Ap Chem Ch. 10-11 Flashcards
0
Q
Force(massXacceleration) acting on an object per unit area.
A
Pressure-
P=f/a
1
Q
4 properties of gases:
A
- expand to fill their containers
- highly compressible
- always mix homogeneous with other gases
- only occupy a small fraction of the actual volume of their container
- extremely low densities
2
Q
Weight of air per unit of area
A
Atmospheric pressure
3
Q
Pascals-SI units
A
1 Pa= 1 N/m^2
4
Q
Bar
A
1 bar= 10^5 Pa= 100 kPa
5
Q
Difference in the heights measured in mm(h) of two connected columns of mercury
A
mm Hg , torr
6
Q
Normal atmospheric pressure at sea level
A
Standard pressure
7
Q
Convertions for standard pressure
A
1 atm = 760 torr = 760 mm Hg = 101.325 kPa
8
Q
Volume is _________ proportional to Pressure.
A
Inversly
P1V2=P2V2
9
Q
Voulme is ___________ proportional to temperature
A
Directly
10
Q
The volume of a gas at constant temperature and pressure is _________ proportional to the number of moles of the gas.
A
Directly
11
Q
Pressure is ________ proportional to kelvin temperature.
A
Directly
12
Q
Charles’ law
A
V1 V2
➖ = ➖
T2 T2
13
Q
Boyle’s law
A
P1V2=P2V2
14
Q
Gay-lussac’ law
A
P1 P2
➖ = ➖
T2 T2
15
Q
The product of the pressure and volume of a fixed quantity of gas is ______ proportional to the kelvin temperature.
A
Directly
16
Q
Conbined gas law
A
P1V1 P2V2
➖➖ = ➖➖
T1 T2
17
Q
Ideal gas law:
A
PV=nRT
18
Q
Constants for R( ideal gas constant)
A
.08206 L(atm) / mol( k)
- 314 L(kPa) / mol(k)
- 36 L(mm Hg) / mol(k)
- 314 J / mol(k)
19
Q
Solving for the volume of 1 MOL at standard temperature and pressure (STP) gives 22.41 L / mol
A
Standard molar volume
20
Q
Molar mass form of ideal gas law
A
M= mRT
——
PV
21
Q
Density form of the idal gas law
A
D= MP
—–
RT
22
Q
In which cases would you know you have to use Gas stoichiometry ?
A
- they have to be at constant pressure and temperature
* look for an equation
23
Q
The total pressure of a mixture of gases equals the sum of the pressures that each would exert if it were present alone.
A
Dalton’s law of partial pressures
P(total)= P1+P2+P3…
24
Gases consist of large numbers of molecules that are in continuous, random ______.
Motion
25
The speed of a molecule possessing AVERAGE KINETIC ENERGY.
Root-mean-square speed
26
The escape of gas molecules through a tiny hole into an evacuated space.
Effusion
27
The spread of one substance throughout a space or throughout a second substance.
Diffusion
28
Which diffuse faster, lighter molecules or heavier molecules??
Lighter molecules
29
Distance between collisions
Mean free path
30
Root-mean-square speed equation
______
u= \| 3rT
----
M
31
Properties of solids
- Definite shape and volume
- ordered arrangement
- fixed positions
- virtually incompressible
- Diffusion occurs extreamly slowly
- close together
32
Properties of liquids
- Definite volume, but takes shape of container
- disorder
- virtually incompressible
- Flows readily
- diffusion occurs slowly
- particles close together
33
The state a substance is in at a particular temperature and pressure depends on the balance of 2 antagonistic entities:
- The kinetic energy of the particles
| - the strength of the attractions between particles
34
Attractions BETWEEN molecules.
| Weaker!
Intermolecular forces
35
Attraction WITHIN molecules
| Stronger!
Intramolecular forces
36
However intermolecular forces are able to control physical properties such as:
- boiling point
- melting point
- vapor pressures
- viscosities
37
The intermolecular forces that exist between NEUTRAL molecules.
