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GCSE Physics > Particle Model of Matter > Flashcards

Particle Model of Matter Flashcards

1
Q

What is density defined as?

A

The mass per unit volume of a material

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2
Q

How do objects made from low density materials compare in mass to those made from high density materials?

A

Objects made from low density materials typically have a low mass, while similarly sized objects made from high density materials have a high mass

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3
Q

What is an example of a comparison between two objects of different densities?

A

A bag full of feathers is lighter than a similar bag full of metal

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4
Q

What is the relationship between density, mass, and volume?

A

Density is related to mass and volume by the equation: density = mass/volume

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5
Q

What are the units of density if mass is measured in grams and volume in cubic centimeters?

A

g/cm3

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6
Q

What are the units of density if mass is measured in kilograms and volume in cubic meters?

A

kg/m3

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7
Q

What happens to an object that is more dense than water?

A

It will sink

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8
Q

How do gases compare in density to solids?

A

Gases are less dense than solids because the molecules are more spread out

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9
Q

What is the typical density of a gas compared to a solid or liquid?

A

The density of a gas is typically around one-thousandth (1/1000) of the density of a solid or liquid

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10
Q

What is the density of water?

A

1000 kg/m3

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11
Q

What is the density of air at sea level and room temperature?

A

1.3 kg/m3

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12
Q

What is the particle model?

A

A model that describes the arrangement and movement of particles in a substance

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13
Q

What are the three states of matter?

A

Solid, liquid, gas

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14
Q

Describe the arrangement of particles in a solid.

A

The particles are closely packed and vibrate about fixed positions

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15
Q

Describe the arrangement of particles in a liquid.

A

The particles are closely packed but can flow over one another

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16
Q

Describe the arrangement of particles in a gas.

A

The particles are far apart and move randomly

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17
Q

How does the density of solids and liquids compare?

A

The density of solids and liquids are roughly the same because their molecules are tightly packed

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18
Q

What is the equipment resolution for a digital balance?

A

0.01 g

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19
Q

What is the aim of Experiment 1 in measuring density?

A

To determine the densities of regular objects by using measurements of their dimensions

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20
Q

What is the independent variable in measuring the density of irregularly shaped objects?

A

Different irregular shapes / mass

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21
Q

In changes of state, what happens to the number of molecules in a substance?

A

The number of molecules does not change

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22
Q

What is melting?

A

A solid turns into a liquid when energy is transferred to the system

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23
Q

What is boiling?

A

A liquid turns into a gas when energy is transferred to the system

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24
Q

What is condensing?

