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Chemistry > Chapter 6 Gas > Flashcards

Chapter 6 Gas Flashcards

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1
Q

Properties of Gas

A 
A. Gases have an indefinite shape.
B. Gases have a low density
C. Gases are very compressible
D. Gases exert pressure equally in all
directions on the walls of a container.
E. Gases mix spontaneously and completely
with one or more other gases.
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2
Q

a gas consists of?

A

small particles that move rapidly in straight lines

- indefinite shape; mix spontaneously

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3
Q

compared to the volume of the container they occupy gas particles have?

A

very small volumes

- low density; compressibility

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4
Q

gas particles having essentially no attraction or repulsion towards one another means..

A

they colide frequently with each other and with the walls of the container, the ollisioins are perfectly “elastic”

  • no loss of energy
  • exert pressure in all direction
  • kinetic energy of gas particles affects the pressure/volume
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5
Q

the average kinetic energy (energy of motion) of the gas particles are?

A

directly proportional ot its absolute temperature

kelvin temperature

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6
Q

what are the 4 variables of the physical behaviors of gases

A

pressure P
volume V
temperature T
amount n

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7
Q

pressure

A

the force exerted by gas against the walls of the container

- atm; mm Hg: torr; pascal

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8
Q

volume V

A

the space occupied by the gas

- L; mL

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9
Q

temperature T

A

determines the kinetic enegy and rate of motion of the gas particles
- C; K

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10
Q

amount n

A

the quantity of gas present in a container

- g; moles

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11
Q

Pressure of A Gas

A

gas pressure is the force acting on a unit area
Pressure P = (Force/area)

  • pressure is indicated by Δh (mm) of Hg column
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12
Q

atmospheric pressure

A
  • pressure exerted by a column of air from the top of the atmosphere to the surface of the earth
  • about 1 atm at sea level
  • lower at high altitudes where the density of air is less
  • is affected by weather, being lower on a rainy day than on a sunny day
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13
Q

atmospheric pressure at sea level is about 1 atm = (mmHg, torr, psi, kPa)

A 
1 atm = 760 mmHg (exact)
1 atm = 760 torr
1 atm = 14.7 psi (lb/in.2
)
1 atm = 101.325 kPa (kiloPascals).
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14
Q

temperature
- the property of a gas is related to the kinetic energy (speed) of the gas particle, thus the absolute temperature kelvin

A

K = oC + 273.0

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15
Q

the volume of a gas is the

A

volume of the container it occupies

- L or mL

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16
Q

the property of a gas is related to?

A

the number of as particles in the same, NOT the nature of gas particles
- moles (av.#)

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17
Q

the 4 variable of a gas PVTn are interdependent

A

Any one variable can be determined by
measuring the other three.
In the laboratory, scientists often hold 2
variables constant and then observe how the
other 2 variables change with respect to each
other

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18
Q

Boyle’s law (for pressure and volume)

A 
• At constant temperature, the
pressure of a fixed amount of gas
increases, when the volume
decreases.
• At constant T and n, V of a gas is
inversely related to its P.
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19
Q

Boyle’s law formula

A

P1V1 = P2V2

Kinetic Molecular Theory: when the volume decreases, the
gas particles moves in smaller space, thus colliding more
often with the wall and exerting higher pressure.

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20
Q

Charle’s Law for temperature and volume

A 
At constant pressure
,
The volume of a fixed
amount of gas is directly
related to its Kelvin
temperature.
21
Q

Charles law formule

A

V1 = V2
__ ___
T1 T2

22
Q

Kinetic molecular theory of charles law

A

: As Tk increases, gas particles move
faster and collide more with the wall, thereby expanding the
volume of container until the inside pressure equals the
outside pressure.