Van Der Waals forces
38
Examples of van der waals forces from weakest to strongest
1. London didpersion forces
2. Dipole-Dipole interactions
3. Hydrogen bonding
39
Other electrostatic attractions, polar molecule to ion attraction.
These are important in solutions of ions
Ion-Dipole
40
Other electrostatic attractions, ion to ion bonding
Ionic Bonding
41
Molecules that have permanent _______ are attracted to each other.
Dipoles
42
The ______ end of one dipole is attracted to the _____ of the other and vice-versa.
Positive
| Negative
43
The more polar the molecule, the _______ is its melting point.
Higher
44
Attractions between an instantaneous dipole( uneven dispersion of electrons ) and an induced dipole.
-these forces are present in all molecules, whether they are polar or nonpolar
London dispersion forces.
45
The ease in which an electron colud can be deformed
Polarizability
46
The _______ of a molecule affects the strength of dispersion forces.
Shape
47
Larger atoms have larger electron clouds which are easier to _________.
Polarize
48
If two molecules are of comparable size, __________ interactions are probably the dominating force.
Dipole-dipole
49
If one molecule is much larger than another, _______ forces will likely determine its physical properties.
dispersion
50
Dipole-dipole interactions where H is bonded to N,O, or F
Hydrogen bonding
51
Hydrogen bonding arises in part from the high _____________ of nitrogen, oxygen ,and fluorine.
Electronegativity
52
Hydrogen bonding also arises when hydrogen is bonded to the very electronegative elements, the hydrogen nucleous is _____.
Exposed
53
Resistance of a liquid to flow.
Vsicosity
54
As intermolecular forces increases, viscosity _______.
Increases
55
Increase in temperature will _______ surface tension
Decrease
56
The greater the intermolecular forces, the ________ the surface tension.
Greater
57
Intermolecular forces that bond similar molecules to one another.
Cohesive forces
58
Intermolecular forces between a substance and a different surface
Adhesive forces
59
The greateradhesive forces allow water to be drawn up the narrow tube.
Capillary action
60
Energy required to change a solid at it's melting point to a liquid.
Heat of fusion
61
Energy required to change a liquid at it's boiling point to a gas
Heat of vaporization
62
Why is vaporization larger than fusion?
Breaks intermolecular forces completely
63
The stronger __________ the more energy you have to take to change states.
Intermolecular forces
64
Energy needed to vaporize 1 mole of a liquid.
Molar heat of vaporization
| = 40.7 kJ/ mol
65
Energy that must be removed to condense 1 mole of a gas
Molar heat of condensation.
| =-40.7 kJ/mol
66
Energy needed to melt 1 mole of a substance.
Molar heat of fusion
| = 6.01 kJ/mol
67
Energy that must be removed to freeze 1 mole of a substance.
Molar heat of solidification
| =-6.01 kJ/mol
68
What does adding heat to a system at the melting and boiling points result in?
Results in pulling the molecules farther apart from each other.
69
Kinetic energy is spent as ________ in state changes.
Potential energy
70
If kinetic energy is constant while changing states, so is _______
Temperature
71
What equation is used to calculate state changes when KE and temp. Are constant.
q= (
72
Energy while in a single state equation
q= (m)(c)(
73
Highest temperature that a liquid phase can form.
Critical Temperature
74
Pressure needed to cause liquefaction at the critical temperature.
Critical pressure
75
Weaker forces ➡️ ________ critical points
Lower
76
As more molecules escape the liquid, the pressure they exert _______.
Increases
77
In a closed system, the liquid and vapor reach a state in ehich liquid molecules evaporate and vapor molecules condense at the same rate.
Dynamic equilibrium
78
The temperature of a liquid at which it's vapor pressure equals atmospheric pressure.
The boiling point
79
The temperature at which a substance vapor pressure is 760 torr.
Normal boiling point
80
The point in which all three states are in equilibrium
Triple point
81
Above critical temperature and critical pressure the liquid and vapor are indistinguishable from each other.
Critical point
82
Solids in which particles are in highly ordered arrangement
Crystalline
83
Solids in which there is no particular order in the arrangement of particles.
Amorphus