A

A gas turns into a liquid when energy is transferred away from the system

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25
What is freezing?
A liquid turns into a solid when energy is transferred away from the system
26
What is subliming?
A solid turns into a gas when energy is transferred to the system
27
True or False: The mass of a substance changes when it undergoes a physical change.
False
28
What should you do to minimize random errors in density measurements?
Take repeat readings and calculate an average
29
What is a common misconception about changes of state?
That the molecules themselves melt and separate
30
What is internal energy?
The total energy stored inside a system by the particles that make up the system due to their motion and positions.
31
What are the two types of energy that contribute to internal energy?
* Kinetic store (due to their random motion / vibration) * Potential store (due to their position relative to each other)
32
How does heating a system affect a substance's internal energy?
It increases the kinetic energy of its particles.
33
What is the relationship between temperature and kinetic energy of molecules?
The temperature of the material is related to the average kinetic energy of the molecules.
34
What happens to the kinetic energy during a change of state?
The kinetic energy remains the same while the potential energy increases.
35
What does the specific heat capacity of a substance indicate?
The amount of energy required to raise the temperature of 1 kg of the substance by 1 °C.
36
What is the equation for calculating the change in energy due to temperature change?
ΔE = mcΔθ
37
What does each variable represent in the specific heat capacity equation ΔE = mcΔθ?
* ΔE = change in energy, in joules (J) * m = mass, in kilograms (kg) * c = specific heat capacity, in joules per kilogram per degree Celsius (J/kg °C) * Δθ = change in temperature, in degrees Celsius (°C)
38
How does specific heat capacity affect the heating and cooling of substances?
* Low specific heat capacity: Heats up and cools down quickly * High specific heat capacity: Heats up and cools down slowly
39
What is latent heat?
The energy needed for a substance to change state.
40
What happens to temperature during a change of state?
The temperature remains constant despite energy being transferred.
41
What are the two types of latent heat?
* Latent heat of fusion * Latent heat of vaporisation
42
What is specific latent heat?
The amount of energy required to change the state of 1 kg of a substance with no change in temperature.
43
What is the specific latent heat of fusion?
The energy required to convert 1 kg of a substance between a solid and liquid state with no change in temperature.
44
What is the specific latent heat of vaporisation?
The energy required to convert 1 kg between a liquid and gaseous state with no change in temperature.
45
What is the equation for calculating the energy required for a change in state?
E = mL
46
What does each variable represent in the equation E = mL?
* E = thermal energy required for a change in state, in joules (J) * m = mass, in kilograms (kg) * L = specific latent heat, in joules per kilogram (J/kg)
47
What are the specific latent heat values for water?
* Specific latent heat of fusion = 330 kJ/kg * Specific latent heat of vaporisation = 2.26 MJ/kg
48
True or False: The latent heat of vaporisation requires less energy than the latent heat of fusion.
False
49
Fill in the blank: The _______ is the amount of energy needed per kg for all the particles in the substance to overcome intermolecular forces of attraction.
latent heat
50
What is the specific latent heat of fusion for water?
330 kJ/kg
51
What is the specific latent heat of vaporisation for water?
2.26 MJ/kg
52
How much more energy is required to evaporate 1 kg of water compared to melting the same amount of ice?
Roughly seven times more energy
53
What is the formula used to calculate the energy transferred during a change of state?
E = mL
54
In the formula E = mL, what does 'm' represent?
Mass of the substance
55
In the formula E = mL, what does 'L' represent?
Specific latent heat
56
Calculate the energy transferred to the surroundings when 0.60 kg of stearic acid changes from liquid to solid, given the specific latent heat of fusion is 199 000 J/kg.
119 400 J
57
What happens to the temperature of a solid when energy is transferred to it?
The temperature increases as the particles gain kinetic energy
58
What occurs at the melting point of a substance?
Energy is used to overcome intermolecular forces, and temperature stops increasing
59
What is the process called when a liquid turns into a gas?
Evaporation or vaporisation
60
What happens to the temperature of a gas when energy is transferred away from it?
The temperature decreases as the particles lose kinetic energy
61
What is the term for the process of a gas turning into a liquid?
Condensation
62
When energy is transferred away from a liquid, what happens to its temperature?
The temperature starts to decrease
63
What is freezing in terms of energy transfer?
A liquid turning back into a solid as energy is transferred away
64
What does the section from ORIGIN to A on a heating/cooling graph represent?
Energy used to increase the kinetic energy of particles while solid
65
What does the section A to B on a heating/cooling graph represent?
Energy used to overcome intermolecular forces, melting the substance
66
What does the section B to C on a heating/cooling graph represent?
Energy used to increase the kinetic energy of particles while liquid
67
What does the section C to D on a heating/cooling graph represent?
Energy used to overcome intermolecular forces, boiling the substance
68
What is the definition of specific heat capacity?
The amount of heat energy required to raise the temperature of a substance by a certain amount
69
What is the difference between specific heat capacity and specific latent heat?
Specific heat capacity changes temperature without changing state; specific latent heat causes a change of state at constant temperature
70
Fill in the blank: Specific latent heat is the amount of heat energy needed to cause a _______.
Change of state
71
True or False: Specific heat capacity and specific latent heat are the same.
False
72
What is the relationship between temperature and average kinetic energy in a gas?
The hotter the gas, the higher the average kinetic energy; the cooler the gas, the lower the average kinetic energy.
73
What is Brownian motion?
The random motion of tiny particles in a fluid.
74
How does temperature affect the speed of gas molecules?
As the temperature of a gas increases, the average speed of the molecules also increases.
75
What is pressure defined as?
Pressure is defined as the force exerted per unit area of the container.
76
What happens to pressure when a gas is heated at constant volume?
An increase in temperature increases the pressure due to more collisions with the container walls.
77
What is the effect of compressing a gas on its pressure and volume?
Compressing a gas decreases its volume and increases its pressure.
78
What is Boyle's Law?
For a fixed mass of gas at constant temperature, pV = constant.
79
Fill in the blank: When the volume decreases, the pressure _______.
increases.
80
What happens to pressure when a gas expands?
Expansion increases the volume and decreases the pressure.
81
What is the equation to compare initial and final pressure and volume in a gas?
P1 V1 = P2 V2.
82
What is the key assumption when applying Boyle's Law?
The mass and temperature of the gas must remain constant.
83
How does doing work on a gas affect its internal energy?
It increases its internal energy and can also cause an increase in temperature.
84
What happens to the temperature of a gas when it is allowed to expand?
The gas loses energy, resulting in a decrease in temperature.
85
Give an example of doing work on a gas that leads to an increase in temperature.
A bicycle pump.
86
True or False: When work is done on a gas, the temperature rises.
True.
87
What occurs when pressurized carbon dioxide is released from a high-pressure cylinder?
The gas does work, which can cause it to freeze, forming dry ice.
88
What is the relationship between pressure and the frequency of collisions in a gas?
A gas at high pressure has more frequent collisions on the container walls.
89
What happens to gas molecules when they collide with the walls of their container?
They exert pressure on the walls.
90
What is the effect of temperature on the kinetic energy of gas molecules at constant volume?
The kinetic energy increases as the temperature increases.
91
Fill in the blank: The pressure produced by a gas is a net force at _______ to the wall of the gas container.
right angles.
92
Explain the effect of decreasing the volume of a gas at constant temperature.
It increases the density of the gas, allowing more frequent collisions and increasing the pressure.
93
What must be checked after calculating pressure in a gas compression problem?
Ensure the final pressure is greater than the initial pressure.
94
What happens to the temperature of a gas when work is done by the gas?
The temperature falls.

GCSE Physics (9 decks)

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