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Chemistry > Physical States Of Matter > Flashcards

Physical States Of Matter Flashcards

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1
Q

diffusion can happen in gas and liquids. T/F

A

True

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2
Q

what is diffusion?

A

the movement of molecules from a region of high concentration to the region of low concentration.

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3
Q

what is vacuum?

A

space devoid of matter.

devoid = lack

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4
Q

what is effusion?

A

escape of molecules through the hole one after the other without collision.

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5
Q

at any point, a gas exerts _______ pressure in ____ directions.

A

equal
all

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6
Q

what is pressure?

A

force per unit area.
force exerted by a gas on unit area of a container.

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7
Q

full form of atm?
what is atm?
1 atm=

A

atmosphere
unit for measuring the atmospheric pressure.
=760mm of Hg or 760 torr or 1.01325 x 10 5 Pa.

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8
Q

1kPa = ?Pa

A

1000 Pa

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9
Q

what is atmospheric pressure?

A

pressure exerted by air
1atm= 101,300 Pa

air pressure

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10
Q

what is compressibility?

A

the measure of how much a given volume of matter decreases when placed under pressure

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11
Q

the intermolecular space is ____________?

A

maximum in gases less in liquids and the least in solids.

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12
Q

why are gases highly compressible? and solid the least?

A

In gases the interparticle space is very large and hence they are compressible, but in case of solids and liquids particles are close to each other and hence cannot be compressed.
Solids are rigid and cannot be shaped and cannot be compressed.

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13
Q

why gases leak rapidly out of a hole?

A

this is due to the tendency of a gas to expand & fill the entire space available.

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14
Q

what is mobility?

A

Mobility is the ability of particles to move.

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15
Q

is mobility more in gases? why?

A

yes, mobility is maximum in gases as they have the least intermolecular force of attraction.

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16
Q

what is IMF?

A

are the attractive and repulsive forces that arise between the molecules of a substance.

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17
Q

density is ________ to volume.

A

indirectly proportional

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18
Q

density is ___________to mass.

A

directly proportional

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19
Q

when a gas is cooled its density _______________.

A

increases because its volume decreases.

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20
Q

gases have ______ densities under normal conditions.

A

low
less mass in a given volume.

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21
Q

the average kinetic energy of gas molecules is ________________ proportional to the Kelvin temperature.

A

directly

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22
Q

increasing the pressure of gas results in ___________ in volume.

A

decrease
becuase the distance b/w the molecules decreases.

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23
Q

when temp. of a gas is increased, the averge kinetic energy of gas molecules ___________.

A

increase
this causes internal pressure.
volume of gas increases

to restore constant pressure

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24
Q

explain why the volume of gas increases when temperature is increased at constant pressure?

A

to restore constant pressure
the pressure is 1 atm downward
1 atm should be upward but as pressure increase becuase of change in temp. that’s why the volume increases to reduce or restore pressure

as V∝1/P
T∝ P

25
Q

product of volume and pressure of gas is constant how????

A

V= 1/P X constant
V X P = constant

26
Q

unit of pressure and volume

A

pascal
dm3/m3

27
Q

state Boyle’s law?

A

the volume of fixed amount of gas at a given temperature is inversely proportional to the applied pressure.

28
Q

________ of volume & temp. of a gas is constant how?

A

ratio
V∝T
V = constant X T
V/T = constant

29
Q

temp. of a gas is ________ proportional to the volume.

A

directly

30
Q

1cm3= ? dm3

A

0.001 dm3

divide the volume value by 1000

31
Q

state Charles’s law?

A

the volume of a given mass of a gas varies directly with absolute temperature at constant pressure.
V∝ T

absolute temperature: temperature measured on the Kelvin scale.

32
Q

what are the conditions for Boyle’s and charles law?

A

boyles law: temp. constant
charles law: pressure constant

33
Q

name properties of gases?

A
  1. diffusion
  2. effusion
  3. mobility
  4. compressibility
  5. pressure
  6. density
34
Q

name properties of liquids?

A

evaporation
vapor pressure

35
Q

what is density?

A

it is the measure of how packed the material is with mass. It is defined as the mass of an object per unit volume.

How much mass a substance has, per unit its volume.

36
Q

liquid evaporate faster when heated. why?

A

added heat increases the kinetic energy of the molecules.

it’s more likely for a molecule to break away from the liquid to become a gas.

37
Q

what is vaporization?

A

conversion of a liquid into a gas or vapor at all temperatures.

aka evaporation

molecules break away and enter the vapor state. (greater kinetic energy)

38
Q

why when i put cold water in a glass, the glass forms dews?

