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Chemistry 1203 > Test 3 > Flashcards

Test 3 Flashcards

Chapters 7, 8, & 9

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1
Q

exothermic

A

a process or reaction that gives off heat

change of heat < 0

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2
Q

endothermic

A

a process or reaction to which heat is added

change of heat > 0

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3
Q
  1. gases consist of molecules that are in constant, rapid, straight-line motion; different molecules can move at different speeds but the average speed will not change as long as the temperature does not.
  2. the average kinetic energy of the gas molecules depends only upon the temperature and it is directly proportional to the Kelvin temperature
  3. gas molecules interact only when they collide with one another, otherwise there are no forces between gas molecules
  4. gas molecules are very small compared to the distance between gas molecules; a gas is mostly empty space
  5. the force of gas molecules hitting the sides of its container create a pressure on the sides of the container
    NOTE: there are forces fo attraction between the molecules of a real gas
    gas to liquid : decrease temperature, decrease volume, increases pressure
A

The Kinetic - Molecular Theory

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4
Q

pressure definition

A

the force exerted by the gas on a given area of the container wall divides by that area
=(force)/(area)

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5
Q

pressure units

A

atmospheres - atm

millimeters of mercury - mmHg

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6
Q

1 atm =

A

760 mmHg

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7
Q

1 Torr =

A

1 mmHg

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8
Q

atmospheric pressure definition

A

the amount of pressure exerted by the weight of the atmosphere above us on a normal day

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9
Q

barometer

A

measures atmospheric pressure

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10
Q

ideal gas definition

A

a gas that would behave according to Boyle’s law, Charles’ law, and Gay-Lussac’s law and would follow the ideal gas law exactly (no such thing exists)

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11
Q

ideal gas law

A

PV=nRT

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12
Q

Boyle’s Law

A

fixed number of moles at constant temperature increase gas pressure and decrease volume

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13
Q

Charles’ Law

A

fixed number of moles at constant pressure increase temperature and increase volume; decrease temperature and decrease volume

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14
Q

Gay-Lussac’s Law

A

fixed number o f moles at constant volume increase temperature and increase pressure; decrease temperature and decrease pressure

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15
Q

P

A

pressure of gas in atm

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16
Q

V

A

volume of gas in Liters

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17
Q

n

A

number of moles of gas

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18
Q

T

A

temperature of gas in Kelvin degrees

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19
Q

R

A

constant
=0.08205
(L)(atm)/(mole)(K)

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20
Q

Dalton’s law of Partial Pressures

A

an ideal mixture of ideal gases each gas exerts a partial pressure that is the same pressure that would exert if it were only 1 gas present

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21
Q

vapor pressure

A

if a liquid is allowed to evaporate in a closed container the evaporation will eventually stop, the container will have both liquid and gas which was evaporated from liquid; the partial pressure of the gas is referred to as the vapor pressure of a liquid always goes up as the temperature goes up

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22
Q

boiling point

A

the temperature at which the vapor pressure of the liquid equals the atmospheric pressure

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23
Q

normal boiling point

A

the temperature at which boiling occurs when atmospheric pressure is 1 atm

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24
Q

melting point

A

the temperature at which, upon heat, the solid will change to a liquid

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25
Q

freezing point

A

the temperature at which upon cooling, liquid changes to solid

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26
Q

heat of vaporization

A

the amount of heat needed to convert 1g of liquid to vapor, given temperature
unit: cal/g

27
Q

molar heat of vaporization

A

value is given for 1 mole of liquid unit

kcal/mol

28
Q

heat of fusion

A

the amount of heat required to convert 1g of solid into a liquid of the melting point

29
Q

molar heat of fusion

A

1 mole of solid unit is

kcal/mole

30
Q

sublimation

A

the conversion of a solid directly into a gas without the formation of a liquid (ex. dry ice)

31
Q

dynamic equilibrium

A

the amount of a liquid and a gas do not change; there is a constant interchange between liquid and gas in closed container

