushing down

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21
Q

what is atmospheric pressure

A

the force exerted on Earth’s surface by a column of air over a given area (101 325 N/m^2). Pressure is exerted equally in all directions

22
Q

standard pressure and pressure at sea level

A

101.325 kPa

23
Q

One atmosphere = ________kPa

A

101.325

24
Q

STP

A

Standard Temperature and Pressure

at 0 degrees celsius and 101.325 kPa

25
Q

SATP

A

standard ambient temperature and pressure

at 25 degrees celsius and 100.00 kPa

26
Q

Why is SATP better than STP?

A

SATP more conveniently resembles lab conditions

27
Q

1 atm to ________ mmHg

A

650 mm Hg

28
Q

1 Torr = ________ mmHg

A

1

29
Q

psi = ________ Pa

A

6895

30
Q

Boyle’s Law

A

As pressure on a gas increases, the volume fo the gas decreases proportionally, if temperature and amount of gas (moles) remain constant.

31
Q

Boyle’s law equation

A

P1V1=P2V2

32
Q

Describe flying and pressure and ascending

A

as atmospheric pressure, decreases, the relative pressure inside the ear becomes hgiher and pushes out the eardrum

33
Q

Describe flying and pressure and descending

A

as atmospheric pressure increases, the relative pressure inside the ear decreases.

Large pressure differentials cuases pain and even a rupture of the eardrum

34
Q

Describe the creation of the celsius scale

A
  • Anders Celsius created the scale by taking a thin glass tube filled with mercury and recording the height of the liquid in ice cold water, repeated in boiling water
    divided distace between 2 heights in 100 divisions = 1 degree
35
Q

Charles’ Law

A

As the temperature of a gas increases, the volume increases proportionally when pressure and mount of gas remains constant

V1/T1 = V2/T2

36
Q

Gay-Lussac’s Law

A

the pressure of a fixed amount of gas, at a constant volume is directly proportional to its kelvin temperature

P1/T1 = P2/T2

37
Q

combined gas law

A

the product of the pressure and volume of gas divided by its absolute temperature is a constant as long as the amount of gas is kept constant

P1V1/T1 = P2V2/T2

38
Q

volume ratio

A

when measured at the same temperature and pressure, volumes of gaseous reactants and products of chemical reactions are always in simple ratios of whole numbers

39
Q

who came up with law of combining volumes

A

Joseph Gay-Lussac and Amedeo Avogadro

40
Q

Avogadro’s Law

A

the volume of a gas is directly proportional to the amount of gas, when temperature and pressure remain constat.

V1/n1 = V2//n2

41
Q

molar volume

A

the space that is occupied by one mole of gas

same for all gases

measured in L/mol

42
Q

what is molar volume of an ideal gas at STP?

A

22.4 L

43
Q

what is molar volume of an ideal gas at SATP?

A

24.8 L

44
Q

problems with real gas behaviours at high pressures and low temperature

A
  • in very smalll volumes there will be many more interactions and collisions
  • the volumes of the gas molecules is now a significant fraction of the container
45
Q

R

A

the universal gas constant

8.214 kPa *L/mol *K

46
Q

the ideal gas law

A

PV = nRT

47
Q

what is pressure caused by?

A

collisions with the walls of the container

48
Q

Dalton’s law of partial pressures

A

the total pressure of a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases

49
Q

atmospheric pressure

A

N2 = 78.08%
Ar = 0.93%
O2 = 20.95%
CO2 = 0.03%

= 101.3 kPa

50
Q
A

Chemistry (21 decks)

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