23
Q

Avogradro’s law

for volume and moles of the gas

A 
At constant P and T,
the volume (v) of a gas is
directly related to the
number of moles
(
n) of gas
24
Q

avogrado’s law formula

A

V1 V2
__ = ___
n1 n2

25
Q

kinetic molecular theory of avogradro’s law

A

When the number of gas particles
increases, so does the number of collision on the wall,
thereby expanding the volume until the inside pressure
equals the outside pressure

26
Q

The ideal gas law formula

A

PV = nRT
universal gas constant
R = 0.0821 (atm-L/mol-K)

27
Q

Combined gas law

A

P1V1 P2V2
____ = _____
T1 T2

(nature of the gas does not matter)

28
Q

partial pressure

- the pressure of a gas in a mixture

A

at a given T, in a given container, the pressure of a
gas is the same with or without the presence of other
kinds of gas particle.
The partial pressure of a gas (in a mixture)
is the same as the pressure of the gas
if it were alone in the container

29
Q

Dalton’s Law of Partial Pressures

A

The total pressure exerted by gases in a mixture is the

sum of the partial pressures of those gases.

30
Q

physical states of matters

Gas

A

indefinite shape
indefinite volume
compressibility
low density g/L

31
Q

physical states of matter

liquid

A

indefinite shape
definite shape
not compressible
g/ml density

32
Q

physical states of matter solid

A

definite shape
definite volume
not compressible
density g/cm3

33
Q

Solid kinetic-molecular view

A

fixed, very close arrangement of particles
very strong interaction between particles
very slow movement of particles

34
Q

liquid kinetic-molecular view

A
  • random, close arrangement of particles
  • strong interaction between particles
  • moderate movement of particles
35
Q

gas kinetic-molecular view

A
  • random, far apart arrangement of particles
  • essentially none interaction between particles
  • very fast movement of particles
36
Q

inter-particle attraction in Liquid and Solid

- ionic compound

A

solid at Tr

  • smallest particles = ions
  • electrostatic attraction among cations and anions = ionic bonds (chemical bonds)
37
Q

Inter particle attraction in Liquid and solid

- covalent (molecular compounds)

A 
smallest particle = molecules
 attraction within molecule=
covalent bond (chemical bond)
 attraction between molecules =
intermolecular force (IMF)
38
Q

3 types of intermolecular force (IMF)

A 
polar covalent compounds
- dipole-dipole attraction
- hydrogen bonds
Nonpolar covalent compounds
- dispersion force
39
Q

dipole - dipole attraction

A

attractive forces between the
positive and negative “poles”
of different polar molecules.

40
Q

hydrogen bonds

A

A very strong Dipole-Dipole Force
found between or in molecules that
contain H-F, H-O, H-N bonds

41
Q

dispersion forces

A

weak attraction caused by temporary
dipoles that develop when electrons
are not distributed equally

42
Q

criteria’s for hydrogen bonds

A 
Hydrogen atoms that are
covalently bonded to F, O, and
N atoms only may participate in
hydrogen bonding.
• Similarly, the lone pairs on a F,
O, or N atom of another
molecule may participate in
hydrogen bonding.
• There are no exceptions to this
43
Q

London dispersion force

A
  • transient, weak attraction among non-polar molecules
    -LDF is transient
    and weak.
    Only at very 4.2 K
    (-268.8◦C), when He
    atoms move very
    slowly, attraction by
    LDF is strong
    enough to hold He
    atoms in the liquid
    state.
    The boiling point
    (condensation
    point) of He gas is
    4.2 K!
44
Q

Gas - imf

A
  • No IMF
    Gas to solid = deposition
    gas to liquid = condensation
45
Q

solid - imf

A

-High IMF
Solid to liquid = melting
solid to gas = sublimation

46
Q

liquid - imf

A
  • lower imf
    liquid to gas = vaporization
    liquid to solid = freezing`
47
Q

IMF heat absorbed

A

Sublimiation
melting
vaporization

48
Q

IMF heat released

A

deposition
freezing
condensation

Chemistry (17 decks)

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