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10th grade > Chem printed notes unit > Flashcards

Chem printed notes unit Flashcards

1
Q

The Kinetic Theory of Matter

A

all particles of matter are in motion

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2
Q

Kinetic theory of gases

A
  1. gases are tiny
  2. no definite volume and are independent
  3. move fast in a straight line and change direction in collision
  4. are elastic and don’t stick together
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3
Q

Kinetic energy are…

A

transferred but not lost

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4
Q

Gas pressure

A

collision of gas particles with each other and their container.

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5
Q

as collision increases

A

pressure increases

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6
Q

as temperature increases

A

pressure increases

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7
Q

altitude increases

A

atmospheric pressure decreases

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8
Q

As volume increases,

A

pressure decreases.

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9
Q

standard pressure

A

average pressure at sea level.

  • 1 atm
  • 760 mmHg
  • 101.3 kPa
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10
Q

Kelvin
(temperatureis the amt of kenetic energy)
KE is proportional to Kelvin

A

Celsius + 273

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11
Q

Kinetic Molecular theory about gases

A
  1. movement is straight
  2. motion is constant and random
  3. no attractive/repulsive forces among particles
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12
Q

Factors Affecting Gas Pressure

A
  1. as the amt of gas increases, pressure increases
  2. as volume decreases, pressure increases
  3. as temp increases, pressure increases
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13
Q

Boyle’s law

A

PV=PV

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14
Q

Charles’ law

A

v/t=v/t

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15
Q

Gay-Lussac’s Law

A

p/t=p/t

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16
Q

the combined gas law

A

pv/t=pv/t

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17
Q

Ideal gases

A

gases that follow the kinetic molecular theory/gas laws (ATM IS AT A CONSTANT)

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18
Q

Ideal Gas Law

A

PV=nRT

R= .0821, pressure is in atm

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19
Q

Dalton

A

Ptotal=P1+P2+P3

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20
Q

Diffusion

A

gas particles spread

21
Q

Effusion

Graham

A

gas escape through a small hole

22
Q

When will real gas deviate from ideal gas behavior

A
  • high pressure
  • low temp
  • high molar mass
  • polar molecules
23
Q

Intermolecular Forces (IM)

A

forces of attraction btw particles (more in solids)

24
Q

Flow

A

particles can slide past eachother (only gas and liquids)

25
Q

Compressible

A

liquid and gas but gas is more

26
Q

KE

A

gas has more and solid has least

27
Q

Viscosity:

A

inability to flow

28
Q

Evaporation

A

liquid to gas below boiling point. Particles must have enough KE to beat IM. Highest KE at surface. cools overall

29
Q

Evaporation in a closed container

A

after evaporation, particles will lose energy and become a liquid.

30
Q

Equilibrium

A

reaction ocuring at the same rate, dynamic process bc looks likes nothing is happening

31
Q

Vapor Pressure

A

pressure caused by evaporated particles in closed container. vapor can b measure in container

32
Q

As temp increases

A

pressure increases

33
Q

as im forces increases

A

vp decreases

34
Q

boiling

A

conversion throughout substance. In order to boil, vapor pressure=atm pressure. Temp remains constant. also occurs by lowering atm pressure

35
Q

normal boiling point

A

boiling at standard pressure (sea level)

36
Q

high atm

A

bp increases

37
Q

low atm

A

bp decreases

38
Q

Crystaline

A

solid particles arranged in a pattern

39
Q

Amorphous

A

no order in particle

40
Q

Ionic (metal and nonmetal)

A

positive and negative, stronger higher normal boiling point

41
Q

Molescular (nonmetal)

A

covalent bond, weaker IM

42
Q

Sublimation

A

solid to gas without liquid. occurs when vapor pressure is greater/equal to atm

43
Q

deposition

A

gas to solid without liquid

44
Q

VP of soild

A

is lower than vp of a liquid

45
Q

phase diagram

A

shows temp and pressurre

46
Q

liquid state more dense than solid

A

slant left

47
Q

Molarity (M)

A

Liters of solution on bottom

47
Q

Molarity

A

Liters of solution on bottom

48
Q

Molality (m)

A

Kg

10th grade (45 decks)

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