Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Physics > Solids, Liquids and Gases New > Flashcards

Solids, Liquids and Gases New Flashcards

You may prefer our related Brainscape-certified flashcards:
Physics 101 flashcards AP® Physics flashcards
1
Q

density definition

A

mass per unit volume of a material

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

density equation

A

ρ = m/V

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

why do gases have a lower density

A

particles in a gas are more spread out

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

method to measure density of a regular object

A
  1. Place the object on a digital balance and note down its mass
  2. Use either the ruler, Vernier callipers or micrometer to measure the object’s dimensions (width, height, length, radius) – the apparatus will depend on the size of the object
  3. Repeat these measurements and take an average of these readings before calculating the density
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

method to measure the density of irregular object

A
  1. Place the object on a digital balance and note down its mass
  2. Fill the eureka can with water up to a point just below the spout
  3. Place an empty measuring cylinder below its spout
  4. Carefully lower the object into the eureka can
  5. Measure the volume of the displaced water in the measuring cylinder
  6. Repeat these measurements and take an average before calculating the density
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

method to measure density of liquids

A
  1. Place an empty measuring cylinder on a digital balance and note down the mass
  2. Fill the cylinder with the liquid and note down the volume
  3. Note down the new reading on the digital balance
  4. Repeat these measurements and take an average before calculating the density
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

pressure

A

the concentration of a force or the force per unit area

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

pressure equation

A

P = F/A
A = cross sectional area

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

in what directions is pressure exerted by a fluid on a surface

A

all directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

pressure in a liquid formula

A

P = h x ρ x g

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

how are the particles in a solid packed and how do they move

A

-they are closely packed
-vibrate about fixed positions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

shape and volume of solids

A

-definite shape
-definite volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

how are the particles in a liquid and how do they move

A

-particles are closely packed
-particles can flow over one another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

shape and volume of liquids

A

-no definite shape - flow and take the shape of a container
-definite volume

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

how are the particles in a gas and how do they particles move

A

-particles are far apart
-particles move randomly in all directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

shape and volume of gases

A

-no definite shape- take the shape of the container
-no fixed volume - can expand to fill up an evacuated container

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

why are gases compressible

A

-large gaps between the particles
-easier to push the particles closer together than in solids or liquids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

arrangement of particles in solids, liquids and gases

A

-solids are in a regular pattern
-liquids and gases are randomly arranged

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

energy of particles in solid, liquids and gases

A

solids have low energy
liquids have greater energy
gases have the greatest energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what happens when a solid is heated to form a liquid

A

-thermal energy transfer take places and supplies the particles in the solid with energy in their kinetic store
-this breaks the rigid bonds(IMF)between the particles meaning they can now flow over each other

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what happens when a liquid is heated to form a gas

A

-thermal energy transfer takes place and supplies the particles on the surface of the liquid with energy in their kinetic store
-this removes the bonds between the particles meaning they can move about randomly and spread far apart

22
Q

what happens when there is an increase in kinetic energy in a system

A

-causes the temperature of the system to increase
-OR produces a change of state

23
Q

what does higher temperature mean in terms of molecules

A

higher average kinetic energy of the molecules

24
Q

method to investigate changes of state

A
  1. Place the ice cubes in the beaker (it should be about half full)
  2. Place the thermometer in the beaker
  3. Place the beaker on the tripod and gauze and slowly start to heat it using the bunsen burner
  4. As the beaker is heated, take regular temperature measurements (e.g. at one minute intervals)
  5. Continue this whilst the substance changes state (from solid to liquid)
25
Q

why does the temperature of a substance remain constant throughout a state shift when being heated

A

-heat energy being produced is used up in changing the state of matter and for breaking numerous bonds or attractive forces

26
Q

specific heat capacity

A

the amount of energy required to raise the temperature of 1kg of the substance by 1C per kg of mass (J/kgC)

27
Q

how does the temperature of an object with a lower SHC change compared to an object with a higher SHC

A

-lower SHC object will heat up and cool down quickly

28
Q

specific heat capacity of water

A

4200 J/kg C

29
Q

specific heat capacity of alumnium

A

910 J/kg C

30
Q

specific heat capacity of copper

A

390J/kg C

31
Q

factors affecting how much the temperature of a system increases

A

-mass of the substance heated
-type of material
-amount of energy put into the system in the form of thermal energy

32
Q

change in thermal energy of a substance equation

A

change in thermal energy = mass x specific heat capacity x change in temperature
ΔQ = m x c x ΔT

33
Q

method to investigate specific heat capacity

A
  1. Place the beaker on the digital balance and press ‘zero’
  2. Add approximately 250 ml of water and record the mass of the water using the digital balance
  3. Place the immersion heater and thermometer in the water
  4. Connect up the circuit as shown in the diagram, with the ammeter in series with the power supply and immersion heater, and the voltmeter in parallel with the immersion heater
  5. Record the initial temperature of the water at time 0 s
  6. Turn on the power supply, set it at approximately 10 V, and start the stopwatch
  7. Record the voltage from the voltmeter and the current from the ammeter
  8. Continue to record the temperature, voltage and current every 60 seconds for 10 minutes
  9. Repeat steps 2-8, replacing the beaker of water for the solid block of aluminium and starting with recording its mass using the digital balance
    -electrical energy = voltage x current x time
    -SHC = gradient (when straight line)of energy supplied = y and temperature x mass = x
34
Q

brownian motion

A

random motion of tiny particles in a fluid

35
Q

at what angle do is there a net force on a container containing gas

A

right angle

36
Q

why does a gas at concentration have a higher pressure

A

-more particles in a given area
-more frequent collisions with the container walls and a greater force
-higher force exerted per unit area

37
Q

absolute zero definition

A

the temperature at which the molecules in a substance have zero kinetic energy

38
Q

kelvin to celcius

A

θ/C = T/K - 273

39
Q

celcius to kelvin

A

T/K = θ/C +273

40
Q

what is a one degree increase in kelvin equal to in celcius

A

one degree increase in celcius

41
Q

what is the lowest possible value of kelvin

A
  1. cannot be negative
42
Q

relationship between temperature in kelvin and average KE of the molecules

A

proportional(directly)

43
Q

how does the pressure of a gas change when it is compressed and expands

A

compressed - increases pressure
expands - decreases the pressure

44
Q

why does gas have more pressure when it is in a lower volume

A

-particles travel the same speed, but the distance they travel is reduced when the container is smaller
-molecules hit walls of the container more frequently
-larger overall net force on the wall, increasing the pressure

45
Q

why does gas at an increased temperature have more pressure

A

collide with the walls more often, creating increase in pressure

46
Q

pressure law

A

pressure is directly proportional to temperature is the volume is constant

47
Q

relationship between the pressure and temperature of two gases

A

p1/T1 = p2/T2

48
Q

Boyle’s law

A

p x V = constant

49
Q

unit of pressure

A

pascals(newton metres)

50
Q

difference between pascals and joules(Nm)

A

pascals is newtons/metres, joules is newton x metres

51
Q

relationship between pressure and volume

A

pressure and volume are inversely proportional to each other

52
Q

relationship between the pressure and volume of two gases(Boyle’s law)

A

p1V1 = p2V2

Physics (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions