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AP Chemistry > Unit 5 > Flashcards

Unit 5 Flashcards

1
Q

Pressure

A

-force exerted per unit area as gas molecules strike surfaces around them
-how much exerted by gas sample depends on number of gas particles in a given volume
-fewer gas particles, lower total force exerted per unit area and lower the pressure

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2
Q

properties of gases

A

-gases expand to fill any space available
-all gases have low density(g/L)
-volume of a as changes dramatically with a change in pressure or temperature
-volume, pressure and temperature are interrelated for a particular mass of gas

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3
Q

millimeters of mercury/torr

A

-atmospheric pressure can support a column of mercury that is 760. mm high in barometer
-1mm Hg=1 torr

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4
Q

atmospheres(atm)

A

-average pressure at sea level
-1atm=760. mm Hg

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5
Q

pascal(Pa)

A

-SI unit of pressure
-1atm=101,300 Pa

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6
Q

kilopascals

A

-1atm=101.3 kPa

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7
Q

pounds per square inch(psi)

A

-measure of force per unit area
-1atm=14.7 psi

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8
Q

standard atmospheric pressure

A
  1. mm Hg = 760. torr = 1 atm = 101.3 kPa = 14.7 psi
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9
Q

Boyle’s Law

A

-inverse relationship between pressure and volume (T-temperature and n-amount of gas molecules constant)

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10
Q

volume vs. pressure

A

-as volume of gas sample decreases, gas molecules collide with surrounding surfaces more frequently, resulting in greater pressure

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11
Q

Charle’s Law (Volume and Temperature)

A

gases expand when heated decreasing density of gas

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12
Q

relationship between gas and temperature

A

-direct relationship as long as temperature is measured in kelvins

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13
Q

when temperature of gas increases, gas particles move faster

A

-collisions with the walls are more frequent and the force exerted with each collision greater
-only way for pressure(force per unit area) to remain constant is for the gas to occupy a larger volume so that collisions are less frequent and occur over a larger area

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14
Q

Charles Law expressed

A

-V1/T1=V2/T2
-V1 and T1 initial volume and temperature

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15
Q

at constant temperature

A

-volume occupied by a fixed mass of gas is inversely proportional to its pressure

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16
Q

Boyle’s law expressed

A

P1V1=P2V2
-P1 and V1 are initial pressure

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17
Q

Avogadro’s Law(amount in moles and volume)

A

-relationship between volume and number of moles is linear
-extrapolation to zero moles shows zero volume

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18
Q

when amount of gas in a sample increases at constant T and P

A

-its volume increases in direct proportion because the greater number of gas particles fill more space

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19
Q

Avogadro’s law expressed

A

V1/N1=V2/N2

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20
Q

celsius to kelvin

A

C+273=Kelvin

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21
Q

Gay-Lussac’s Law(Pressure and Temperature)

A

-if gas is contained in container, as kelvin temperature increases, pressure increases
-direct relationship
-volume held constant

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22
Q

Gay-Lussac’s law expressed

A

P1/T1=P2/T2

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23
Q

combined gas law(pressure, volume, and temperature)

A

-combines Boyle’s, Charles, and Gay-Lussac’s laws

24
Q

combined gas law expressed

A

P1V1/T1=P2V2/T2

25
Q

ideal gas law

A

-combination of Boyle’s, Charles, and Avogadro’s law

26
Q

ideal gas law expressed

A

PV=nRT

27
Q

R

A

ideal gas constant

28
Q

n

A

moles in mol

29
Q

P

A

pressure in atm

30
Q

T

A

temperature in K

31
Q

V

A

volume in L

32
Q

Partial Pressure(Pn)—> Dalton’s Law

A

Pressure due to an individual component of gas

33
Q

P-total equation

A
  • P-total= ntotal * RT/V
  • P-total= Pa + Pb + Pc …
34
Q

Mole fraction

A

-na / ntotal
-number of moles of a component in a mixture divided by total number in mixture

35
Q

Mole fraction equation

A

-Pa = XaPtotal

36
Q

Molar volume

A

-volume occupied by one mole of a substance

37
Q

Standard temperature and pressure (STP)

A

-for gases, molar volume is often specified at this (T=0 degrees Celsius and P=1.00 atm)
- 22.4 L

38
Q

Density equations

A

-Density = molar mass/ molar volume
- d=PM/RT

39
Q

Vapor pressure

A
  • gas mixture has partial pressure of H2O
  • directly proportional to temperature
40
Q

Postulates of Kinetic Molecular Theory(KMT)

A

-models a gas as a collection of particles (atoms or molecules) in constant motion
- single particle moves in straight line until it collides with another particle
-Postulates:
1. Size of particles is negligible small
2. Average kinetic energy of a particle is proportional to kelvin temperature
3. Collision of one particle with another (or with walls of its container) is completely elastic

41
Q

Size of particle is negligibly small

A

-KMT assumes particles have no volume, even if they have mass
-under normal conditions space between atoms or molecules in gas is very large compared to size of atoms or molecules

42
Q

Average kinetic energy of a particle is proportional to kelvin temperature

A

-motion of atoms or molecules in a gas is due to thermal energy, which distributes itself among particles in a gas
-some particles move faster than others at times, so there’s distribution of velocities
-higher temperature=faster overall motion and greater average kinetic energy

43
Q

Collision of one particle with another (or with walls of its container) is completely elastic

A

-when two particles collide, they may exchange energy p, but there’s no loss of energy

44
Q

Pressure defined

A

-P = F/A

45
Q

Relationship of V and P

A

-inversely proportional when T and number of particles constant
-Boyle’s Law
-decrease V forces gas particles to occupy less space and number of collisions with surrounding surfaces increase( increasing P)

46
Q

Relationship of V and T

A

-Charles’ Law
-directly proportional when n and P are constant
-when T increases, average speed and average kinetic energy of particles increase

47
Q

Relationship of V and n

A

-Avogadro’s law
-when T and P are constant, V is proportional to
=when number of particles in gas sample increases, number of collisions with surrounding surfaces increases
-Vgas directly proportional to number of molecules

48
Q

At given temperature…

A

-particles at different masses have same average kinetic energy

49
Q

Relationship of gas and partial pressure

A

-Dalton’s Law
-total pressure of gas is sum of partial pressure of its components
components of gas mixture act identically to and independently of one another

50
Q

temperature and molecular velocity

A

-in order for kinetic energy to e constant, V must decrease for heavier particles and increase for lighter particles
-KE = 1/2mv^2

51
Q

to keep Kinetic Energy constant…

A

-smaller molar mass = higher velocity

52
Q

Diffusion

A

-process by which gas molecules spread out in response to a concentration gradient
-heavier molecules diffuse more slowly than lighter molecules

53
Q

Effusion

A

-process by which gas escapes from a container into a vacuum through a small hole
-heavier molecules effuse more slowly than lighter molecules(at same temperature)

54
Q

Graham’s law of effusion

A

-rate of effusion inversely proportional to square root of molar mass of gas

55
Q

Gases behave ideally when both of the following are true:

A

-volume of the gas particles is small compared to the volume(empty space) between them
-attractions between gas particles are not significant

56
Q

Effect of Finite Volume of Gas Particles

A

-finite volume(actual size) of gas particles becomes important at high pressure because the volume of particles occupies a significant portion of total gas volume

57
Q

Intermolecular attractions are small in gases and do not matter much at:

A

-low pressures because the particles are too far apart for the attractions to have any effect
-high temperatures because the particles have a lot of kinetic energy and when two particles with high kinetic energies collide, a weak attraction between them does not affect collision

AP Chemistry (2 decks)

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