A

When you pour cold water into a glass, the glass is typically cooler than the room’s air temperature. This temperature difference causes the air surrounding the glass to lose heat and cool down. As the warm, moist air comes into contact with the cold surface of the glass, it cools down as well. When the air reaches its dew point, it can no longer hold all the water vapor it contains, and condensation occurs.

39
Q

what is vapor pressure?

A

pressure exerted by the vapors of the liquid in equilibrium with its liquid.

40
Q

at equilibrium, the space above the liquid is saturated with ______________.

A

vapors

cz it’s in equilibrium

41
Q

temp. increase, vapor pressure _______________.

A

increase

more kinetic energy

more molecules gain the energy & enter the gas phase, leading to an increase in vapor pressure.

42
Q

when does the boiling of liquid starts?

A

when atm. pressure = vapor pressure

43
Q

boiling point of water? why?

A

100°C

at this temp. water converts to gas & starts boiling.

or vapor pressure becomes = atmospheric pressure which 101.325 kPa

44
Q

what is boiling point?

A

temp. at which vapor pressure of a liquid becomes equal to the external or atmospheric pressure.

45
Q

water boils at ________ temperature in higher altitudes?

A

lower

atmospheric pressure is lower so less vapor pressure temp. will make it equal to the atm pressure.

46
Q

pressure __________ with increasing altitude. why?

A

decreases
Gravity pulls the atmosphere toward the Earth’s surface, causing the majority of atmospheric mass to be concentrated closer to sea level.

As you ascend, there are less air molecules above you exerting pressure.

because the atmosphere is less dense at higher elevations.

47
Q

what is distillation?

A

process in which a liquid is heated to vaporize it and the vapors are cooled to condense them back to the liquid in a different container.

48
Q

what is melting point?

A

the temp. at which a solid turns into a liquid.

49
Q

freezing point is the reverse of ___________.

A

melting

50
Q

what is boiling point?

A

the temp. at which a liquid changes into the gas.

the temperature at which liquid starts to boil

temperature at which the vapor pressure of liquids becomes equal to its atmospheric pressure.

51
Q

melting point depends upon ____________?

A

strength of attractive forces that hold particles together.

52
Q

what is sublimation? examples?

A

phase change when solids on heating turn into gaseous state without passing through liquid state.

on heating= it’s endothermic

eg: iodine, benzonic acid, ammonium chloride

53
Q

what are the types of solids?
what are they based on?
examples?

A

2
crystalline solids: a solid composed of orderly repeating 3D arrangement of particles. sharp melting points.
amorphous solids: a solid that lack ordered arrangement of its particles. don’t melt at definite temp. but soften when heated

based on macrscopic appearence= arrangement of particles in solid

examples: NaCl
examples: glass, plastic

54
Q

what are allotropes?
chemical formula of all the allotropes of carbon?

A

the different forms of an element in the same physical state are called allotropes.
different arrangement of atoms.

the allotropes of carbon has only carbon element in it and thus has a chemical formula of C.

55
Q

name allotropes of carbon?
why is diamond hardest substance?
how are atoms arranged in graphite?
what makes graphite soft?
how are atoms arranged in bucky ball?

A

3 graphite diamond & buckey ball
carbon atom is bonded to 4 other atoms, creating a rigid compact array.
In graphite, carb atoms are arranged in layers of hexagonal arrays. weak bonds exist b/w the layers that allow them to slide over one another.
In bucky ball, 60 carbon atoms form a hollow sphere.

56
Q

allotropes of phosphorus?

A

red & white phosphorus
white phosphorus consist of tetraatomic molecules P4 that aren’t bonded to each other.
red phosphorus, molecules are bonded to one another in long chains.

Tetraatomic molecules: molecules composed of four atoms.
ammonia (NH₃)

57
Q

compare physical states of matter?
how can we differentiate b/w them?

A

by intermolecular forces present b/w their particles.

Gas: no attractive forces, so molecules move freely in all directions, no definite shape & volume.
Liquid: significant attractive forces exist b/w molecules of liquid. These forces keep molecules together. But these forces can’t hold molecules in fixed positions. So molecules in liquid slide past one another, definite volume but no definite shape.
Solids: strong attractive forces exist b/w particles. strong enough to hold particles in fixed positions. As a result, solid has definite shape as well as definite volume.

58
Q

how to find pressure at given temperature (boiling point)?

A

760/100 X given temp.

59
Q

if a subtance melting point is -17 degrees C what will happen at -18 & -16?

A

-18: solid, temp. is lower than its melting point. -18 is less than -17 & temp. lower than melting point, the substance remains solid.
-16: liquid, temp. is higher than its melting point.

Melting occurs when the temperature is equal to or higher than the melting point.

Chemistry (8 decks)

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