32
Q

solution

A

a homogeneous mixture of 2 or more substances at molecular level

33
Q

solvent

A

that which does the dissolving (usually a liquid)

34
Q

solute

A

that which is dissolved (liquid, gas, or solid)

35
Q

concentration

A

a measure of the amount of solute dissolved in a fixed amount of solvent (%m/v and molarity)

36
Q

solubility

A

a measure of the maximum amount of solute that can normally be dissolved in a fixed amount of solvent, at a given temperature

37
Q

saturated solution

A

a solution containing the maximum amount of solute that can normally be dissolved in a given amount of solvent

38
Q

unsaturated solution

A

a solution which contains an amount of solute less than that required to form a saturate solution

39
Q

miscible

A

if 2 liquids will dissolve in one another in any amoutn

40
Q

immiscible

A

if 2 liquids will not dissolve in one another

41
Q

hydrophilic

A

soluble in water

42
Q

hydrophobic

A

not soluble in water

43
Q

Principles Governing Solubility

A

attractions between solute molecules are similar in type and strength to attraction between solvent molecules
“like dissolves like”
polar solvents dissolve polar solutes
non polar solvents dissolve non polar solutes
polar substances do no readily form solutions with non polar substances

44
Q

the effects of pressure on solubility

A

only when the solute or solvent is a gas
the most important situation involves the solution of a gas in a liquid
as the pressure of the gas increases, its solubility in the liquid increases
doubling the pressure doubles the solubility, doubling the gas pressure allows us to dissolve twice as much gas

45
Q

percent weight/volume =

(%m/v)=

A

(mass of the solute in g) / (volume of solution in mL) x 100

do not need to know identity only mass
ALWAYS TRUE: always equal to t eh number of grams of solute in 100.0 mL of solution

46
Q

molarity =

M

A

(moles of solute) / (total value of solution in L)

do not need to know identity bc need to know moles

47
Q

strong electrolyte

A

a substance that dissociate completely not ions when dissolved(in H2O)
includes strong acids, strong bases, and all ionic compounds

48
Q

weak electrolyte

A

a molecular substance such that most of the dissolved molecules do not dissociate
includes: weak acids, weak bases, and water itself

49
Q

non electrolyte

A

a substance that does not dissociate at all

sugars, dextrose

50
Q

colligative properties

A

solution properties that depend on the concentration of solute particles but not upon their identity

51
Q

osmolarity definition

A

(moles of solute particles)/(volume of solution in L)
osmol/L or osm/L
goes up as solution volume goes down
goes down as solution volume goes up

52
Q

osmoles

A

number of moles of solute particles

53
Q

four important colligate properties

A

vapor pressure lowering
freezing point depression
boiling point elevation
osmosis

54
Q

osmosis

A

2 solutions which are separated by a membrane though which small solvent molecules(water) can pass but through which solute particles cannot pass
traveling form the solution f lower osmolarity to the solution of high osmolarity

55
Q

osmolarity calculation for 1 solute

A

(molarity) x (# of solute particles per formula unit)

56
Q

flow of osmolarity

A

water flows in the direction that ten to make the osmolarity the same on both sides
solution flows from hypo-osmotic solution to the hyper-osmotic solution

57
Q

osmotic membrane definition

A

water can pass through but solute particles cannot

58
Q

terms isotonic, hypertonic, and hypotonic when…

A

comparing a given solution to. physiological solution

59
Q

physiological solution

A

a solution with a milliosmolarity in the range of 280-310 mosmol/:; osmolarity of blood and cells falls within this range
IV solutions are described using these terms

60
Q

milliosmolarity =

A

osmolarity x 1000

61
Q

hypotonic

A

a solution with osmolarity less that that of a physiological solution

62
Q

isotonic

A

a solution with osmolarity equal to that of a physiological solution

63
Q

hypertonic

A

a solution with osmolarity greater than that of a physiological solution

Chemistry 1203 (5 decks)

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